EXAM 1 - PREP

Question 1

(Q:1.1)What the definition of a Scientific Law?

A) A law is a number of similar observations generalized into a brief statement summarizing past observations and predicting new ones.

B) A law is the underlying reason for scientific theory

C) A law is a way of learning that emphasizes observation and experimentation

Answer 1

A) A law is a number of similar observations generalized into a brief statement summarizing past observations and predicting new ones.

LAWS PREDICT WHILE THEORIES TRY TO EXPLAIN

Question 2

what is kinetic energy definition?

Answer 2

kinetic energy is the energy of motion

Question 3

(Q:1.1)What is the definition of a scientific theory?

A) A brief statement that summarizes past observations and predicts future ones

B) It is a model that explains the underlying reasons for observations and laws

C) It is a method of learning that emphasizes reason as the way to understand the world

Answer 3

B)it is a model that explains the underlying reasons for observations and laws

THEORIES ATTEMPT TO EXPLAIN OBSERVATIONS

Question 4

(Q:1.1)Which of the following statements best describes the purpose of performing experiments?

A) Experiments are designed to produce the results predicted by a theory or hypothesis.

B) Experiments can be replaced by logical reasoning based on the known facts

Answer 4

A) Experiments are designed to produce the results predicted by a theory or hypothesis.

SCIENTIFIC METHOD IS A CYCLE AND RELIES ON OBSERVATIONS

Question 5

(Q:1.1)Which of the following would be considered a hypothesis?

A) Birds can fly because they have hollow bones

B) Spiders have eight legs

C) Fresh Lava from a volcano is hot

D) None of the choices can be considered a hypothesis

Answer 5

A) Birds can fly because they have hollow bones.
++BECAUSE EMPHASIZES AN ATTEMPT TO EXPLAIN IF THIS.. THEN THAT..
++A HYP IS TESTABLE AND TENTATIVE EXPLANATION FOR AN OBSERVATION

Question 6

(Q:1.1)Which of the statements below is NOT part of the Scientific method?

A) Observations and measurement

B) Formation of a hypothesis

C) Testing of a hypothesis by experimentation

D) Refinement of a hypothesis
as needed

E) All of the above steps are part of the scientific method

Answer 6

E) All of the above steps are part of the scientific method

Question 7

(Q:1.1)Which of the following is false?

A) Experiments can be used show that a theory is somewhat limited in scope.

B) A hypothesis which has successfully withstood many tests eventually can become a theory

C) In general, a theory can be proven to be absolutely true

Answer 7

C) In general, a theory can be proven to be absolutely true

Question 8

(Q1.1)TRUE OR FALSE: Science is the same as Technology?

Answer 8

FALSE

Question 9

(Q1.1)TRUE OR FALSE: There is much overlap between science and technology

Answer 9

TRUE

Question 10

(Q:1.1) Explain the similarities between a scientific Law and scientific theory as they relate to the scientific method:

Answer 10

A scientific Law and scientific theory are both based on the scientific foundation of observing and experimentation. They both trying to describe conditions that are happening based on information gathered. However a Law does not explain why, just the conditions for which a certain phenomenon is observed. A theory tries to predict and explain WHY.

Question 11

(PS:1)
“In the scientific method, a ______________ is a tentative interpretation, or an initial explanation.

Answer 11

Hypothesis

Question 12

(PS:1)
“___________________ are garnered from experiments in order to test an explanation or theory.”

Answer 12

Observations

Question 13

(PS:1) “You may be able to make a brief statement that will only predict a future event, this is called a ___________”

Answer 13

Law

Question 14

(PS:1) “It is possible that after enough testing and scrutiny, you have a well-supported explanation of a phenomenon that also makes predictions, this is called a ________________”

Answer 14

Theory

Question 15

(HW:1.1) Which of the following is NOT part of the scientific method?

A) observation and measurement

B) formation of a hypothesis

C) testing of a hypothesis by experimentation

D) refinement of a hypothesis as needed

E) All of the above are parts of the scientific method

Answer 15

E) All of the above are parts of the scientific method

Question 16

(H.W:1.1) Which Statement about the scientific method is TRUE?

A)The scientific method emphasizes reason as the way to understand the world

B)The scientific method emphasizes observations and experimentation as the way to understand the world

Answer 16

B) The scientific method emphasizes observations and experimentation as the way to understand the world

Question 17

(H.W:1.1) Which of the statements below can be classified as an observation?

A)The universe began as a cosmic explosion called the Big Bang

B) All Matter is made up of atoms

C) When wood is burned in a closed container, the mass of the container and its contents are the same before and after burning

Answer 17

C) When wood is burned in a closed container, the mass of the container and its contents are the same before and after burning.

Question 18

(HW:1.1)Which of the following statements best describes the purpose of performing experiments?

A) Experiments can be replaced by logical reasoning based on the known facts

B) Experiments attempt to produce other observations that support or refute a theory or hypothesis

Answer 18

A) Experiments can be replaced by logical reasoning based on the known facts

Question 19

(1.1) TRUE/FALSE All Leading Zeros are significant
i.e 000002.00

Answer 19

FALSE
leading zeroes are never sig figs

Question 20

(HW:1.1) What is the definition of a scientific theory?

A) It is a brief statement that summarizes past observations and predicts future ones.

B) It is a model that explains the underlying reasons for observations and laws

C) It is a method of learning that emphasizes reason as the way to understand the world.

Answer 20

B) It is a model that explains the underlying reasons for observations and laws

**A LAW PROVIDES PREDICTIONS BASED ON OBSERVATIONS. IT CAN PREDICT NEW OBSERVATIONS

Question 21

(HW:1.1) Which of the following items does NOT contain chemicals?

A) drain cleaner

B) organically grown vegetables

C) air

D) All of the above contain chemicals

Answer 21

D) all of the above contains chemicals

++ALL SUBSTANCES CONTAIN CHEMICALS BC ALL CONTAIN MASS = ATOMIC STRUCTURE

Question 22

(HW:1.1) Which of the following statements is true?

