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Honors Chemisty > Final Exam > Flashcards

Final Exam Flashcards

1
Q

Which of the following defines a hypothesis?

A

A hypothesis is a tentatively accepted explanation of the facts.

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2
Q

Why is Antoine Lavoisier considered by some to be the “father” of chemistry?

A

He was the first to apply quantitative measurements to a chemical problem. He weighed out the reactants and the products of a chemical reaction before and after the reaction. What he learned became the law of conservation of matter.

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3
Q

“Melting point” is not a(n) _____________________.

A

qualitative property of a substance

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4
Q

Calcium carbonate is a compound that can decompose into carbon dioxide and calcium oxide. Carbon dioxide, in turn, is made up of the elements carbon and oxygen. What needs to happen to a compound in order for it to be broken down into either elements or simpler compounds?

A

The compound needs to undergo a chemical reaction.

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5
Q

How many neutrons are in the nucleus of an atom of calcium-43?

A

23

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6
Q

A new stable element with an atomic number of 120 and an atomic mass of 246 is created in a particle accelerator. Enough of this element is created to determine that it combines with chlorine in a 1:2 ratio. Element 120 should be placed in the same group as _____ on the periodic table.

A

beryllium (Be)

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7
Q

What is the coefficient for water in the properly balanced equation for the combustion of butane and oxygen gas to form carbon dioxide gas and water according to the equation:

C4H10 + O2 → CO2 + H2O

A

10

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8
Q

What are the conversion factors that would be used to determine the number of atoms of oxygen in 0.23 moles of silver nitrate (AgNO3 )?

A
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9
Q

A reaction has an expected yield of 30.5 grams. What is the percent yield if performing the reaction produced 29.6 grams of product?

A

97.0 percent

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10
Q

The following reaction is of which type?

2KClO3(s) —> 2KCl(s) + 3O2(g)

A

oxidation-reduction reaction

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11
Q

If 145.0 mL of 0.350 M lithium hydroxide is required to titrate 35.0 mL of an unknown monoprotic acid, what is the molar concentration of the unknown acid?

A

1.45 M

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12
Q

A 2.32 L balloon contains helium at 1.00 atm and 25°C. How many grams of helium are contained in the balloon?

A

0.380 g He

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13
Q

What is the root-mean-square speed (urms) in m/s for ethane (C2H6) at 298 K?
R = 8.314 J/(mol•K), and 1 J = 1 kg•m2/s2.

A

497 m/s

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14
Q

What are the two ways that energy can be transferred between the system and the surroundings?

A

work and heat

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15
Q

The molar heat of neutralization of a strong acid and a strong base is determined by mixing 50.0 mL of 1.0 M HCl with 50.0 mL of 1.1 M NaOH in a coffee cup calorimeter. The initial temperatures of two solutions was 25.32°C and the final temperature inside the calorimeter was 31.43°C. What is the molar heat of neutralization? Assume that the specific heat capacity of the solution is identical to water and the density is 1.00 g / mL.

A

−51.6 kJ / mol

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16
Q

When filling multiple orbitals that have the same energy (called degenerate orbitals), two electrons are placed in different orbitals rather than paired in a single orbital. This is an example of which of the following?

A

Hund’s rule

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17
Q

Moving accross a row in the periodic table from left to right, which of the following quantities increases?

A

electron affinity and ionization energy

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18
Q

In the following chemical reaction, what is being reduced?

2K(s) + 2H2O(l) —> H2(g) + 2K+(aq) + 2OH-(aq)

A

water molecule

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19
Q

The electron configuration for vanadium is 1s22s22p63s23p64s23d3.
How many valence electrons does vanadium have?

A

5

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20
Q

Which of the following is the correct Lewis dot structure of nitric acid, HNO3?

A
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21
Q

Which of the following shows (in the correct order) the oxidation numbers for phosphorous (P) and oxygen (O) in the polyatomic ion PO43−?

A

+5, −2

22
Q

Which of the following does not play a role in determining when a phase change occurs?

A

the amount of compound

23
Q

What is a saturated solution?

A

A saturated solution is a solution that contains the maximum possible concentration of solute (at a given temperature).

24
Q

A certain type of sugar dissolves in water, but the solution created does not conduct electricity. Therefore, the sugar does not form ions when dissolved in solution. When 10.0 g of this sugar are dissolved in 25.0 g of water, the freezing point of the solution is −5.0°C. If the freezing point depression constant for water (Kf) is 1.86°C/m, what is the molar mass of the sugar?

