Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry 2013-2014 > Finals Flash Cards > Flashcards

Finals Flash Cards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Matter is defined as anything that occupies space and has

A

Mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Which pair Is classified as a substance

A

Elements and Compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Which of the following statements is an identifying characteristic of a mixture?

A

Can be separated by physical means

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

When sample X is passed through a filter paper, a white residue, Y, remains on the paper and a clear liquid, Z, passes through. When liquid Z is vaporized, another white residue remains. Sample X is best defined as

A

Heterogeneous Mixture

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What best describes a chemical property of the element Iodine?

A

It reacts with Hydrogen to form a gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Ductility and malleability are examples of

A

Physical Properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How man kilo-joules is the equivalent of 750 joules

A

.750 kj

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Review 8-12 in the packet

A

Skip

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Compounds are usually broken down into their component elements by

A

Chemical Changes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Which Substance can be decomposed by chemical change?

A

Ammonia (Anything that is a substance and not an element)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is an EXTENSIVE physical property?

A

Mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

How many kilo-joules of heat energy are absorbed when 100 grams of water is heated from 20 degrees Celsius to 30 degrees Celsius

A

4.18kj

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the total number of joules of heat energy released when 20 grams of water is cooled from 20 degrees Celsius to 10 Degrees Celsius

A

836J

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Homo means

A

Evenly Mixed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Hetero means

A

Unevenly Mixed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Intensive means

A

Value stays the same

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Study 19 In Packet

A

Skip

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

An ideal gas is made up of gas particles that

A

are in random motion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What are the qualities of an ideal gas

A

Random Motion, Little attraction for each other, Insignificant volume, Hit wall and build up pressure, Hit each other and transfer energy but total energy remains the same

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What are the qualities of a real gas?

A

Has volume, have force of attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Normal Units of pressure

A

STP, 1 atm, 0 degrees Celsius, 760 mmHg, 273 Kelvin, 760 torr

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Equation for Volume Pressure, Temperature and Moles

A

V1 Phave 1 = V2 P2
____________
T1 n1 = T2 n2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

An assumption of the kinetic theory of gas is that the particles of a gas have

A

little attraction for each other and an insignificant volume

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

The pressure on 30 milliliters of an ideal gas icreases from 101.3 kPa to 202.6 kPa at constant temperature. The new volume is equal to

A

101.3 kPa
30 mL x ________
202.6 kPa

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

A sample of gas has a volume of 2.0 liters at a pressure of 1.0 atm. When the volume increases to 4.0 liters, at a constant temperature, the pressure will be

A

.5 atm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

a 2.5 liter sample of gas is at STP. When the temperature is raised to 273 degrees Celsius and the pressure remains constant the new volume of the gas will be

A

5.0 Liters

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

S 16 Liter sample of CH4(g) is at 0 degrees Celsius and 1 atm. The volume of the gas sample in liters at 27 Degrees Celsius and 1 atm is equal to

A

300
22.4 x _____
273

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

When 7.0 Moles of gas A and 3.0 moles of Gas B are combined, the total pressure exerted by the gas mixture is 1.0 atm. What is the partial pressure exerted by gas A in this mixture

A

.7 atm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Which gas will diffuse at the rate under the same conditions of temperature and pressure

A

H2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

A .50 mole sample of CO2(g) at 2.0 atm occupies 11.2 liters. What is the temperature of the sample

A

546 K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

The density of a gas is 3.00 grams per liter at STP What is the gram molecular mass of the gas

A

22.4g

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What is the formula for Lead (II) Oxide

A

PbO

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

No “o”

A

Hydro

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

O

A

Hydro

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Ate becomes your

A

Ic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Ite becomes your

A

Ous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

Complete Combustion

A

—–> CO2 + H2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Incomplete Combustion

A

—–> CO + H2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

What order you go in when balancing equation

A

HCO

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

What is the formula for Chromium (III) Oxide

A

Cr2O3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

Which Formula is correctly paired with its Name

A

CuCl2 —–> Copper (II) Chloride

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

What is the correct name for the compound with the formula CrPO4

A

Chromium (III) Phosphate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

What is the name of the compound whose formula is H2SO4

A

Sulfuric Acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

The chemical equation 4Na(s) + O2 —> 2Na^2O(s) is best described as a

A

Synthesis reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

What type of reaction is illustrated by the following chemical equation 2H2O(l) —> 2H2(g) + O2(g)

