Deck 12: Reaction Rates and Chemical Equilibrium

Question 1

Identify the intermediate in the following two-step reaction. Cr²⁺(aq)+ Sn⁴⁺(aq)⇌ Cr³⁺(aq)+ Sn³⁺(aq)Cr²⁺(aq)+ Sn³+(aq)→ Cr³+(aq)+ Sn²⁺(aq)

A)Sn³⁺(aq)
B)Sn⁴⁺(aq)
C)Sn²⁺(aq)
D)Cr²⁺(aq)
E)Cr³⁺(aq)

Answer 1

Sn³⁺(aq)

Question 2

Which of the following statements regarding catalysts is incorrect?

A)A catalyst increases the rate of a reaction by giving the reaction an alternate pathway with a lower activation energy.
B)Catalysts need not be present in large amounts because they are regenerated during the reaction.
C)Enzymes act as catalysts in our bodies.
D)In a chemical reaction, the catalyst is shown on the reactant side of the equation.
E)The shape of an active site on an enzyme is unique, allowing it to react with only one substrate.

Answer 2

In a chemical reaction, the catalyst is shown on the reactant side of the equation.

Question 3

Which of the following changes will increase the fraction of collisions that are effective collisions?

A)increasing the temperature
B)increasing the concentration of the reactants
C)decreasing the concentration of the reactants
D)increasing the surface area of the reactants
E)All of these choices are correct.

Answer 3

increasing the temperature

Question 4

Factors that influence reaction rates include all of the following except the

A)magnitude of the equilibrium constant.
B)reaction temperature.
C)presence of a catalyst.
D)size of solid reactant particles.
E)concentration of reactants.

Question 5

The rate of a reaction can be increased by all of the following except

A)increasing the temperature.
B)increasing the concentration of the reactants.
C)increasing the surface area of the reactants.
D)adding a catalyst.
E)increasing the volume of the reaction vessel.

Question 6

A catalyst speeds up a chemical reaction by

A)providing an alternate reaction pathway.
B)increasing the activation energy.
C)shifting the equilibrium.
D)increasing the heat of the reaction.
E)decreasing the heat of the reaction.

Question 7

Which of the following will not increase the rate of a reaction?

A)decreasing the temperature
B)decreasing the concentration of the reactants
C)decreasing the surface area of the reactants
D)removing a catalyst
E)All of these will not increase the rate of a reaction.

Question 8

Which of the following statements regarding catalysts is incorrect?

A)A catalyst increases the rate of a reaction by giving the reaction an alternate pathway with lower activation energy.
B)A catalyst is formed temporarily in an early step of a reaction.
C)Most enzyme catalysts are large protein molecules.
D)In a chemical equation the catalyst is shown above the reaction arrow of the equation.
E)The shape of an active site on an enzyme is unique, allowing it to react with only one substrate.

Question 9

Identify any intermediates in the following three-step reaction: H₂C=CH₂ + H₃O⁺ → H₃C=CH₂⁺ + H₂O
H₃C=CH₂⁺ + H₂O → CH₃CH₂OH₂⁺
CH₃CH₂OH₂⁺ + H₂O → CH₃CH₂OH + H₃O⁺

A)H₃O⁺ is an intermediate.
B)H₃C=CH₂⁺ is an intermediate.
C)H₃C=CH₂⁺, CH₃CH₂OH₂⁺, and H₂O are intermediates.
D)CH₃CH₂OH₂⁺ is an intermediate.
E)H₂O is an intermediate.

Question 10

In a chemical reaction at constant temperature, the addition of a catalyst

A)affects the equilibrium constant.
B)increases the average kinetic energy of the reactants.
C)provides an alternate reaction pathway with a different activation energy.
D)decreases the energy released in the chemical reaction.
E)increases the concentration of the products at equilibrium.

Question 11

Identify any intermediates or catalysts in the following two-step reaction: Cu²⁺ + H₂ → CuH⁺ + H⁺ CuH⁺ + H⁺ + H₂C=CH₂ → Cu²⁺ + H₃C-CH₃

A)CuH⁺ is an intermediate.
B)Cu²⁺ is a catalyst, H⁺ is an intermediate.
C)Cu²+ is a catalyst, CuH⁺ is an intermediate.
D)Cu²+ is a catalyst, CuH⁺ and H⁺ are intermediates.
E)CuH⁺ and H⁺ are catalysts, Cu²⁺ is an intermediate.