A) Nanotechnology employs devices that are generally greater than 100nm

B) Nanotechnology works with devices that are always less than 1 nm

C) Nanotechnology deals with dimensions that are less than 100nm

D) Nanotechnology deals with dimensions at any size

Answer 22

C) Nanotechnology deals with dimensions that are less than 100nm

Question 23

(HW:1.1) TRUE/FALSE Science is the pursuit of knowledge of the world around us, whereas technology is the application of scientific knowledge for practical purposes.

Answer 23

TRUE

Question 24

(1.1) TRUE/FALSE The Scientific method is a systematic approach to gaining knowledge

Answer 24

TRUE

Question 25

(1.1)"When wood is burned in a closed container, the mass of the container before burning remains the same after burning." Is an example of an _____________

Answer 25

Observation

Question 26

(1.1) "John's blue T-Shirt is blue because it reflects light." This is an example of ______________

Answer 26

Hypothesis

Question 27

(1.1) "When objects fall, they accelerate towards the earth's surface." This is an example of _______________

Answer 27

Law

Question 28

(1.1) TRUE/FALSE Experiments attempt to produce other observations that support or refute a theory or hypothesis.

Answer 28

TRUE

Question 29

(1.1) TRUE/FALSE A control experiment differs from a test experiment in only one variable.

Answer 29

TRUE

Question 30

(1.1)Nanotechnology is the understanding and control of matter at the _________. Nanotechnology deals with dimensions between approximately __________ and ___________ nanometers where unique phenomena enable novel applications.

Answer 30

Nanoscale....... 1...... 100

Question 31

(1.1)When a hypothesis is thoroughly ________. It may become a ___________.

Answer 31

Tested....Theory

Question 32

(1.2) How many SIG FIGS would be used in calculations with the measurement: 2.34m

Answer 32

3 SF in 2.34m

Question 33

(1.2) How many SF would be used in calculations with the measurement: 2.3467 x 10^6 in

Answer 33

5SF in 2.3467 x 10^6

Question 34

(1.2) How many SF would be used in calculations with the measurement: 44,200g

Answer 34

3SF in 44,200

Question 35

(1.2) How many SF would be used in calculations with the measurement: 0.003 L

Answer 35

1 SF in 0.003

Question 36

(1.3445 x 10^6)(9.385 x 10^-4) ------------------------- 12.3454 +84.23

Answer 36

13.07

Question 37

(1.2) Convert 2.34 x 10^-3 meters to kilometers

Answer 37

2.34 x 10^-6 km

Question 38

(1.2) Convert 0.00345km to μm

Answer 38

3.45 x 10^6 μm ( https://youtu.be/EwsCiRcNi3M)

Question 39

(1.2) Titanium is a metal used to make golf clubs. A rectangular bar of this metal measuring 1.84cm x 2.24 cm x 2.24 cm was found to have a mass of 45.7g. What is the density of the titanium in the g/cm3?

Answer 39

4.95 g/cm^3 (https://youtu.be/msjYwHzxDzQ )

Question 40

(1.2) What is the number 3606 expressed in scientific notation? A) 36.06 x 10^2 B) 3.606 x 10^3

Answer 40

C) 3.606 x 10^3

Question 41

(1.2) TRUE/FALSE The exponents in scientific notation must be positive if the number is greater than 1

Answer 41

TRUE

Question 42

(1.2)Complete the Base Units of the SI System : length: Meter (m) mass: _______ time: ________ temperature: __________ amount of substance: mole (mol)

Answer 42

mass: kilogram (kg) time: second (s) temperature: kelvin (K)

Question 43

(1.2) Complete the conversion map: 1 Gallon : ____ quarts 1 Quart : _____pints

Answer 43

4 quarts.... 1/2 (.5) pints...

Question 44

(1.2) Common unit prefixes: Kilo (k)

Answer 44

K 10^3 or 1000

Question 45

(1.2) Common unit prefixes: Nano (n)

Answer 45

n 10^-9 /9 places behind the decimal ie 4 nanograms = 0.000000004 g

Question 46

(1.2) Common unit prefixes: centi (c)

Answer 46

10^-2 ie. 7 cm is 0.07m

Question 47

(1.2) Common unit prefixes: micro (µ)

Answer 47

10^-6 ie microliter µL = 0.000001 L

Question 48

(1.2) Common unit prefixes: deci (d)

Answer 48

10^-1 ie deciliter (dL) = 0.1 L

Question 49

(1.2) Common unit prefixes: mega (M)

Answer 49

10^6 ie 3 megahertz (MHz) = 3,000,000Hz

Question 50

(1.2) Common unit prefixes: mili (m)

Answer 50

10^-3 i.e 2 milimoles (mmol) o.oo2 mol

Question 51

(1.2)100cm is 1 _______

Answer 51

1 meter

Question 52

1000g is 1 ________.

Answer 52

kilogram

Question 53

a millionth of the base unit is a _________ unit. (in the SI system)

Answer 53

micro

Question 54

(1.2) TRUE/FALSE "All certain digits along with the first uncertain digit in measurements are called significant figures or significant digits (or sig. figs.)."

Answer 54

TRUE

Question 55

(1.2) TRUE/FALSE "Exact numbers have no uncertainty as measured numbers do. Hence, exact numbers have an unlimited number of significant figures"

Answer 55

TRUE

Question 56

(1.2) TRUE/FALSE Only some non zero numbers are significant.

Answer 56

FALSE. all numbers 1-9 are significant numbers (all non zeroes).

Question 57

(1.2) Sigfig rules about zeros: Leading zeros (zeros to the left of the first nonzero digit) are __________________. (For example, 0823 contains three significant figures.)

Answer 57

Not significant

Question 58

(1.2) Trailing zeros that fall before a decimal point __________________. (For example, 6000. contains four significant figures, the 6 and the three zeros before the decimal point. Note that there is nothing after the decimal point.)