A

Decomposition

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

The chemical reaction Zn(s) + CuSO4(aq) —> ZnSO4(aq) + Cu(s) is best described as a

A

Single replacement reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

What type of reaction best describes the following chemical reaction 2AlCl3(aq) + 3Na2CO3(aq) —> Al2(CO3)3(s) + 6NaCl(aq)

A

Double replacement reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

C2H4(g) + 3O2(g) —> 2CO2(g) + 2H2O(g)

A

Complete Combustion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

When the equation C2H4 + 3O2 —> 2CO2 + 2H2O balanced using the smallest whole numbers, what is the coefficient of the O2

A

3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

Al2(SO)3 + 3ZnCl2 —> 2AlCl3 + 3ZnSO4 is correctly ballanced using the smallest whole number coefficient, the sum of the coefficients is

A

9

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

KCl(aq) + AgNO3(aq) —> KNO3(aq) + X What is the correct formula for the product representing X

A

AgCl

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

In the 1880’s JJ Thomson proved the cathode ray hadn a negative charge. What subatomic particle makes up the cathode rays

A

Electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

What did the discovery of cathode rays reveal about the structure of the atom

A

Made of subatomic Particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

Most alpha articles passed through the gold foil undeflected. What conclusion was made about the structure of the atom based on this observation

A

Mostly empty space, had to be some postive ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

A few alpha particles were deflected back at the source. What did this observation reveal about the structure of the atom

A

Small dense positive nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
56
Q

What term refers to the region of an atom where an electron is most likely to be found

A

orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
57
Q

The atomic number of an atom is always equal to the total number of

A

Protons and Neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
58
Q

All atoms of an element have the same

A

Atomic Number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
59
Q

The mass number of an atom is equal to the number of

A

Neutrons plus electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
60
Q

What is the mass number of the atom below? 3 H

1

A

3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
61
Q

Where is mass

A

On top

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
62
Q

How do you find neutrons

A

Subtract two numbers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
63
Q

In which pair of atoms do both neclei contain the same number of neutrons

A

Whichever two subtract to the same number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
64
Q

What is the total number or nucleons (protons and neutrons) in the atom below

A

Top number is mass and mass is equal to protons+neutrons= Nucleons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
65
Q

What is the mass number of an atom which contains 21 electrons, 21 protons, and 24 neutrons

A

45

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
66
Q

Find the average mass of a sample of magnesium which contains 78.7% Mg-24, 10.1% Mg-25 and 11.2% Mg-26

A

(24)(.787)+(25)(.101)+(26)(.112)=24.3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
67
Q

Element X has two isotopes. If 72% of the element has an isotopic mass of 84.9 atomic mass units, and 28% of the element has an isotopic mass of 87 atomic mass units, the average atomic mass of element X is numerically equal to

A

(72.0 x 84.9) (28.0 x 87.0)
___________ + ____________
100 100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
68
Q

The average isotopic mass of chlorine is 35.5. Which mixture of isotopes (show percents) produces this average mass?

A

75%^35Cl and 25%^37Cl

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
69
Q

Which electron dot symbol could represent a metalloid (B, Si, As, Te, At)

A

If it has 5 dots around it

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
70
Q

The characteristics bright-line spectrum of an element is produced when its electron

A

Returns to a lower energy state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
71
Q

Which electron configuration represents a potassium ion in the excited state

A

Add up then identify element if matches, ground state if not excited

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
72
Q

What is the total number of occupied sublevels in an atom of chlorine in the ground state

A

5

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
73
Q

An atom has 8 electrons in a d sublevel. How many d orbitals in this sublevel are half filled

A

2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
74
Q

How do the orbitals go

A

2, 8, 18, 32, 50

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
75
Q

What is the total number of sublevels in a principal energy level

A

2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
76
Q

How much does one principal energy level go up by

A

1 Each Time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
77
Q

How many protons are in the nucleus of a magnesium atom?