Question 12

Identify the intermediate(s)in the following two-step reaction. O₃(g)⇌ O₂(g)+ O(g)O(g)+ O₃(g)→ 2O₂(g)

A)O(g)
B)O₃(g)
C)O₂(g)
D)O2(g)and O(g)

Question 13

Which of the following changes will increase the average kinetic energy of the reactants?

A)increasing the surface area of the reactants
B)increasing the concentration of the reactants
C)adding a catalyst
D)increasing the temperature
E)none of these choices

Question 14

According to collision theory, the increase in the rate constant with increasing temperature is due mostly to the fact that

A)the activation energy decreases with increasing temperature.
B)the fraction of the collisions having sufficient energy to react increases with increasing temperature.
C)the pressure of the reactants increases with increasing temperature.
D)the heat change for most reactions is negative.
E)the fraction of the collisions that have the proper orientation for reaction increases with increasing temperature.

Question 15

Identify an intermediate in the following two-step reaction. Sn²⁺ + Fe³⁺ → Sn³⁺ + Fe²⁺ Sn³⁺ + Fe³⁺ → Sn⁴⁺ + Fe²⁺

A)Sn²⁺
B)Fe³⁺
C)Sn³⁺
D)Fe²⁺
E)Sn⁴⁺

Question 16

Which of the images shows the molecules in a proper orientation for an effective collision for the following reaction? 2HI(g)→ H₂(g)+ I₂(g)

A)I only
B)II only
C)III only
D)I and II
E)II and III

Question 17

Identify the intermediate(s)in the following three-step reaction. Cl₂(g)⇌ 2Cl(g)CHCl₃(g)+ Cl(g)→ HCl(g)+ CCl₃(g)CCl₃(g)+ Cl(g)→ CCl₄(g)

A)CHCl₃(g)
B)HCl(g)
C)Cl₂(g)
D)Cl(g)
E)Cl(g)and CCl₃(g)

Question 18

Identify any intermediates or catalysts in the following two-step reaction: H₂O₂ + 2Br⁻ + 2H⁺→ 2H₂O + Br₂ H₂O₂ + Br₂ → 2H⁺ + O₂ + 2Br⁻

A)H₂O₂ is an intermediate.
B)H₂O₂ is a catalyst, Br⁻ is an intermediate.
C)Br⁻ is a catalyst, Br₂ is an intermediate.
D)H⁺ is a catalyst.
E)Br⁻ and H⁺ are catalysts, Br₂ is an intermediate.

Question 19

Identify any intermediates or catalysts in the following two-step reaction: S₂O₈²⁻ + I⁻ → 2SO₄²⁻ + I⁺ I^{+ +} I⁻ → I₂

A)S₂O₈²⁻ is an intermediate.
B)S₂O₈²⁻ is a catalyst.
C)I⁻ is a catalyst.
D)I⁺ is an intermediate.
E)SO₄²⁻ is a catalyst.

Question 20

The kinetics of a reaction is studied at 25ºC and at 50ºC. Which of the following statements is correct?

A)The rate of the reaction at 50ºC will be lower than the rate at 25ºC, since the molecules will be moving too fast to collide effectively.
B)The rate of the reaction at 50ºC will be twice that of the rate at 25ºC, since the temperature has doubled.
C)The rate of the reaction at 50ºC will be greater than the rate at 25ºC, since the activation energy will be lower at the higher temperature.
D)The rate of the reaction at 50ºC will be greater than the rate at 25ºC, since a greater fraction of the molecules will possess sufficient energy to react at the higher temperature.
E)None of these statements is correct.

Question 21

When a chemical system has reached equilibrium

A)the forward and reverse reactions have stopped.
B)the rate of the forward reaction is greater than the rate of the reverse reaction.
C)the rate of the forward reaction is less than the rate of the reverse reaction.
D)the rate of the forward reaction is equal to the rate of the reverse reaction.
E)the equilibrium constant has reached a minimum.