A

150 g/mol

25
Q

A _____ is a gas dispersed in a liquid.

A

foam

26
Q

Using the following data for the reaction 2NO2(g) + F2(g) → 2FNO2(g)
what are the values of m, n, and k in the rate law rate = k[ NO2 ]m [ F2 ]n?

A

m = 1, n = 1, k = 1.6 M −1s−1

27
Q

Which of the following expresses the half-life for a first-order reaction?

A

t1/2 = In 2/ k

28
Q

In the Arrhenius equation the “A” is:

A

the frequency factor

29
Q

For many reactions involving enzymes (E) reacting with substrates (S) to form products (P), steady state approximations can be applied to derive the rate law:

Which of the following shows the rate law when the concentration of substrate is very large in relation to the k values?

A

rate = kobs[E]0

30
Q

Which reaction shown below involves a heterogeneous catalyst?

A

2NO(g) ——-> N2(g) + O2(g)

31
Q

If the value of the equilibrium constant with regard to concentration (Kc ) is found to be 2.54 × 106 at 30°C, what is the value of the eqilibrium constant with regard to pressure?
(R = 0.0821 L • atm / mol • K)

PCl3(g) + Cl2(g) PCl5(g)

A

1.02 × 105

32
Q

In the following equation for the dissociation of sulfuric acid in water, identify the conjugate bases.

H2SO4(aq) + H2O(l) —> HSO4-(aq) + H3O+(aq)

A

HSO4- and H2O

33
Q

What is the pH of a 0.10 M solution of the weak base methylamine (NH2CH3 )?
(Kb = 4.4 × 10−4 )

A

11.82

34
Q

Consider the following reaction between nitrous and ammonia:

HNO2(aq) + NH3(aq) NH4NO2(aq)

Ka = 4.5 x 10^-4
Kb = 1.8 x 10^-5

What is the equilibrium constant for this reaction?

A

8.1 × 10^5

35
Q

The value for Kf for Ag(NH3)2+ is 1.7 × 107. What is the dissociation constant for this complex ion?

A

5.9 x 10–8

36
Q

Which acid contains the most electronegative halogen?

A

hydrofluoric acid

37
Q

Considering hybridization effects, which of these organic compounds must be the strongest acid?

A

The alkyne

38
Q

What happens when a bond is broken heterolytically?

A

One atom gets a pair of electrons.

39
Q

Refer to the potential energy diagram below. Which of the following statements concerning this reaction is TRUE?

A

This reaction is reversible.

40
Q

What is entropy?

A

a thermodynamic quantity that is a measure of the randomness or disorder in a system

41
Q

At what temperature does ΔH = TΔS for the phase change of liquid water to gaseous water at 1 atm?

A

373 K

42
Q

Which of the following is the properly balanced equation for the reaction of nitrous acid and iodide ion?

HNO2(aq) + I-1(aq) —> NO(g) + I2(s)

A

2H+(aq) + 2HNO2(aq) + 2 I-2(aq) —> 2NO(g) + 2H2O(l) + I2(s)

43
Q

Manganese can be found in many oxidation states. Which of the following is the strongest oxidant?

MnO4−, MnO2, MnCl2, Mn

A

MnO4−

44
Q 
All of the following batteries use zinc metal at the anode except
I. 	lead storage battery
II. 	Leclanché dry cell battery
III. 	alkaline battery
IV. 	mercury battery
V. 	lithium battery
A

I and V only

45
Q

In the formation of rust in aerobic conditions, what is the role of the iron metal?

A

anode and conduit for electrons

46
Q

Which of the following is produced at the cathode of an electrolytic cell containing a 1.0 M solution of sodium chloride?

A

hydrogen gas

47
Q

The energy gap between the valence band and the conduction band in silicon is 100 kJ/mol. The energy gap for germanium will be:

A

smaller

48
Q

Which of the following compounds cannot exist?

A

Na(OH)2

49
Q

What is the complimentary DNA strand for the following sequence?

T–T–C–G–A–C–G–A

A

A–A–G–C–T–G–C–T

50
Q

Which of the following shows the alcohol called ethanol?

A

Honors Chemisty (145 decks)

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