A

12 (atomic number)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
78
Q

Write the electron configuration for Magnesium in the ground state

A

1s22s22p63s2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
79
Q

How does an atom of magnesium become Mg+2 ion

A

Loses 2 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
80
Q

What noble gas has the same electron configuration as Mg+2

A

Neon

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
81
Q

Name three elements that could be X

A

Oxygen, Sulfur, Selenium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
82
Q

The pair of elements with the most similar chemical properties are

A

The ones right on top and below each other are the closest

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
83
Q

Which atom has the largest atomic radius?

A

The one closest to the lower left of the table

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
84
Q

As the elements of Group 16 are considered from top to bottom on the Periodic Table , the atomic radii

A

Increase and the ionization energies decrease

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
85
Q

The S-2 ions differ from the S0 atom in that the S-2 ion has a

A

Larger radius and more electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
86
Q

What type of energy represents in the equation Na+energy—-> Na+ + e-

A

Ionization energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
87
Q

Define Ionization Energy

A

The ionization energy is the exact quantity of energy that it takes to remove the outermost electron from the atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
88
Q

In which reaction is the first ionization energy greatest

A

The one closest to the top right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
89
Q

Which element in period 2 has the greatest tendency to gain electrons (electronegativity)

A

One closest to upper right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
90
Q

Period is

A

Horizontal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
91
Q

Group is

A

Vertical

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
92
Q

What group in the periodic table contains the elements to the alkaline earth family

A

2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
93
Q

When oxygen combines with any alkaline metal, M, the formula of the compound produced usually is

A

MO2

94
Q

Which Element is a halogen

A

Group 7A

95
Q

Ozone is an allotropic form of the element

A

Oxygen

96
Q

Who was credited with creating the first periodic table that organized the elements according to atomic mass

A

Dmitri Mendeleev

97
Q

A diagram with two same size circles one white, one black labeled X and Z yield one smaller circle white with X+ plus one larger circle black Z- Which particle (X or Z) most likely represents a metal atom?

A

X is metal because it becomes a smaller positive ion

98
Q

A diagram with two same size circles one white, one black labeled X and Z yield one smaller circle white with X+ plus one larger circle black Z- which most likely represents a nonmetal atom?

A

Z because it become a larger negative ion

99
Q

Which metal is the most reactive metal?

A

The closest to the bottom left is

100
Q

Which is the most reactive non metal

A

The closest to top right

101
Q

Which element has properties of both metals and non metals

A

Any metalloid (on the line)

102
Q

Which two elements would most likely combine to form an ionic compound

A

The metal and non metal farthest from each other

103
Q

Which element can lose electrons from its two outermost energy level

A

Any transition metal (One of the metals in the middle)

104
Q

Which element exists as a monoatomic gas at STP

A

Any of the Noble Gases

105
Q

Which element exists as a diatomic gas at STP

A

C,N,O,F,Cl,Br,I,H

106
Q

Define a transition metal

A

Is more than one color and can take electrons from more than 1 energy level, can have more than one binary compound

107
Q

Given the reaction: H2 + Cl2 —-> 2HCl

Which of the following statements best describes the energy change as bonds are formed and broken in this reaction

A

The forming of the H—Cl bind releases energy

108
Q

Which formula represent an Ionic Compound

A

Any one with a metal and non metal

109
Q

If the last element is an even coefficiant what is it

A

Non polar

110
Q

If the last element is an odd coefficient what is it?

A

Polar

111
Q

Review Questions number 89-93 + Compounds in back of packet

A

SKIP

112
Q

Which combination of atoms can form a polar covalent bond?

A

H and Br

113
Q

Which two compounds contain only polar molecules

A

2 elements with odd coefficients

114
Q

In a nonpolar covalent bond, electrons are

A

Shared equally by two atoms

115
Q

Which of the following statements best explain why a CH4 molecule is non polar

A

CH4 has a symmetrical charge distribution

116
Q 
The table below shows four compounds and the boiling point of each: Which type of molecular attraction accounts for the high boiling points 
Compound | Boiling Point 
H2O             100 C
H2S             -60.7 C
H2Se           -41.5 C
H2Te           -2.2 C
A

Hydrogen Bonding

117
Q 
The table below shows four compounds and the boiling point of each: Compared the boiling points of H2S, the boiling point of H2O is relatively high. Which type of bonding causes this different?
Compound | Boiling Point 
H2O             100 C
H2S             -60.7 C
H2Se           -41.5 C
H2Te           -2.2 C
A