Question 22

Identify the catalyst in the following three-step process for the decomposition of ozone. O₃(g)⇌ O₂(g)+ O(g)NO(g)+ O₃(g)→ NO₂(g)+ O₂(g)O(g)+ NO₂(g)→ O₂(g)+ NO(g)

A)O(g)
B)O₃(g)
C)O₂(g)
D)NO(g)
E)NO₂(g)

Question 23

Given that the following reaction is exothermic, which of the following sets of changes would cause the following system at equilibrium to shift to increase the number of N₂O₄(g)molecules? 2NO₂(g)⇌ N₂O₄(g)What observation would indicate that the reaction is at equilibrium in a closed container?

A)Increasing container volume and increasing temperature
B)Increasing container volume and decreasing temperature
C)Decreasing container volume and increasing temperature
D)Decreasing container volume and decreasing temperature
E)Changing volume or temperature will not affect the number of gas molecules present at equilibrium

Question 24

Activated complexes are

A)stable molecules that are formed during an early step of a reaction, and consumed in a later step.
B)materials which act to increase the rate of a reaction without themselves being consumed.
C)substances which form during a reaction that have a definite, well-known structure.
D)short-lived, high-energy chemical species that are produced during a reaction.
E)a molecular species with normal chemical bonds that is produced during a reaction.

Question 25

Consider the following reaction carried out in a sealed container: 2SO₃(g)⇌ 2SO₂(g)+ O₂(g)A state of equilibrium cannot be reached if the container initially contains

A)SO₃ only.
B)O₂ only.
C)SO₂ and O₂ only.
D)SO₃ and O₂ only.
E)SO₃ , SO₂ and O₂.

Question 26

For the reaction, CoO(s)+ H₂(g)⇌ Co(s)+ H₂O(g), at 550°C, the value of the equilibrium constant, K, is 67. The equilibrium constant expression is

A)
B)
C)
D)
E)

Question 27

Identify the catalyst in the following three-step reaction. NO(g)+ O₂(g)→ NO₃(g)NO₃(g)+ NO(g)→ 2NO₂(g)NO₂(g)+ SO₂(g)→ NO(g)+ SO₃(g)

A)SO₂(g)
B)NO₃(g)
C)O₂(g)
D)NO(g)
E)NO₂(g)

Question 28

Consider the following reaction carried out in a sealed container: N₂(g)+ 3H₂(g)⇌ 2NH₃(g)A state of equilibrium cannot be reached if the container initially contains

A)NH₃ only.
B)N₂ only.
C)NH₃ and N₂ only.
D)NH₃, N₂, and H₂.

Question 29

In order to write the equilibrium constant expression for a reaction, you must

A)know the mechanism for the reaction.
B)know the rate of the forward and reverse reactions.
C)know the concentrations of all reactants and products.
D)have the balanced chemical equation for the reaction.
E)know the conditions of pressure, temperature, and concentration for the system.

Question 30

Select the correct equilibrium constant expression for the following reaction: H₂(g)+ I₂(g)⇌ 2HI(g)

A)
B)
C)
D)
E)

Question 31

Consider the following reaction at equilibrium at a given temperature: 2NH₃(g)+ heat ⇌ N₂(g)+ 3H₂(g)Which of the following will cause the value of the equilibrium constant for this process to change?

A)Adding more NH₃ to the system, with the volume held constant.
B)Increasing the pressure by reducing the volume of the system.
C)Adding an effective catalyst for the process.
D)Raising the temperature of the system.
E)Adding some neon to the system.

Question 32

Select the correct equilibrium constant expression for the reaction: CH₄(g)+ 2H₂S(g)⇌ CS₂(g)+ 4H₂(g)

A)
B)
C)
D)K_eq = [CS₂][H₂]⁴ − [CH₄][H₂S]²
E)K_eq = [CS₂][H₂]⁴ + [CH₄][H₂S]²

Question 33

What is the balanced chemical equation that corresponds to the equilibrium constant expression (assuming a homogeneous equilibrium in the gas state)?

A)A₂ + B ⇌ C
B)2A + B ⇌ C
C)C ⇌ A + B
D)C ⇌ A₂ + B
E)C ⇌ 2A + B

Question 34

What is the balanced chemical equation that corresponds to the equilibrium constant expression (assuming a homogeneous equilibrium in the gas state)?