Answer 58

signifigant

Question 59

(1.2)Captive/Interior Zeros are always ______________.

Answer 59

significant.

Question 60

(1.2)Trailing zeros (zeros to the right of a nonzero digit) that fall after a decimal point are _________________. (For example, 745.00 contains five significant figures.)

Answer 60

significant.

Question 61

In which of the following are all the zeros significant? A) 0.002g ; 100g; 250.0g B) 1.500 x 10^4 mL; 058 mL; 0.50 mL C) 3.00 m; 405 m; 60.00m

Answer 61

C) 3.00m;405m;60.00m

Question 62

How many sig figs? 2.000 x 10^3

Answer 62

4 SF

Question 63

How many sig figs? 2.00 x 10^3

Answer 63

3 SF

Question 64

(Q1.2) The correct scientific notation for the number 0.00050210 is: A) 5.0210 x 10^4 B) 5.021 x 10^-4 C) 5.0210 x 10^-4

Answer 64

C) 5.0210 x 10^-4

Question 65

(Q1.2) The correct scientific notation for the number 500.0 is?

Answer 65

5.000 x 10^2

Question 66

(Q1.2) The correct decimal representation of 1.201 x 10^-7 is: A) 12010000 B) 0.0000001201

Answer 66

B) 0.0000001201

Question 67

(Q1.2) How many liters are in 333 mL?

Answer 67

0.333 L divide by 1000 (mili means divide by 1000 or multiply by .001)

Question 68

How many mililiters are in 17.5 L (expressed in scientific notation)

Answer 68

1.75 x 10^4 mL multiple by 1000 product is 17500 convert to scientific notation (3SF) 1.7500 (move decimal 4 places)

Question 69

Convert 17.40 ft^2 to in^2. Your answer must by given with the correct number of significant figures

Answer 69

2505.6 SF is 4. but remember the rules. all non zeros and captive zeros are sigfig

Question 70

(1.2) When _________ or ____________ numbers, round the result to the same number of digits as the number with the least number of significant figures (the least certain value in terms of multiplication and division).

Answer 70

When MULTIPLYING or DIVIDING

Question 71

(1.2) When doing ___________________ apply the two previous rules sequentially. For example, what is the answer or the following: (4.89 + 5.58) ÷ 1.327?

Answer 71

MIXED OPERATIONS the sum will have 2 sigfig past the decimal 4.89 + 5.58 = 10.47. then divide final answer will have 4 SF 7.890

Question 72

(1.2) If you add or subtract two ______________, the answer is ____________. If you add or subtract two ____________ digits, the result is ____________. Therefore, if you add or subtract a certain and an uncertain digit the result is ________________.

Answer 72

TWO CERTAIN.... ANSWER IS CERTAIN. UNCERTAIN, .....THE RESULT IS UNCERTAIN

Question 73

(2.1)The Formula for providing information about the accuracy of a measurement , is calculated using _______________ = error / true value * 100

Answer 73

Percent Error

Question 74

(2.1)The Formula for ____________ = experimental value - true value

Answer 74

Error

Question 75

(2.1)Precision is determined by the _________ of the experimental value from the average value (rather than true value) it's as follows: Average _______________ from the Mean Formula: (Sum of Deviations) / (number of deviations)

Answer 75

Deviations

Question 76

(1.2)Deviation from the ____________ = (experimental value - mean)

Answer 76

Mean

Question 77

(1.2)To indicate the precision relative to the mean in terms of percentage: _________________ = (deviation) / (mean) * 100

Answer 77

Percent Deviation

Question 78

(1.2)Two types of problem solving in Chemistry calculations are:

Answer 78

Specific equation type Unit conversion type

Question 79

(1.2)The formula: (Mass)/(Volume) is

Answer 79

Density

Question 80

(1.2)Dimensional analysis uses ______________ as a guide to solve problems. The _________ and ____________ must be subjected to the same mathematical operations as their associated numbers.

Answer 80

UNITS UNITS AND QUANTITIES

Question 81

(1.2)Dimensional analysis involves the use of one of more ________ conversion factors. A conversion factor is a _________ of two equivalent quantities expressed with different measurements.

Answer 81

UNITS. RATIO

Question 82

(1.2) ______________________ is a method that can be applied to computations ranging from simple unit conversions to more complex, multi-step calculations involving several different quantities.

Answer 82

DIMENSIONAL ANALYSIS

Question 83

(1.2) Convert 168 in. to meters. [1in. = 2.54 cm]

Answer 83

4.27m

Question 84

(1.2)1meter = ____ yard

Answer 84

1.0936yd

Question 85

(1.2)1in. = _____ cm

Answer 85

2.54cm

Question 86

(1.2) 1mile = ____meters

Answer 86

1609.3m

Question 87

(1.2) 1lb = 453.59 ____

Answer 87

grams

Question 88

(1.2) 1kg = 2.2046 ______

Answer 88

lbs (pounds)

Question 89

(1.2) km = 1000 ____

Answer 89

meters

Question 90

(1.2) 1meter = 100 _____

Answer 90

centimeters (cm)

Question 91

(1.2) 1yd = _____ ft

Answer 91

3 feet (ft)

Question 92

(1.2) 1cm = 10 ______

Answer 92

milimeters (mm)

Question 93

(1.2) What is the number 0.0001870 expressed in scientific notation?

Answer 93

1.870 x 10^-4

Question 94

(1.2)Compute the following with the correct SF: (2.057 x 0.0450 x 132)

Answer 94

12.2

Question 95

Set A Measurements: 8.84g, 8.69g, 8.75g Set B Measurements: 8.62g, 8.66g, 8.69g Which set of measurements are more precise if the true value for the object is 8.76g

Answer 95

SET B is more precise because the values are closer together (less variation)

Question 96

What is 3.67kg expressed in lb? [1 lb = 453.59g] A) 8.09lb B)1.66lb C)8.09 x 19^-6 lb

Answer 96

A) 8.09lb

Question 97

(Q1.2) How many meters are in 7528 cm?