Hydrogen

118
Q

What is the Gram Formula Mass of Al2(SO4)3

A

342g

119
Q

What is the total number of moles contained in 115 grams of C2H5OH

A

2.50

120
Q

A sample of nitrogen containing 3.0x10^23 molecules has the same number of molecules as a sample of

A

.50 (Half) Moles of Ne

121
Q

What is the mass of 3.0x10^23 atoms of Neon

A

10 grams

122
Q

Which sample of O2 contains a total of 3.01x10^23 molecules at STP

A

16.0 grams

123
Q

The percent bny mass of oxygen in H2C2O4

A

64
____ x 100
90

124
Q

The empirical (reduced) formula of the compound whose molecular formula is P4O10

A

P2O5

125
Q

What is an empirical formula?

A

The most reduced formula

126
Q

A 10 gram sample of a hydrate was heated until all the water of hydration was driven off. The mass of anhydrous product remaining was 8.00 grams. What is the percent of water in the hydrate?

A

Second number/First Number= T
T - 100 = Answer
20%

127
Q

What is the empirical formula of a compound consisting of 29.6% Oxygen and 70.4% Fluorine by mass

A

Divide percents by the elements mass then divide the smalled number by all other numbers should equal .0 or .9 if not multiply by (5 3 5 2 5 3 5)

128
Q

A compound contains .5 moles of sodium, .5 moles of Nitrogen, and 1 mole of hydrogen. The empirical formula of the compound is

A

NaNH2

129
Q

A 16 gram sample of a compound containing only copper and sulfur is decomposed to produce 12.8 grams of copper and 3.2 grams of sulfur. What is the empirical formula of the compounds

A

Cu2S

130
Q

NaOH + HCl —> NaCl + H2O

What is the total number of grams of H2O produced when 116 grams of the product, NaCl is formed?

A

36g

131
Q

N2(g) + 3H2(g) —> 2NH3(g)

What is the total number of liters of NH3 Formed when 20 liters of N2 react completely

A

40L

132
Q

C8H16 + 12O2 —> 8CO2 + 8H2O

How many moles of H2O are produced when 11.2 liters of C8H16 gas measure at STP react completely

A

4.00

133
Q

In the reaction N2 + 3H2 —> 2NH3 how many grams of H2 are needed to produce exactly 1 moles of Ammonia

A

3 gram

134
Q

4Al(s) + 3O2(g) —> 2Al2O3(s)

Calculate the gram molecular mass of Al2O3

A

102 grams

135
Q

4Al(s) + 3O2(g) —> 2Al2O3(s)

How many moles of Al are needed for the production of 3.00 moles of Al2O3

A

6 moles

136
Q

4Al(s) + 3O2(g) —> 2Al2O3(s)

Calculate the mass in grams of 3.00 moles of Al2O3

A

306 grams

137
Q

What is the percent by mass of water present in 1.0 mole of CaSO4 o 2H2O

A

36
____ = 21%
172

138
Q

What is the total number of grams of KCl (formula mass = 74.6) in 1 liter of .200 moles solution

A

14.9 grams

139
Q

What is the molarity of a solution of KNO3 (molecular mass = 101) that contains 404 grams of KNO3 in 2.00 liters of solution

A

2.00 M

140
Q

What is the total number of solute contained in .5 liters of 3.0 M HCl

A

1.5

141
Q

How many grams of ammonium chloride (gram formula mass = 53.5 g) are contained in .500L of 2.00 liters of solution

A

53.5 grams

142
Q

How many grams of KI are dissolved in 250 grams of a 20% solution

A

50 grams

143
Q

A solution will boil at the highest temperature when it contains 1 mole of nonvolatile solute dissolved in

A

250 grams of solvent

144
Q

When 2.00 moles of sugar (C6H12O6) are dissolved in 1.00 grams of water the boiling point of the resulting solution is closest to

A

101 C

145
Q

Which solute, when qdded to 1000 grams of water, will produce a solution with the highest boiling point

A

58 grams of NaCl

146
Q

The heat of reaction (Delta H) is equal to the

A

Heat content of the products minus the heat content of the reactants

147
Q

Review 126-130 In Packet

A

SKIP

148
Q

A(g) + B(g) –> C(g)

As the concentration of A(g) increases, the frequency of collisions of A(g) with B(g)