A)A + B ⇌ C
B)2A + 2B ⇌ C
C)C ⇌ A + B
D)A + B ⇌ 2C
E)2C ⇌ A + B

Question 35

What is the balanced chemical equation that corresponds to the equilibrium constant expression (assuming a homogeneous equilibrium in the gas state)?

A)A + B₂ ⇌ C + D
B)A + 2B ⇌ C + D
C)C + D ⇌ A + B
D)C + D ⇌ A + B₂
E)C + D ⇌ A + 2B

Question 36

Consider the following reaction carried out in a sealed container: N₂(g)+ 3H₂(g)⇌ 2NH₃(g)A state of equilibrium can be reached if the container initially contains

A)NH₃ only.
B)N₂ and H₂ only.
C)NH₃ and N₂ only.
D)NH₃, N₂, and H₂.
E)any of these combinations of reactants and products.

Question 37

Given that evaporation is an endothermic process, which of the following sets of changes would cause the following system at equilibrium to shift to increase the number of I₂ molecules in the gas phase? I₂(s)⇌ I₂(g)

A)Increasing container volume and increasing temperature
B)Increasing container volume and decreasing temperature
C)Decreasing container volume and increasing temperature
D)Decreasing container volume and decreasing temperature
E)Changing volume or temperature will not affect the number of gas molecules present at equilibrium

Question 38

Select the correct equilibrium constant expression for the reaction 4NH₃(g)+ 3O₂(g)⇌ 2N₂(g)+ 6H₂O(g)

A)K_eq =
B)K_eq =
C)K_eq =
D)K_eq = [N₂]²[H₂O]⁶ − [NH₃]⁴[O₂]³
E)K_eq = [N₂]²[H₂O]⁶ + [NH₃]⁴[O₂]³

Question 39

Consider the following reaction carried out in a sealed container: 2SO₃(g)⇌ 2SO₂(g)+ O₂(g)A state of equilibrium can be reached if the container initially contains

A)SO₃ only.
B)SO₂ and O₂ only.
C)SO₃ and O₂ only.
D)SO₃, SO₂, and O₂.
E)any of these combinations of reactants and products.

Question 40

The graph shows the change in concentrations of the reactant and product as a reaction proceeds. At what point is equilibrium first reached?

A)I
B)II
C)III
D)IV
E)V

Question 41

Which equilibrium constant represents a reaction that is reactant favored?

A)K_eq = 0.025
B)K_eq = 5.2
C)K_eq = 8.4 x 10^-5
D)K_eq = 6.3 x 10⁵
E)not enough information

Question 42

Consider the reaction CO(g)+ H₂O(g)⇌CO₂(g)+ H₂(g), represented by the following diagram: What is the composition of this system when the reaction reaches equilibrium?

A)3 CO, 3 H₂O, 7 CO₂, 7 H₂
B)1 CO, 1 H₂O, 4 CO₂, 4 H₂
C)2 CO, 2 H₂O, 8 CO₂, 8 H₂
D)8 CO, 8 H₂O, 2 CO₂, 2 H₂
E)4 CO, 6 H₂O, 4 CO₂, 6 H₂

Question 43

The value of the equilibrium constant for the following reaction is 0.200 at a given temperature 2HI(g)⇌ H₂(g)+ I₂(g)Find the value of the equilibrium constant for the reaction: H₂(g)+ I₂(g)⇌ 2HI(g)

A)0.200
B)0.0400
C)5.00
D)0.500
E)-0.200

Question 44

The reaction S₂Cl₂(g)+ Cl₂(g)⇌ 2SCl₂(g)has an equilibrium constant of K = 8. The image shows a partially reacted system. What is the composition of this system when the reaction reaches equilibrium?