Answer 97

75.28 m

Question 98

(1.2)What is 55mi/hr expressed in km/hr? [i mi = 1.609km]

Answer 98

88 km/hr

Question 99

(1.2)What is 35.0m^2 expressed in ft^2? [1in. = 2.54cm]

Answer 99

377ft^2

Question 100

(1.2)What is the mass of 25 cm^3 of gold? The density of gold is 19.3 g/cm^3

Answer 100

4.8 x 10^2 g

Question 101

(1.2) A metric ruler has markings of 0.1cm, which measurement is accurately reported by this ruler?

Answer 101

5.55cm

Question 102

(Q1.3) Which of the following items is a pure substance? A) air B) brass C) ice

Answer 102

C) ice water is H2O molecule containing a controlled ratio of ONLY Hydrogen and Oxygen

Question 103

(Q1.3) Which of the following statements is true about compound? A) A compound is always made up different types of atoms bonded together in proportions that may vary. B) A compound is always made up of different types of atoms bonded together in proportions that are fixed

Answer 103

B) A compound is always made up of different types of atoms bonded together in proportions that are fixed

Question 104

(Q1.3) Which of the following is physical property? A) The corrosive action of acid rain on granite B) The tarnishing of a copper statue C) The odor of spearmint gum

Answer 104

C) The odor of spearmint gum b/c the smell does not change the chemical properties or change the substance

Question 105

(Q1.3) Which of the following items is a chemical property? A) The melting and boiling point of water B) The tarnishing of a copper statue C) The odor of spearmint gum

Answer 105

C) The tarnishing of a copper stature Tarnishing is caused by a chemical reaction between the metal and oxygen and changes the atomic level

Question 106

(Q1.3) If you hold a solid piece of pure gallium metal in your hand, your body heat will melt the gallium into its liquid form. This illustrates which of the following: A) Distillation B) Physical change C) Chemical Change or a Chemical Property

Answer 106

B) Physical change melting does not induce any chemical or atomic changes in the elements (no bonding and no breaking)

Question 107

(Q1.3) How many joules are there in a 255 Calories snack bar? 1 cal = 4.184 J 1 Cal = 1000 cals

Answer 107

1.07 x 10^6 J

Question 108

Convert 68853 milijoules (mJ) to Calories [1 cal = 4.184 J and 1000 mJ in 1 J J A) 0.01646 Cal B) 60.77 Cal C) 164.6 Cal D) 16.46

Answer 108

D) 16.46 To convert millijoules to Calories, divide by 1000 to convert millijoules to joules and then divide by 4.184 to convert joules to Calories. 68852 millijoules is approximately equal to 16.47 Calories.

Question 109

If the monthly electricity consumption of a household in 6619 kWh, what is this consumption expressed in KJ? [1kWh = 3.60 x 10^6J] A) 2.38 x 10^7 kJ] B) 2.38 x 10^10 kJ

Answer 109

A) 2.38 x 10^7 kJ

Question 110

What is the value of 98 degrees F in units of C degrees A) 35 degrees Cels B) 37 degrees Cels C) 46 degrees Cels

Answer 110

B) 37 degrees Cels

Question 111

(Q1.3)What is 18 degrees Farenheit in terms of K (kelvin)? A) 251 K B) 265 K C) 301 K

Answer 111

B) 265K

Question 112

(Q1.3)In an exothermic reaction: A) The surroundings absorb heat from the reaction mixture B) The surroundings release heat to the reaction mixture B) Both the reaction mixture and surroundings release heat.

Answer 112

A) The surroundings absorb heat from the reaction mixture (Exo- exterior. Heat is absorbed by the surrounds or exterior surroundings)

Question 113

(1,3)In an endothermic: A) The energy of the reactants is higher than the energy of the products B) The energy of the reactants is lower than the energy of the products

Answer 113

B) The energy of the reactants is lower than the energy of the products

Question 114

(HW1.3) The rusting of iron is due to its reaction with oxygen. An iron nail weighing 8.531 g was left outdoors for a period of one year. After the year, it was found to have a mass of 12.197 g. How much oxygen did the nail combine with?' A) 3.666g B) 0.699g

Answer 114

A) 3.666g

Question 115

(HW1.3) Which statement is NOT part of the atomic theory? A) All atoms of an element have the same mass and other properties B) All elements are made up of indestructible particles called atoms D) Atoms are made up of protons, neutrons, and electrons

Answer 115

%%D maybe double check

Question 116

(HW1.3) According to Dalton's atomic theory: A) An atom cannot be subdivided into smaller particles B) An atom can be subdivided into smaller particles C) The nucleus is made up of protons and neutrons D) Electrons are lighter than protons

Answer 116

A) An atom cannot be subdivided into smaller particles

Question 117

(HW1.3) For most atoms, the nucleus consists of:

Answer 117

protons and neutrons

Question 118

The number of _____________ in an atom represented by the symbol Z, is used to identify the atom as a particular element, it and is the same for all atoms of a particular element.

Answer 118

protons the number of protons...

Question 119

If a calcium atom loses two electrons, how many electrons does it have? A) 18 B) 20 C) 22 D) not enough information

Answer 119

A) 18

Question 120

Atoms have no charge because their numbers of protons and electrons are ___________.

Answer 120

equal

Question 121

In general ________________ have the greatest effect on the size of an atom.

Answer 121

Electrons have....

Question 122

(3.1)What is matter?

Answer 122

matter is defined as anything that has mass and occupies space.

Question 123

(3.1) matter is classified based on _______, size, ________, and methods of separation.

Answer 123

state....composition

Question 124

Matter is classified into different states based on the following: The _______ between the particles. The ______ movement of the particles. The ________ of the sample The __________ The _________ of the sample.

Answer 124

spacing.... movements... shape.... volume... compressibility

Question 125

Summarize the properties that distinguist the states of matter: Solids.... Liquids.... Gases....

Answer 125

Solid substances have a rigid shape and volume. Liquids flow and posesses a definite volume but not a definite shape. Liquids take the shape of its container (except that it forms a flat or slightly curve upper surface when acted upon by gravity) Gases are COMPRESSIBLE and take the shape and volume of their container. Gases are volumes are depended on pressure conditions.

Question 126

The spacing of particles in each state of matter: Solid... Liquid.... Gas...

Answer 126

Solids particles are spaced VERY CLOSE TOGETHER Liquids are spaced CLOSE TOGETHER Gases are spaced FAR APART

Question 127

Movement of the particles of each state of Matter: Solids... Liquid... Gas...

Answer 127

Particles in Solids VIBRATE Liquids MOVE RELATIVE TO EACH OTHER Gases MOVE INDEPENDENTLY OF EACH OTHER

Question 128

The THEORY that states matter is comprised of tiny particles that are in random motion.

Answer 128

Kinetic molecular theory

Question 129

Gas Laws describe the behavior of gases by showing the relationships between a gases's volume, temperature, and _____________.

Answer 129

pressure.

Question 130

The gas law that states the volume of a gas is inversely proportional to applied pressure ((if temperature and moles of gas (n) are constant))

Answer 130

Boyle's Law

Question 131

The gas law that states the volume of a gas is directly proportional to the kelvin temperature ((if pressure and number of moles are constant))

Answer 131

Charles's Law

Question 132

What's an Ideal Gas?

Answer 132

An ideal gas is not a real gas. It's a hypothetical gas that obeys the gas laws at all temperatures and pressures perfectly. The construct of an Ideal gas help to calculate what real gases may do at HIGH TEMPERATURES and LOW PRESSURES

Question 133

PV = nRT

Answer 133

The ideal Gas Law equation P= gas pressure V= gas volume n = moles of gas R = gas constant T = kelvin in temp

Question 134

Name an example of the Boyle's law in application

Answer 134

When a diver experiences the "bends" or "decompression sickness" if they rise to quickly from a lower depth because it will make their lungs (which holds O2 and Co2 ) expands out into the blood stream to quickly

Question 135

Name an example of Charles's law in application

Answer 135

When the gas in a hot air balloon is heated, the expansion of the hot gas leads to a LOWERING of the density of the balloon. the balloon becomes less dense than the surrounding air, allowing the hot air balloon to rise.

Question 136

A sample of gas will increase in VOLUME if it is heated at a constant pressure.... _______ law

Answer 136

Charles's law

Question 137

At high altitudes, the air pressure is lower than at sea level..... _______ law

Answer 137

Boyle's law

Question 138

(1.3) Name examples of matter classified PARTICULATE (diameters less than 1nm):

Answer 138

Virus Protein molecule Aspirin molecule water molecule atom (descending order)

Question 139

(1.3) Name examples of matter classified as MICROSCOPIC (diameters ranging from 1mm to 10nm):

Answer 139

plant cell animal cell bacterial cell

Question 140

(1.3) name examples of matter classified as MACROSCOPIC

Answer 140

Height of a human sheet of paper wedding ring thickness of a CD grain of sand

Question 141

Matter with constant properties and composition such as Ice cubes is a __________substance

Answer 141

Pure substance

Question 142

Matter without constant properties/composition/fixed ration are a __________.

Answer 142

mixture

Question 143

TRUE/FALSE all pure substances are heterogeneous mixture.

Answer 143

FALSE pure substances are homogeneous and uniform throughout (having fixed properties and ratio).

Question 144

Examples of a heterogenous mixture are:

Answer 144

tossed salad, pizza, oil in watter, coffee

Question 145

A Pure substance that can be simplified chemically is a _______

Answer 145

COMPOUND because its made of multiple parts but fixed ratios. Therefore a compound can be broken down into base elements

Question 146

A Pure substance that CANNOT be simplified chemically is an _______________

Answer 146

ELEMENT one type of atom makes up the substance. cannot be chemically brokendown/ simplified

Question 147

Examples of compounds

Answer 147

Salt, Sugar, Water, Oxygen, Carbon

Question 148

examples of elements

Answer 148

Hydrogen, copper, helium, argon,

Question 149

Elements on the periodic table are organized in 7 rows called ___________ and 18 columns called ____________.

Answer 149

7 periods across.... 18 groups vertical...

Question 150

(3.1)Whats the element in group 1 period 1?

Answer 150

Hydrogen

Question 151

Mixtures can be seperated by physical means such as, Filtration, _________, magnetism, and chromatography

Answer 151

Distillation

Question 152

Color is a _________ property.

Answer 152

Physical property

Question 153

Density is a _______ (chemical/physical) property and ______ (intensive/extensive) property

Answer 153

Physical property : there is no chemical change intensive because : When a property, like density, is independent of the amount of sample measured, it is known as an "intensive" property.

Question 154

Odor is a _________ property.

Answer 154

Physical property

Question 155

Boiling point of a substance is a _________.

Answer 155

Physical property

Question 156

burning of a log is an example of a ___________________.

Answer 156

chemical change

Question 157

Which one is NOT chemical change A) rusting of iron B) decomposition of milk C) melting iron

Answer 157

C) melting iron is a physical change because the atomic/chemical bonds are not changed

Question 158

Which one is NOT physical property? A) color B) odor C) rusting of iron

Answer 158

C) the rusting of iron is an oxidation process. thus it's a chemical change

Question 159

TRUE/FALSE The following: filtering a mixture, boiling water, melting iron, seperating the components of dyes in a mixture, is a list of chemical changes.

Answer 159

FALSE the list is all physical changes

Question 160

TRUE/FALSE If the property depends on the amount of matter present, it is an extensive property.

Answer 160

TRUE

Question 161

TRUE/FALSE Temperature is an intensive property, because the property (temperature) of a sample of matter does not depend on the amount of matter present.

Answer 161

TRUE

Question 162

TRUE/FALSE the mass and volume of a substance are examples of extensive properties

Answer 162

TRUE because the value of an extensive property is directly proportional to the amount of matter in question. EX a gallon of milk has a larger mass that a cup of milk.

Question 163

Temperature is intensive property, heat is an ______ extensive property.

Answer 163

extensive property. (when you combine oil at 100 degrees the temperature remains the same). But more oil means more heat (extensive).

Question 164

Changing a substances size or shape is an example of a ______ change.

Answer 164

physical change

Question 165

The ________ change affects a composition of the substance. It's when the substance reacts to another and gives rise to another or more new substances i.e iron rusting

Answer 165

chemical

Question 166

(1.3) A candy bar contains 225 Cal of nutritional energy. How many joules does it contain? [1 cal = 4.184 J]

Answer 166

9.41 x 10^5 J solution map: Cal > cal > J

Question 167

____ cal = 4.184 J ____ cal = 1 Cal ____ cal = 1kcal ____ kWh = 3.60 x 10^6 J

Answer 167

1 cal 1000 cal 1000 cal 1 kWh

Question 168

Convert 485 cal to kilojoules. [1 cal = 4.184 J

Answer 168

2.03 kJ

Question 169

Energy is neither __________ nor ____________ but it can be changed from one form to another.

Answer 169

created..... destroyed

Question 170

(1.3) Kinetic energy is the energy associated with ___________.

Answer 170

motion

Question 171

(1.3) Potential energy is the energy associated with ________ and _______ of matter. Objects with high potential energy ten to be unstable. So they have a tendency to change in a way that lowers their potential energy

Answer 171

position.... composition

Question 172

______ molecules tend to undergo rapid chemical changes that lower their potential energy, which is why it's so explosive. (name of molecule that's explosive)

Answer 172

TNT (trinitrotoluene)

Question 173

Energy and Change of States generally involve the ______ or ______ of energy.

Answer 173

gain.... loss

Question 174

(1.3) involves the loss of heat in a system. When heat is released the potential energy of the system is lowered and the process is _______________.

Answer 174

Exothermic

Question 175

(1.3) When heat is absorbed, the potential energy of the system is increased and the process is said to be _______________.

Answer 175

Endothermic

Question 176

Products of an endothermic reaction gain ______ energy.

Answer 176

potential (starting materials have lower potential energy than the products)

Question 177

products of an exothermic reaction ______ potential energy.

Answer 177

loss energy.

Question 178

(1.3) Condensation, ________, and deposition involve a loss of heat. When heat is released, the potential energy of the system is _______.

Answer 178

Freezing..... Lowered. (Exothermic)

Question 179

(1.3) Melting (fusion), __________, and sublimation involve a gain of heat in the system. When the system absorbs heat, the potential energy is ___________.

Answer 179

Vaporization, increased. (Endothermic)

Question 180

Complete the blanks: EXO Condensation : ____ to liquid Freezing : _____ to solid Deposition: ____ to solid ENDO Melting : ____ to liquid Vaporization : _____ to gas Sublimation : _____ to gas

Answer 180

gas to liquid liquid to solid gas solid solid to liquid liquid to gas solid to gas

Question 181

Potential energy that is lost during an exothermic process is generally converted to ______.

Answer 181

heat

Question 182

Because energy is __________ in a change, an increase in potential energy means that there is a decrease in the kinetic and vice versa.

Answer 182

conserved

Question 183

Lower _____ energy content means that temperature is lowered and a higher ______ energy content means that temperature is increased.

Answer 183

kinetic, kinetic.

Question 184

(1.3) the degree of hotness or coldness of a body is __________.

Answer 184

temperature

Question 185

original and converted temperatures must have the same _________.

Answer 185

precision

Question 186

(3.1) approximately twice the degree Celsius

Answer 186

degree Fahrenheit

Question 187

Convert 15.5 Fahrenheit into Celsius and Kelvins F to C: (F-32)* 5 /9 F to K: F-32 * 5 / 9 + 273.15

Answer 187

-9.2 Celsius 264.0 Kelvin

Question 188

F = (Celsius x 1.8 ) + 32

Answer 188

Converting Fahrenheit to Celsius

Question 189

C = (F - 32 )/1.8

Answer 189

Converting Celsius to Fahrenheit

Question 190

K = C + 273.15

Answer 190

Converting Celsius to Kelvin

Question 191

C = K - 273.15

Answer 191

Converting Celsius to Kelvin

Question 192

According to what Theory is: "Matter is made of extremely small particles called atoms"

Answer 192

Dalton's Atomic Theory

Question 193

According to Dalton's Atomic Theory: "All atoms of a given element are identical in mass and properties. Atoms of one element ______ in properties from atoms of all other elements."

Answer 193

differ.

Question 194

According to Dalton's Atomic Theory "____________ are formed by a combination of two or more different kinds of atoms."

Answer 194

Compounds

Question 195

According to Dalton's Atomic Theory: "Atoms cannot be __________, created, nor ________."

Answer 195

subdivided, destroyed

Question 196

According to Dalton's Atomic Theory: Atoms of one element cannot be ________ into atoms of another element. A _________ reaction is a rearrangement of atoms.

Answer 196

converted.... chemical

Question 197

Why was the Atomic theory proposed by Dalton so important?

Answer 197

It explained two important laws that were established in the 18th century by previous chemists. These two lass was the mass conservation in chemical changes and of definite proportions or constant composition

Question 198

__________ states that in a chemical change mass is conserved. This means that the total number and kinds of atoms present at the start of a chemical process will be the same at the end.

Answer 198

Law of Conservation of Mass

Question 199

_______________ states that all samples of a pure compound contain the same elements in the same proportion by mass. The idea that the numbers of atoms of the elements in a given compound always exist in the same ratio is consistent with these observations.

Answer 199

The law of definite proportions (or the law of constant composition)

Question 200

___________________ is applied whenever the chemical formula of a compound is written. For instance, we write the chemical formula for water as H2O regardless of who makes it, where it is made, or the reaction by which it is made. If the substance is water, any sample of it will have a mass ratio of 8 g oxygen to 1 g hydrogen. The laws of conservation of mass and of definite proportions are foundational to the advances in chemistry.

Answer 200

The law of constant composition

Question 201

_______________ states that when two elements react to form more than one compound, a fixed mass of one of the elements will react with masses of the other element in a ratio of small, whole numbers.

Answer 201

The Law of Multiple Proportions

Question 202

When 0.96g of oxygen and 0.12g of hydrogen combine, 1.08g of water is expected to form is a condition that illustrates the law of _______________.

Answer 202

The law of conservation of mass

Question 203

An amount of 0.96g of oxygen is expected to react with 0.12g of hydrogen to form water illustrates the law of ______________________.

Answer 203

The law of constant composition

Question 204

A substance that is represented by at least two different types of spheres arranged in an orderly fashion illustrates an example of a _____________

Answer 204

compound

Question 205

Each Element is comprised of tiny, indivisible particles illustrates _________ theory.

Answer 205

atomic theory

Question 206

The ______ and the neutron have very similar masses and each is nearly two thousand times as heavy as an electron

Answer 206

proton

Question 207

The _________ therefore, contains the majority of an atom's mass, whereas electrons occupy almost all of an atom's volume

Answer 207

nucleus

Question 208

the more __________ an atom has, the greater the volume of space that the electrons will occupy. This means that atoms with more electrons will generally be larger in size than atoms with fewer electrons.

Answer 208

Electrons

Question 209

The number of ___________ in the nucleus of an atom is called its atomic number and is denoted as Z. This is the defining trait of an element: Its value determines the identity of the atom

Answer 209

protons

Question 210

The _________ of an atom is influenced by the number of electrons i that it has

Answer 210

size

Question 211

Consider a sample of H2O, in which form is the average kinetic energy the highest? A) Steam B) water C) Ice

Answer 211

A) Steam

Question 212

Identify the property that is both physical and intensive. A) color B) odor C) density D) all physical and intensive properties

Answer 212

D) All are physical and intensive properties

Question 213

Which is the correct temperature in Celsius of 46.8 degrees Fahrenheit A) 8 degrees Celsius B) 8.2 degrees Celsius

Answer 213

B) 8.2

Question 214

Which of the following statements are NOT true? A) the law of multiple proportions B) The atomic theory explains the law of conservation of mass. C) the atomic theory explains the law of definite proportions

Answer 214

A) the law of multiple proportions was known before Dalton proposed the atomic theory

Question 215

O2 (gas)

Answer 215

Molecule and Element 2 bonded oxygen atoms

Question 216

Fe (s)

Answer 216

Atom, Element (single atom)

Question 217

NaCl(s)

Answer 217

Compound, Ionic Compound ionic compounds are usually metals

Question 218

Melting iron is a ________change. Browning Marshmellows is a ___________ change.

Answer 218

physical , chemical

Question 219

If exactly 441g of propane and 1,600grams of oxygen combust to form 721g of water. How many grams of carbon dioxide are formed?

Answer 219

1320g carbon dioxide

Question 220

Convert 285 calories to Joules

Answer 220

68.1 Joules

Question 221

Convert 32 degrees F to degrees C

Answer 221

0 degrees C

Question 222

10) Convert 30.0 degrees C to degrees K

Answer 222

303 degrees Kelvin

Question 223

Convert 2.34 x 10^-3m to km

Answer 223

2.34 x 10^-6 km

Question 224

Convert 0.00345 km to μm

Answer 224

3.45 x 10^6 μm

Question 225

Calculate the density of magnesium in g/cm^3, in a sample of magnesium has a mass of 14.3g and it has a volume of 8.46 cm^3

Answer 225

1.69g/cm^3

Question 226

The density of mercury is 13.6 g/mL. how many pounds lnns does one quart of mercury weigh?

Answer 226

28.4lbs

Question 227

what is 1.74935 rounded to 2 SF?

Answer 227

1.7

Question 228

What is 0.089510 rounded to 2 SF?

Answer 228

0.090

Question 229

What is 100459.7 rounded to 3 SF?

Answer 229

1.00 x 10^5

Question 230

What is the sum of 6.289 + 0.52 + 1.3?

Answer 230

8.109 rounded to 8.1 as final answer because you one want one uncertain digit in you answer max.

Question 231

Five students (A to E) used the same balance to measure a metal block separately. The true mass of the block is 50.0000 g but the students obtained the following masses: A: 49.9990 B: 49.9451 C: 50.0025 D: 50.9000 E: 49.9889 CALCULATE THE MEAN OR AVERAGE

Answer 231

50.1671g HOW: (sum of masses) / (number of masses)

Question 232

Five students (A to E) used the same balance to measure a metal block separately. The true mass of the block is 50.0000 g but the students obtained the following masses: A: 49.9990 B: 49.9451 C: 50.0025 D: 50.9000 E: 49.9889 CALCULATE THE DEVIATION OF ALL STUDENTS AND THE AVG DEVIATION

Answer 232

A. 0.1681g B. 0.2220 C. 0.1681 D. 0.7329 E. 0.1782 AVG: 0.2932 HOW: (measured value - mean) ex student A: 49.9990g-50.1671g=0.1681g for average add the list of values and divide by 5 (number of values)

Question 233

Five students (A to E) used the same balance to measure a metal block separately. The true mass of the block is 50.0000 g but the students obtained the following masses: A: 49.9990 B: 49.9451 C: 50.0025 D: 50.9000 E: 49.9889 CALCULATE THE ERROR OF ALL THE STUDENTS

Answer 233

A. 0.0010 B. 0.0549 C. 0.0025 D. 0.9000 E. 0.0111 HOW: (measured value - true value) ex student A: 49.9990g-50.0000g=0.0010g

Question 234

Five students (A to E) used the same balance to measure a metal block separately. The true mass of the block is 50.0000 g but the students obtained the following masses: A: 49.9990 B: 49.9451 C: 50.0025 D: 50.9000 E: 49.9889 CALCULATE THE PERCENTAGE ERRORS OF ALL STUDENTS AND THE PERCENT ERROR OF THE GROUP

Answer 234

A: 0.002% B: 0.110% C: 0.0050% D: 1.800% E: 0.0222% AVG: 0.3878% HOW: (error) / (true value) *100 ex student A: (0.0010g) / (50.0000g)=0.00002g * 100 =0.002%

Question 235

Five students (A to E) used the same balance to measure a metal block separately. The true mass of the block is 50.0000 g but the students obtained the following masses: A: 49.9990 B: 49.9451 C: 50.0025 D: 50.9000 E: 49.9889 CALCULATE THE PERCENTAGE ERROR ALL THE STUDENTS

Answer 235

0.002% HOW: (error) / (true value) *100 ex student A: (0.0010g) / (50.0000g)=0.00002g * 100 =0.002%

Question 236

DIMENSIONAL ANALYSIS: calculate what is the density of a liquid whose mass is 27.2g and the volume is 22.5 mL?

Answer 236

1.21g/mL density = (mass)/(volume)

Question 237

DIMENSIONAL ANALYSIS: (1inch)/(1inch) = (2.54cm)/(2.54cm) = ______

Answer 237

1 because the ratio is an equality relationship illustrating that a unit of 1in. EQUALS 2.54cm

Question 238

What is 1ft^3? a measure of?

Answer 238

cubic is a measure of volume.

Question 239

Liters is a measure of units for _________.

Answer 239

Volume

Question 240

1L = 1000 ______

Answer 240

mL

Question 241

1mL = _____ cm^3

Answer 241

1

Question 242

A solution map shows how the ______ will be changed in the conversion process, that calculates a dimensional analysis equation.

Answer 242

units

Question 243

What is 194cm converted to ft? [1in = 2.54cm]

Answer 243

6.36 ft Sol map: cm to in. to ft

Question 244

What is 4.86lb in kg? [1lb - 453.59 g]

Answer 244

2.20kg sol map: lb to gram to kg

Question 245

What is 4.89 gal converted to L? [1 L = 1.057 qt]

Answer 245

18.5 L sol map: gal to qt to L

Question 246

What is 3.00 x 10^8 meters/second in miles/hour? [1 mile = 1.609km]

Answer 246

6.71 x 108 miles/hr sol map: numerator: m to km to mi denominator: s to min to hr

Question 247

What is 125m^3 converted to in^3 [1in = 2.54 cm]

Answer 247

7.63 x 10^6 in^3 sol map meters cubed to centimeters cubed to inches cubed **cube the conversion units so it matches the 125^3 in the original problem.

Question 248

If a liquid substance has a density of 1.32 g/cm^3, what volume (in mL) shoud be measured to obtain a mass of 68.4g?

Answer 248

51.8 mL solmap: g to cm3 to mL

Question 249

Classify each statement as an observation, a law, or a theory: a) When the pressure on a sample of oxygen has is increased 10%, the volume of the gas decreases by 10% b) The volume of a gas is inversely proportional to its pressure c) A gas is composed of small particles in constant motion d) A gas sample has a mass of 15.8g and a volume of 10.5L

Answer 249

observations: a,d law: b theory: c

Question 250

convert 27m/s to km/hr

Answer 250

97km/hr

Question 251

A graduated cylinder has markings every mililiter. Which measurement is accurately reported for this graduated cylinder? a) 21mL b)21.2mL c)21.23mL

Answer 251

b) 21.2mL

Question 252

How many SF are in the number 0.00620?

Answer 252

3

Question 253

Perform this multiplication to the correct number of significant figures: 65.2*0.0015*12.02

Answer 253

1.2

Question 254

The SI units of ________ are units of length raised to the third power; liters or milliliters are often used as well. The density of a substance is its mass divided by its ________.

Answer 254

volume

Question 255

Always count the following digits as significant: _______ digits interior zeros __________ zeros after a decimal point trailing zeros before a ________ point but after a nonzero number.

Answer 255

nonzero trailing zeros decimal point

Question 256

How many significant figures are in the following numbers? a) 1.0050 b) 0.00870 c) 100.085 d) 5400

Answer 256

a) 5 b)3 c)6 d) impossible to tell in it's current form

Question 257

Answer 257

the result of a multiplication of division should carry the same number of significant figures as the factor with the least number of significant figures

Question 258

Answer 258

In calculations involving both addition/subtraction and multiplication/division, do the steps in parentheses first, keeping track of how many significant figure, then proceeding with the remaining steps. DO NOT ROUND UNTIL THE VERY END!!!

Question 259

convert 108 ft to meters (there are 39.37in in 1 meter)

Answer 259

Question 260

Answer 260

answer = 26.46 mg/kg

Question 261

Answer 261

Question 262

Answer 262

Question 263

Answer 263

Question 264

Answer 264

Question 265

Answer 265

54.9 mL

Question 266

Answer 266

Question 267

A compound is composed of different atoms that are chemically united (bonded). While a _____________ is composed of different substances that are not chemically united, but simply mixed together.

Answer 267

mixture

Question 268

a ________ substance can also be a compound, a substance composed of two or more elements in a fixed definite proportions.

Answer 268

pure substance

Question 269

we can classify mixtures according to how uniformly the substances within them are mixed. In a __________________ mixture, such as oil and water the composition varies from one region to another. in a _______________ mixture, the composition is uniform because the atoms or molecules are mixed uniformly.

Answer 269

heterogeneous homogeneous

Question 270

You can classify a pure substance into 2 categories: __________ and ___________

Answer 270

element and compounds