A

Increases

149
Q

In a gaseous system, temperature remaining constant, an increase in pressure will

A

Increase reaction rate

150
Q

In an gaseous system, temperature remaining constant, a decrease in pressure will

A

Decrease reaction rate

151
Q

As the surface area of the Zn(s) used in the reaction Zn(s) + 2HCl(aq) —> ZnCl2(aq) + H2(g) is increased, the rate of the reaction will

A

Increase

152
Q

The addition of a catalyst to a reaction will cause a change in the

A

Activation Energy

153
Q

CAT (Catalyst)—>

A

ACT (Activation energy)

154
Q

Delta H

A 
- = Exo 
\+ = Endo
155
Q

Delta S

A 
- = Less Disorder 
\+ = More Disorder
156
Q

Delta G

A 
- = Spontaneous 
\+ = Non Spontaneous
157
Q

The pair of changes would indicate that a reaction is endothermic but occurs spontaneously

A

A positive Delta H and a Negative Delta G

158
Q

A chemical reaction will always occur spontaneously if the reaction has

A

Negative Delta G

159
Q

BaSO4(s) = Ba+2(aq) + SO4-2(aq)

As the concentration of the SO4-2(aq) ions increases, at a constant temperature, the concentration of Cl- Ions

A

Decrease

160
Q

CH3COOH(aq) + H2O(l) = H3O+(aq) + CH3COO-(aq)

The addition of what ion will cause the decrease in the concentration of CH3COO-(aq)

A

H3O-

161
Q

N2(g) + 3H2(g) = 2NH3(g) + heat

Which change favors the formation of ammonia?

A

Increasing the concentration of N2(g)

162
Q

2SO2(g) + O2(g) = 2SO3(g)

As the pressure is increased at the constant temperature, the number of moles of SO3(g) produced will

A

Increase

163
Q

2A(g) + B(g) + 10 kcal = C(g)

Which condition would yield the most product

A

High temperature and high pressure

164
Q

What is the equilibrium equation for the reaction 3A(g) + B(g) = 2C

A

[A]3[B]

165
Q

Which of the following is the correct equilibrium expression for
4NH3(g) + 7O2(g) = 4NO2(g) + 6H2O(g)

A

[O2]7[NH3]4

166
Q

A + B =AB

The greatest amount of AB would be produced if the equilibrium constant of the reaction is eqaul to

A

1.0x10^5

167
Q

AgI(s) = Ag+(aq) + I-(aq)

Which of the following is the correct solubility product constant expression for the reaction

A

Ksp = [Ag+][I-]

168
Q

C(s) + CO2(g) + heat —-> 2CO2(g)

Which stress on the system would favor production of CO(g)

A

An increase Pressure

169
Q

A2(g) + 3B2(g) = 2AB3(g) + heat
State two stresses that could be applied to this system that would cause this equilibrium to shift to the right. Explain why each stress would cause a shift in the equilibrium

A

Temperature and Pressure because those can change the state of the substance

170
Q

What is the pH of a solution that has an OH- ion concentration of 1x10^-9 mole per liter (Kw = 1 x 10^-14)

A

5

171
Q

What is the pH of a .00001 molar HCl solution

A

5

172
Q

If the OH- equals 1 x 10-10 at 298 k for a given soltuion, the H+ of the solution equals

A

1 x 10-4

173
Q

What s the H+ ion concentration of an aqueous solution that has a pH of 11

A

1 x 10-11 mol/L

174
Q

The H3O+ ion concentration of a solution is 1x10-5 mole per liter. This solution is

A

Acidic and has a pH of 5

175
Q

Which equation represents a neutralization reaction

A

Any equation with the product of NaCl + H2O

176
Q

What is a neutralization reaction

A

A reaction resulting in NaCl + H2O

177
Q

If 100 milliliters of .75 M HCl is required to exactly neutralize 50 milliliters of KOH, what is the concentration of the base?

A

1.5 M

178
Q

If you see exactly neutralized in an equation what do you do?

A

Multiply the first two numbers you see and then divide it by the last

179
Q

In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:
Write a balance equation for HNO3 and LiOH

A

HNO3 + LiOH —> H2O + LiNO3

180
Q

In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:If 50 milliliters of .50 M LiOH is required to exactly neutralize 100 milliliters of an HNO3 solution, what is the molarity of the HNO3 solution?