A)1 S₂Cl₂, 3 Cl₂, 10 SCl₂
B)2 S₂Cl₂, 4 Cl₂, 8 SCl₂
C)3 S₂Cl₂, 5 Cl₂, 6 SCl₂
D)4 S₂Cl₂, 6 Cl₂, 4 SCl₂
E)5 S₂Cl₂, 7 Cl₂, 2 SCl₂

Question 45

Consider the following reaction at a specific temperature: 2HI(g)⇌ H₂(g)+ I₂(g)If [HI] = 0.447 M, [H₂] = 0.200 M, and [I₂] = 0.200 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

A)0.200
B)0.0400
C)0.0895
D)0.407
E)0.0447

Question 46

The value of the equilibrium constant for the following reaction is 4.0 at a given temperature: A ⇌ 2B What is the value of the equilibrium constant for the reaction 2B ⇌ A?

A)4.0
B)0.25
C)16
D)0.062
E)-4.0

Question 47

Consider the following reaction at a specific temperature: 2HI(g)⇌ H₂(g)+ I₂(g)If [HI] = 1.17 M, [H₂] = 1.37 M, and [I₂] = 0.100 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

A)1.17
B)1.26
C)0.100
D)10.0
E)8.54

Question 48

For a given reaction, which of the following statements can be made about the value of the equilibrium constant?

A)It always remains the same.
B)It increases when the concentration of one of the products is increased.
C)It increases when the concentration of one of the reactants is increased.
D)It changes when temperature is changed.
E)It can be changed by addition of a catalyst.

Question 49

Consider the following reaction at a specific temperature: CO₂(g)+ H₂(g)CO(g)+ H₂O(g)If [CO₂] = 3.60 M, [H₂] = 4.00 M, [CO] = 1.18 M, and [H₂O] = 2.40 M at equilibrium, calculate the value of the equilibrium ⇌ instant under these conditions.

A)0.471
B)0.197
C)5.08
D)2.12
E)0.444

Question 50

The value of the equilibrium constant for the following reaction is 224 at a given temperature: N₂(g)+ 3H₂(g)⇌ 2NH₃(g)If [N₂] = 10.0 M, [H₂] = 10.0 M, and [NH₃] = 10.0 M, determine if the reaction is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

A)The reaction is at equilibrium.
B)The reaction is not at equilibrium, it will shift to the left.
C)The reaction is not at equilibrium, it will shift to the right.
D)It is not possible to tell if the reaction is at equilibrium.
E)To reach equilibrium, the value of K_eq must change.

Question 51

Which of the following statements is correct for a reaction in which K_eq << 1?

A)The forward reaction is faster than the reverse reaction.
B)The reverse reaction is faster than the forward reaction.
C)There are more products than reactants at equilibrium.
D)There are more reactants than products at equilibrium.
E)None of these statements is correct.

Question 52

The value of the equilibrium constant for the following reaction is 16 at a given temperature: CO(g)+ H₂O(g)⇌ CO₂(g)+ H₂(g)If [CO] = 4.0 M, [H₂O] = 4.0 M, [CO₂] = 4.0 M, and [H₂] = 4.0 M, determine if the reaction is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

A)The reaction is at equilibrium.
B)The reaction is not at equilibrium, it will shift to the left.
C)The reaction is not at equilibrium, it will shift to the right.
D)It is not possible to tell if the reaction is at equilibrium.
E)To reach equilibrium, the value of K_eq must change.

Question 53

The value of the equilibrium constant for the following reaction is 0.200 at a given temperature: 2HI(g)⇌ H₂(g)+ I₂(g)If [HI] = 0.200 M, [H₂] = 0.200 M, and [I₂] = 0.200 M, determine if the reaction is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

A)The reaction is at equilibrium.
B)The reaction is not at equilibrium, it will shift to the left.
C)The reaction is not at equilibrium, it will shift to the right.
D)It is not possible to tell if the reaction is at equilibrium.
E)To reach equilibrium, the value of K_eq must change.

Question 54

The value of the equilibrium constant for the following reaction is 16 at a given temperature: CO(g)+ H₂O(g)⇌ CO₂(g)+ H₂(g)Find the value of the equilibrium constant for the reaction: H₂(g)+ CO₂(g)⇌ CO(g)+ H₂O(g)

A)16
B)4.0
C)8.0
D)0.062
E)-16

Question 55

Consider the reaction and the value of its equilibrium constant: S₂Cl₂(g)+ Cl₂(g)⇌ 2SCl₂(g)K_eq = 4 Examine the figure, and determine if the system is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

A)The reaction is at equilibrium.
B)The reaction is not at equilibrium; it will shift to the left.
C)The reaction is not at equilibrium; it will shift to the right.
D)It is not possible to tell if the reaction is at equilibrium.
E)To reach equilibrium, the value of K_eq must change.

Question 56

Which equilibrium constant represents a reaction that is product favored?

A)K_eq = 0.025
B)K_eq = 5.2
C)K_eq = 8.4 x 10^-5
D)K_eq = 6.3 x 10⁵
E)not enough information

Question 57

The value of the equilibrium constant for the following reaction is 16 at a given temperature: 2A ⇌ B What is the value of the equilibrium constant for the reaction B ⇌ 2A?

A)5.0
B)25
C)0.20
D)0.040
E)-5.0

Question 58

The value of the equilibrium constant for the following reaction is 224 at a given temperature: N₂(g)+ 3H₂(g)⇌ 2NH₃(g)Find the value of the equilibrium constant for the reaction: 2NH₃(g)⇌ N₂(g)+ 3H₂(g)

A)224
B)0.00446
C)448
D)5.02 x 10⁴
E)-224

Question 59

Which of the following statements is correct for a reaction in which K_eq >> 1?

A)The forward reaction is faster than the reverse reaction.
B)The reverse reaction is faster than the forward reaction.
C)There are more products than reactants at equilibrium.
D)There are more reactants than products at equilibrium.
E)None of these statements is correct.

Question 60

Consider the following reaction at a specific temperature: CO₂(g)+ H₂(g)⇌ CO(g)+ H₂O(g)If [CO₂] = 1.80 M, [H₂] = 2.00 M, [CO] = 0.590 M, and [H₂O] = 1.20 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

A)0.471
B)0.197
C)5.08
D)2.12
E)0.444

Question 61

For the reaction CO(g)+ 3H₂(g)⇌ CH₄(g)+ H₂O(g)q = −206 kJ What conditions favor maximum conversion of reactants to products?

A)low pressure and low temperature
B)removal of H₂(g)and low temperature
C)high pressure and high temperature
D)high pressure and low temperature
E)low pressure and high temperature

Question 62

Consider the following reaction and the value of its equilibrium constant: FeO(s)+ CO(g)⇌ Fe(s)+ CO₂(g)K_eq = 0.67 If the equilibrium concentration of CO is measured at 0.50 M, what is the equilibrium concentration of CO₂?

A)0.50 M
B)1.2 M
C)0.34 M
D)0.27 M
E)1.3 M

Question 63

Write the equilibrium constant expression for the following reaction: Pb²⁺(aq)+ 2Cl^-(aq)⇌ PbCl₂(s)

A)
B)K_eq = [Pb²⁺][ Cl⁻]²
C)
D)
E)

Question 64

Write the equilibrium constant expression for the following reaction: PbCl₂(s)⇌ Pb²⁺(aq)+ 2Cl^-(aq)

A)
B)K_eq = [Pb²⁺][ Cl⁻]²
C)
D)
E)

Question 65

Write the equilibrium constant expression for the following reaction: CH₃NH₂(g)+ H₂O(l)⇌ CH₃NH₃⁺(aq)+ OH^-(aq)

A)K_eq = [CH₃NH₃⁺][OH⁻]
B)
C)
D)
E)

Question 66

Write the equilibrium constant expression for the following reaction: 2HgO(s)⇌ 2Hg(l)+ O₂(g)

A)
B)
C)K_eq = [O₂]
D)K_eq = [Hg]²[O₂]
E)

Question 67

Consider the following system at equilibrium: CH₄(g)+ 2H₂O(g)⇌ CO₂(g)+ 4H₂(g)What change will cause the equilibrium to shift to form more H₂?

A)increase [H₂]
B)decrease [H₂O]
C)decrease the volume of the reaction vessel
D)decrease [CH₄]
E)decrease [CO₂]

Question 68

Consider the reaction 3Fe(s)+ 4H₂O(g)⇌ 4H₂(g)+ Fe₃O₄(s)If the total pressure is increased by reducing the volume,

A)the equilibrium constant increases.
B)no change occurs.
C)more Fe(s)is produced.
D)more H₂(g)is produced.
E)more H₂O(g)is produced.

Question 69

Consider the following system at equilibrium: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g)What change will cause the equilibrium to shift to form more NO?

A)increase [SO₃]
B)decrease [SO₂]
C)decrease the volume of the reaction vessel
D)decrease [NO₂]
E)decrease [SO₃]

Question 70

Consider the following reaction and the value of its equilibrium constant: FeO(s)+ CO(g)⇌ Fe(s)+ CO₂(g)K_eq = 0.67 If the equilibrium concentration of CO is measured at 0.15 M, what is the equilibrium concentration of CO₂?

A)0.10 M
B)1.2 M
C)0.15 M
D)0.52 M
E)0.22 M

Question 71

Which one of the following changes has no effect on the position of the equilibrium?

A)concentration change
B)volume change
C)pressure change
D)temperature change
E)addition of a catalyst

Question 72

Consider the following system at equilibrium: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g)What change will cause the equilibrium to shift to form more SO₂?

A)decrease [NO]
B)increase [NO₂]
C)decrease the volume of the reaction vessel
D)decrease [NO₂]
E)decrease [SO₃]

Question 73

Consider the following system at equilibrium: CH₄(g)+ 2H₂O(g)⇌ CO₂(g)+ 4H₂(g)What change will cause the equilibrium to shift to form more CH₄?

A)decrease [H₂]
B)increase [H₂O]
C)decrease the volume of the reaction vessel
D)increase [CH₄]
E)decrease [CO₂]

Question 74

Consider the following reaction: N₂(g)+ 3H₂(g)⇌ 2NH₃(g)+ heat Which conditions would favor maximum conversion of the reactants to the products?

A)high temperature and high pressure
B)low pressure; temperature is not important
C)high temperature and low pressure
D)low temperature and high pressure
E)low temperature and low pressure

Question 75

The position of equilibrium would not be appreciably affected by changes in the volume of the container for

A)NiO(s)+ CO(g)⇌ Ni(s)+ CO₂(g).
B)BaCO₃(s)⇌ BaO(s)+ CO₂(g).
C)2H₂O(g)⇌ 2H₂(g)+ O₂(g).
D)2CO(g)+ O₂(g)⇌ 2 CO₂(g).
E)PCl₅(s)⇌ PCl₃(g)+ Cl₂(g).

Question 76

Consider the following system at equilibrium: CH₄(g)+ 2H₂O(g)⇌ CO₂(g)+ 4H₂(g)What change will cause the equilibrium to shift to form more CO₂?

A)increase [H₂]
B)decrease [H₂O]
C)decrease [CH₄]
D)increase [CH₄]
E)decrease [H₂]

Question 77

Consider the following reaction and the value of its equilibrium constant: H₂O(g)+ Cl₂O(g)⇌ 2HOCl(g)K_eq = 0.090 If the equilibrium concentration of HOCl is measured at 0.20 M, what are the equilibrium concentrations of H₂O and Cl₂O, assuming that they are equal?

A)0.67
B)0.20
C)0.87
D)0.44
E)0.49

Question 78

Write the equilibrium constant expression for the reaction: CH₃NH₃⁺(aq)+ OH^-(aq)⇌ CH₃NH₂(g)+ H₂O(l)

A)K_eq = [CH₃NH3⁺][OH⁻]
B)
C)
D)
E)

Question 79

Consider the following reaction and the value of its equilibrium constant: H₂O(g)+ Cl₂O(g)⇌ 2HOCl(g)K_eq = 0.090 If the equilibrium concentration of HOCl is measured at 0.15 M, what are the equilibrium concentrations of H₂O and Cl₂O, assuming that they are equal?

A)0.15 M
B)0.090 M
C)0.50 M
D)0.25 M
E)0.60 M

Question 80

Consider the following reaction and the value of its equilibrium constant: FeO(s)+ CO(g)⇌ Fe(s)+ CO₂(g)K_eq = 0.67 If the equilibrium concentration of CO is measured at 0.40 M, what is the equilibrium concentration of CO₂?

A)0.40 M
B)1.1 M
C)0.67 M
D)0.27 M
E)1.7 M