A

.25 M

181
Q

In the laboratory, a student titrated HNO3 with .50 M LiOH until the indicator changed from colorless to pink:What indicator was used in the titration

A

Moles

182
Q

What color does Phenothaline turn in Acid

A

Colorless

183
Q

What color does Phenothaline turn in Base

A

Pink

184
Q

What color does Litmus turn in Acid

A

Red

185
Q

What color does Litmus turn in Base

A

Blue

186
Q

Arrhenius Acid

A

Gives H+

187
Q

Arrhenius Base

A

Gives OH-

188
Q

Bronsted Lowry Acid

A

Gives H+ (Proton)

189
Q

Bronsted Lowry Base

A

Accepts H+ )Proton

190
Q

Lewis Acid

A

e- pair Acceptor

191
Q

Lewis Base

A

e- pair Donor

192
Q

How do you know what the Bronsted Lowry Bases are

A

Compare the two similar elements on each side and the one with the less H’s is the base

193
Q

In a redox reaction there is conservation of

A

Both mass and charge (everything)

194
Q

Review 161 and 162 In Packet

A

SKIP

195
Q

How do you know which substance is being oxidized?

A

Pick the first element in the equation or the metal

196
Q

How do you know a reaction is redox

A

Look for a single element and not compounds

197
Q

If there is no metal in the equation how do you know what was oxidized?

A

Look for an increase in ions

198
Q

0
e-
-1

A

Beta

199
Q

4
He
2

A

Alpha

200
Q

0
e-

1

A

Positron

201
Q

0
V
0

A

Gamma

202
Q

1

A

Beta

203
Q

2

A

Gamma

204
Q

3

A

Positron and Alpha

205
Q

To solve a Nuclear Problem what do you do?

A

Equal Everything

206
Q

What is the equation for Decay

A

TGB
——- = Decay
HL

207
Q

At the end of 12 days 1/4 of an original sample of a radioactive element remains. What is the half life of the element

A

6 Days

208
Q

An Original Sample of a radioisotope has a mass of 10 grams. After 2 days, 5 grams of the radioisotope remains unchanged. What is the half life of the radioisotope

A

2 Days

209
Q

In 6.20 Hours a 100 gram sample of Ag-112 decays to 25 grams. What is the half life of Ag-112

A

3.10 Hours

210
Q

The half life of carbon-14 is 5730 years. What fraction of a 1 gram sample of carbon-14 would remain after 17190 years?

A

1/8

211
Q 
Which quantity expresses the sum of the values below to the proper degree of precision 
 2.1
33.566
\+12.22
--------------
A

47.9g

212
Q

Using the rules for sig fig, the sum of .027g and .0023 grams should be expressed

A

.029

213
Q

What is the product of (2.324 cm x 1.11 cm) expressed to the correct sig fig

A

2.58 cm2

214
Q

During a titration, a student used 50 milliliters of .1 M acid. How many moles of acid, expressed to proper significance, were used?

A

.005

215
Q

What is the number 215 expressed in proper scientific notation with the correct number of sig fig,

A

2.150 x 102

216
Q

A student investigated the physical and chemical properties of a sample of an unknown gas ans then identified the gas. Which of the following statements represents a conclusion rather than an experimental observation

A

The gas is carbon dioxide

217
Q

What is the number 2.1 x 10^3 expressed in conventional form with the proper number of sig fig

A

2100

218
Q

The solid block shows below has a mass of 146 and a length and width of 3 and a height of 6 what is the density

A

2.7

219
Q

The process of filtration is preformed in the laboratory to

A

Separate insoluble substances in an aqueous mixture

220
Q

Linear CH4

A

CO2

221
Q

Tetrahedral

A

CH4

222
Q

Bent

A

H2O

223
Q

Trigonal Pyramidal

A

NH3

224
Q

NP

A

LDF

225
Q

P

A

DD

226
Q

Equation for moles

A

C

227
Q

Equation for Grams

A

C (mass)

228
Q

Equation for Liters

A

C (22.4)

229
Q

Equation for Molecules

A

C (6.02x10^23)

230
Q

When in Doubt

A

PV=nRT

231
Q

What is another equation for Grams

A

LP

232
Q

What is another equation for Density

A

P

Chemistry 2013-2014 (20 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions