Deck 15: Principles of Chemical Equilibrium

Question 1

One method to aid in working equilibrium problems is the ICE table.

Answer 1

True

Question 2

The value of the equilibrium constant for a given reaction depends on the initial concentrations of reactants.

Answer 2

False

Question 3

Given the following: I) N2O(g) + 1/2 O2(g) ⇌ 2NO(g) Kc = 1.7 × 10-13
II) N2(g) + O2(g) ⇌ 2NO(g) Kc = 4.1 × 10-31
Find the value of the equilibrium constant for the following equilibrium reaction:
N2(g) + 1/2 O2(g) ⇌ N2O(g)

A) 7.0 × 10-44
B) 4.2 × 1017
C) 2.4 × 10-18
D) 1.6 × 10-9
E) 2.6 × 10-22

Answer 3

2.4 × 10-18

Question 4

Which of the following substances present in the chemical reaction would be excluded from the equilibrium constant expression?

A) Na+ (aq)
B) H2O(g)
C) Cl-
D) H2O(l) (reactant and solvent)
E) CO(g)

Question 5

What is the value for Kc for the reaction below if the equilibrium concentrations are [N2] = 0.025, [H2] = 0.0013 and [NH3] = 0.028 for the following reaction? N2(g) + 3 H2(g) ⇌ 2 NH3(g)

A) 8.6 × 102
B) 1.4 × 107
C) 1.2 × 10-3
D) 7.1 × 10-8
E) 7.4 × 105

Question 6

Choose the INCORRECT statement.

A) A certain amount of energy, called the activation energy, must be available if a reaction is to take place.
B) A reversible chemical reaction is one in which equilibrium is never established due to the constant decomposition of the products.
C) When the rate of the reverse reaction equals the rate of the forward reaction, equilibrium has been established.
D) Changes in temperature will change the value of an equilibrium constant.
E) Chemical equilibrium is a dynamic equilibrium.

Question 7

In a system in equilibrium, two opposing reactions occur at equal rates.

Question 8

For the reaction: H2(g) + I2(g) ⇌ 2 HI(g), Kc = 92.0 When equilibrium concentrations of HI and I2 are [HI] = 0.115 M and [I2] = 0.250 M, the equilibrium concentration of [H2] is:

A) 5.00 × 10-3 M
B) 5.75 × 10-4 M
C) 1.74 × 103 M
D) 0.135 M
E) 9.56 M

Question 9

For the following chemical equilibrium, Kp = 4.6 × 10-14 at 25°C, find the value of Kc for this reaction at 25°C. 2 Cl2(g) + 2 H2O(g) ⇌ 4 HCl(g) + O2(g)

A) Kc = 1.9 × 10-15
B) Kc = 2.2 × 10-14
C) Kc = 1.1 × 10-12
D) Kc = 9.4 × 10-14
E) Kc = 4.6 × 10-14

Question 10

Which of the following equilibrium constants-reaction type is INCORRECT?

A) 1.4 × 1083 goes to completion.
B) 1.6 × 10-23 does not occur.
C) 1.8 × 10-5 equilibrium reaction more reactants than products at equilibrium.
D) 1.0 equilibrium reaction-equal amounts of products and reactants.
E) 3.2 × 103 equilibrium reaction-more reactants than products at equilibrium.

Question 11

What is the value for Kc if [CO] = 0.025, [H2] = 0.013 and [CH3OH] = 0.0028 for the following reaction? CH3OH(g) ⇌ CO(g) + 2 H2(g)

A) 1.5 × 10-3
B) 0.12
C) 6.6 × 102
D) 8.6
E) 9.1 × 10-7

Question 12

Changes in temperature cause change in the equilibrium position.

Question 13

Reaction quotient Q will always be equal to the reaction's equilibrium constant K.

Question 14

For which of the following reactions does Kp = Kc?

A) 3Fe(s) + 4H2O(g) ⇌ Fe3O4(s) + 4H2(g)
B) C(s) + H2O(g) ⇌ CO(g) + H2(g)
C) 2SO2(g) + O2(g) ⇌ 2SO3(g)
D) H2(g) + I2(s) ⇌ 2HI(g)

Question 15

The concentration of a pure solid is left out of a equilibrium constant expression but a pure liquid is included.

Question 16

Equilibrium reactions are noted by a single straight arrow for a yield sign.

Question 17

In an equilibrium process, the concentrations of products and of reactants are equal.

Question 18

Both products and reactants will be present in an equilibrium reaction unless K is very small or very large.

Question 19

Large value for equilibrium constant K means the reaction will be less complete at the equilibrium point.

Question 20

Given that the equilibrium concentrations of [N2] = 0.035 M, [C2H2] = 0.057 M, and [HCN] = 6.8 × 10-4 M, find the value of the equilibrium constant expression for the reaction:
N2(g) + C2H2(g) ⇌ 2 HCN

A) 3.4 × 10-1
B) 2.9
C) 4300
D) 2.3 × 10-4
E) 6.8 × 10-1

Question 21

For the reaction: 3 Fe(s) + 4 H2O(g) ⇌ Fe3O4(s) + 4 H2(g) what is the effect on equilibrium of increasing temperature of an exothermic reaction?

A) The reaction shifts to the right.
B) There is no change.
C) The reaction shifts to the left.
D) The Kp is decreased.
E) The Kp is doubled.

Question 22

Consider the reaction: CH4(g) + 4 Cl2(g) ⇌ CCl4(l) + 4 HCl(g) ΔH° -398 kJ/mol
The equilibrium is displaced to the right if:

A) the temperature is raised
B) the pressure is lowered
C) some carbon tetrachloride is removed
D) some hydrogen chloride is added
E) some chlorine gas is removed

Question 23

For the reaction CO(g) + 3 H2(g) ⇌ H2O(g) + CH4(g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M, [H2] = 0.045, [H2O] = 0.020, and [CH4] = 0.031, in which direction will a reaction occur and why?

A) toward products because Q = 0.38
B) toward reactants because Q = 0.24
C) toward products because Q = 4.1
D) toward reactants because Q = 61
E) it is at equilibrium because Q = 1

Question 24

For the reaction 2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g), Kc = 2.8 × 102 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [SO2] = 0.025, [O2] = 0.035, and [SO3] = 0.046, in which direction will a reaction occur and why?

A) toward products because Q = 53
B) toward reactants because Q = 0.019
C) toward products because Q = 96
D) toward reactants because Q = 2.8 × 103
E) it is at equilibrium because Q = 1

Question 25

For the reaction: CH4(g) + 2 H2O(g) ⇌ CO2(g) + 4 H2(g) ΔH° = +190 kJ when catalyst is added:

A) the reaction reacts to the right
B) the reaction reacts to the left
C) the ΔH° increases
D) the temperature increases
E) there is no change, catalyst changes reaction rate only

Question 26

Which of the following keep the equilibrium position unchanged?

A) temperature decrease
B) concentration change
C) temperature
D) pressure change
E) homogeneous catalyst

Question 27

Choose the correct statement about a container in which the chemical equilibrium is established: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) + heat

A) A decrease in amount of O2 will decrease the amount of SO2 present.
B) A decrease in the volume will decrease the amount of SO2 present.
C) A decrease in temperature will increase the amount of SO2 present.
D) A decrease in the amount of SO3 present will increase the amount of SO2 present.
E) An increase in amount of O2 will increase the amount of SO2 present.

Question 28

For the reaction: CH4(g) + 2 H2O(g) ⇌ CO2(g) + 4 H2(g) ΔH° = +190 kJ when CH4 is added:

A) the reaction reacts to the right
B) the reaction reacts to the left
C) the ΔH° increases
D) the temperature increases
E) there is no change in equilibrium position

Question 29

For the reaction: CH4(g) + 2 H2O(g) ⇌ CO2(g) + 4 H2(g) ΔH° = +190 kJ raise the temperature to 1200 K:

A) the reaction reacts to the right
B) the reaction reacts to the left
C) the ΔH° increases
D) the temperature increases
E) there is no change in equilibrium position

Question 30

Consider the following reaction. C(s) + H2O(g) ⇌ CO(g) + H2(g)
At equilibrium at a certain temperature, [H2O(g)] = 0.12 M, and [CO(g)] = [H2(g)] = 1.2 M. If suddenly these concentrations are increased by 0.50 M, which of the following is true?

A) more products are formed
B) Kc = 4.66
C) more H2O(g) will be formed
D) Since Kc does not change, nothing happens.

Question 31

Which factor influences the value of the equilibrium constant for a reversible reaction?

A) addition of a catalyst
B) raising the temperature
C) removing product
D) removing reactant
E) increase in mixing rate

Question 32

Choose the correct statement about the equilibrium: N2(g) + 3 H2(g) ⇌ 2 NH3(g), Kp = 1 × 10-4 atm-2

A) The rate constant for the forward reaction is greater than that of the reverse reaction.
B) Since the reaction has a high activation energy, a catalyst is not needed.
C) The equilibrium constant is given by Kp = [N2][H2]3/[NH3]2.
D) Conducting the reaction under high pressures will increase the yield of ammonia.
E) The Kp is independent of temperature.

Question 33

For the reaction CO(g) + 3 H2(g) ⇌ H2O(g) + CH4(g) , Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025, [H2] = 0.045, [H2O] = 0.025, and [CH4] = 0.046M, in which direction will a reaction occur and why?

A) toward products because Q = 0.17
B) toward reactants because Q = 0.0029
C) toward products because Q = 0.35
D) toward reactants because Q = 504
E) it is at equilibrium because Q = 1

Question 34

For the reaction: 3 Fe(s) + 4 H2O(g) ⇌ Fe3O4(s) + 4 H2(g) what is the effect of removing H2?

A) The reaction shifts to the right.
B) There is no change.
C) The reaction shifts to the left.
D) The Kp is decreased.
E) The Kp is doubled.

Question 35

For the reaction PCl5 (g) ⇌ PCl3 (g) + Cl2 (g) Kc = 0.0454 at 261°C. If a vessel is filled with these gases such that the initial concentrations are [PCl5] = 0.2 M, [PCl3] = 0.20 M, and [Cl2] = 2.25 M, in which direction will a reaction occur and why?

A) toward products because Q = 0.56
B) toward reactants because Q = 1.8
C) toward products because Q = 2.8
D) toward reactants because Q = 0.0454
E) it is at equilibrium because Q = 1

Question 36

For the reaction: CH4(g) + 2H2O(g) ⇌ CO2(g) + 4H2(g) ΔH° = +190 kJ add H2(g):

A) the reaction reacts to the right
B) the reaction reacts to the left
C) the ΔH° increases
D) the temperature increases
E) there is no change in equilibrium position

Question 37

In a reaction at equilibrium involving only gases, a change in pressure of the reaction mixture shifts the position of equilibrium only when:

A) heat is absorbed by the reaction proceeding to the right
B) the gases are impure
C) the collision rate increases
D) the reaction is exothermic as written
E) the moles of gas are not equal on the two sides of the equation.

Question 38

Consider the exothermic reaction: 4 HCl(aq) + MnO2(s) ⇌ Cl2(g) + 2 H2O(l) + MnCl2(aq)
The equilibrium is displaced to the left if:

A) catalyst is added
B) pressure is lowered
C) temperature is lowered
D) H2O(l) is added
E) MnO2 (s) is added

Question 39

According to Le Chatelier's Principle:

A) an increase in pressure always causes a change in the position of equilibrium for any reaction
B) the greatest yield of ammonia in the exothermic reaction N2 + 3H2 ⇌ 2NH3 is attained at a high temperature
C) the equilibrium constant is increased for the reaction A + B ⇌ C if the concentration of A is increased
D) an increase of temperature causes a decrease in the value of the equilibrium constant for an exothermic reaction
E) when an equilibrium system is stressed, the system reacts to offset the stress

Question 40

Consider the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g) ΔH° = -196.6 kJ/mol
The equilibrium is displaced to the left if:

A) some sulfur trioxide is removed
B) the temperature is raised
C) some sulfur dioxide is added
D) the pressure is raised
E) the temperature is lowered

Question 41

2.5 moles H2O and 100 g of C are placed in a 50-L container. At equilibrium for the reaction C(s) + H2O(g) ⇌ CO(g) + H2(g), [H2] = 0.040 M. Which of the following is true?

A) [CO] = 0.020 M
B) [H2O] = 0.010 M
C) no carbon is left
D) [H2O] = 0.020 M
E) [C(s)] = 0.04 M

Question 42

What is the equilibrium constant expression for: 4 NH3(g) + 5 O2(g) ⇌ 4 NO(g) + 6 H2O(g)

A)
B)
C)
D)
E)

Question 43

For the decomposition of SO3(g), Kc = [SO2]2[O2]/[SO3]2, at equilibrium, there are 0.090 mol SO2, 0.110 mol O2, 0.100 mol SO3 in a 25.0-L container. What is the value of Kc?

A) 3.6 × 10-3
B) 0.040
C) 2.23
D) 0.089
E) 7.89

Question 44

For the following reaction O2(g) ⇌ 2O(g)
What conditions favor production of oxygen atoms?

A) high temperature and low pressure
B) high temperature and high pressure
C) low temperature and low pressure
D) low temperature and high pressure

Question 45

Consider the following equilibrium reaction: PCl3(g) + Cl2(g) ⇌ PCl5(g) Kc = 96.2 The equilibrium constant for the decomposition of PCl5(g) to PCl3(g) and Cl2(g) is ________.

A) -Kc
B)
C)
D)
E)

Question 46

In a reaction at equilibrium involving only gases, a pressure change will shift the reaction only when:

A) heat is absorbed by the reaction proceeding to the right
B) the number of molecules on one side is greater than the number on the other side of the balanced equation
C) the number of molecules increases during the chemical reaction
D) the gases are impure
E) the collision rate increases

Question 47

0.75 mol of N2 and 1.20 mol of H2 are placed in a 3.0 liter container. When the reaction N2(g) + 3H2(g) ⇌ 2 NH3(g) reaches equilibrium, [H2] = 0.100 M. Which of the following is true?

A) [NH3] = 0.150 M
B) [NH3] = 0.200
C) [N2] = 0.650 M
D) [N2] = 0.250
E) [NH3] = [H2] = 0.05 M

Question 48

Consider the following chemical reaction at equilibrium: 2 Cl2(g) + 2 H2O(g) ⇌ 4 HCl(g) + O2(g)
This equilibrium can be shifted to the right by:

A) removing H2O(g) from the mixture.
B) adding more O2(g) to the mixture.
C) adding Ne(g) to the mixture.
D) decreasing the volume of the mixture.
E) increasing the volume of the mixture.

Question 49

For 2 NO2(g) ⇌ N2O4(g), Kc = [N2O4]/[NO2]2. At equilibrium there are 0.0270 mol N2O4 and 0.450 mol NO2 in a 50.0-L container. What is Kc?

A) 0.00267
B) 6.81
C) 6.67
D) 0.133
E) 2.45

Question 50

For the reaction: CH4(g) + 2H2O(g) ⇌ CO2(g) + 4H2(g) ΔH° = +190 kJ add N2(g) at constant volume and:

A) the reaction reacts to the right.
B) the reaction reacts to the left.
C) the ΔH° increases.
D) the temperature increases.
E) there is no change.

Question 51

Consider the following gas phase reaction at 25°C. N2(g) + C2H2(g) ⇌ 2 HCN(g)
1)600 mol N2(g) and 1.750 mol C2H2(g) are placed in a 1.000 L vessel and the mixture is allowed to react. At equilibrium, there are 1.587 mol N2(g) in the mixture. What is Kc for this reaction at 25 °C?

A) 9.8 × 10-4
B) 9.4 × 10-3
C) 2.5 × 10-4
D) 4.7 × 10-3
E) 6.7 × 10-5

Question 52

For CO2(g) + H2(g) ⇌ CO(g) + H2O(g), Kc = [CO][H2]/[CO2][H2], if there are 1.43 mols each of CO and H2, 0.572 mol H2 and 4.572 mols CO2, in a 4.0 L container at equilibrium, what is Kc?

A) 0.547
B) 0.782
C) 1.28
D) 0.137
E) 2.34

Question 53

Consider the following equation: N2O4(g) ⇌ 2 NO2(g) Kc = 5.8 × 10-3
If the initial concentration of N2O4(g) = 0.040 M and the initial concentration of NO2(g) is 0 M, what is the equilibrium concentration of N2O4(g)?

A) 1.7 × 10-2 M
B) 1.9 × 10-2 M
C) 3.3 × 10-2 M
D) 2.6 × 10-2 M
E) 2.3 × 10-6 M

Question 54

What will happen to the equilibrium in the reaction 2 A(g) ⇌ B(g) + C(g), Kc = 1.25 at 300 K if a catalyst is added?

A) The reaction is forced to the right.
B) The reaction is forced to the left.
C) No change, catalyst only changes the rate.
D) Kc is increased.
E) Kc is decreased.

Question 55

For the production of NO2, Kc = [NO2]2/[NO]2[O2]. At equilibrium in a 2.50 L container, there are 3.00 mol NO, 4.00 mol O2 and 22.0 mol NO2. The value of Kc is ________.

A) 13.4
B) 33.6
C) 5.38
D) 0.0116
E) 3.75

Question 56

Equilibrium constant K is constant except when one varies the:

A) concentrations of the reactants
B) temperature of the reaction
C) concentration of the products
D) partial pressures of the reactants
E) K always remains constant

Question 57

For the reaction; N2(g) + 3 H2(g) ⇌ 2 NH3(g), the equilibrium amount of NH3 will be increased by: I) increasing the pressure
II) adding H2
III) removing N2
IV) decreasing the pressure

A) I, III
B) III only
C) II, III
D) I, II
E) II, IV

Question 58

Write the equilibrium constant expression for the following reaction: N2(g) + 3 H2(g) ⇌ 2 NH3(g)

A)
B)
C)
D)
E)

Question 59

Consider the following reaction at a certain temperature. 2SO3(g) ⇌ 2SO2(g) + O2(g)
When the initial concentration of SO3(g) is 0.128 M, the concentration of oxygen gas at equilibrium is found to be 0.0130 M. Calculate Kc for this reaction.

A) 8.45 x 10-4
B) 1.62 x 10-2
C) 7.64 x 10-5
D) 1.47 x 10-3

Question 60

For the reaction below CO(g) + 2H2(g) ⇌ CH3OH(g)
The equilibrium concentrations at 483 K are [CO(g)] = 0.0753 M, [H2(g)] = 0.151 M, and [CH3OH(g)] = 0.0247 M. Calculate the value of Kc.

A) 14.4
B) 1.09
C) 2.17
D) 0.0694

Question 61

For the reaction: PCl3(g) + Cl2(g) ⇌ PCl5(g) at 70.5°C, Kp = 1.05.
If one starts with 1.80 atm pressure of PCl3(g), 1.72 atm pressure of Cl2(g), and no PCl5(g), what is the partial pressure of PCl5(g) at equilibrium?

A) 0.827 atm
B) 0.856 atm
C) 0.818 atm
D) 0.599 atm
E) 0.080 atm

Question 62

Write the equilibrium constant expression for the following reaction: 2 KI(aq) + H2O2(aq) ⇌ 2 KOH(aq) + I2(aq)

A)
B) Kc = [I2]
C) Kc = [I2]2
D)
E)

Question 63

For the reaction: 2 Cl2(g) + 2 H2O(g) ⇌ 4 HCl(g) + O2(g), Kp = 6.4 × 10-6 at 500 K. If a fixed volume is filled with initial concentrations of these gases at 227°C such that [Cl2] = 0.5 M, [H2O] = 0.40 M, [HCl] = 0.5 M, and [O2] = 0.015 M, in which direction will the reaction proceed?

A) The reaction proceeds to the right.
B) The reaction proceeds to the left.
C) The reaction is already at equilibrium.
D) The reaction volume must be specified to answer this question.
E) The value of Kp at 25 °C must be specified to answer this question.

Question 64

Find Kp for the following reaction at 25.0°C. SbCl5(g) ⇌ SbCl3(g) + Cl2(g) Kc = 2.51 × 10-2

A) 0.614
B) 1.03 × 10-3
C) 5.15 × 10-2
D) 9.74 × 102
E) 39.8

Question 65

For a reaction, the reaction quotient, Qc > Kc, the reaction ________.

A) is at equilibrium
B) is exothermic
C) shifts to the right
D) shifts to the left
E) is endothermic

Question 66

For the reaction 2 NO(g)⇌ N2O4(g) Kp equals ________.

A) Kc
B) RT/Kc
C) Kc(RT)
D) Kc/RT
E) Kc(RT)2

Question 67

For the reaction 2 A(g) ⇌ B(g) + C(g), Kc = 1.25 at 300 K. If a 1.00 L mixture contains 0.619 mol A, 0.693 mol B, and 0.689 mol C at 300 K, will the mixture be in equilibrium? If not, in what direction will a net reaction occur?

A) Yes, at equilibrium.
B) No, net reaction to the left.
C) No, net reaction to the right.
D) No, but there is no net reaction.
E) Yes, net reaction to the right

Question 68

At a certain temperature, Kc = 0.0500 and △H = +39.6 kJ for the reaction below. 2MgCl2(s) + O2(g) ⇌ 2MgO(s) + 2Cl2(g)
Calculate Kc for the reaction
MgO(s) + Cl2(g) ⇌ MgCl2(s) + O2(g)
And indicate whether the value will be larger or smaller at a lower temperature.

A) 4.47, larger
B) 400, smaller
C) 0.224, larger
D) 0.224, smaller

Question 69

What is the relationship between Kp and Kc for the reaction below? 4NH3(g) + 7O2(g) ⇌ 2N2O4(g) + 6H2O(g)

A) Kp = Kc(RT)-3
B) Kc = Kp(RT)-3
C) Kp = Kc(RT)3
D) Kp = Kc(RT)

Question 70

Write the equilibrium constant expression for the following reaction: 6 CO2(g) + 6 H2O(l) ⇌ C6H12O6(s) + 6 O2(g)

A)
B)
C)
D)
E)

Question 71

Write the equilibrium expression Kc for the reaction: sodium sulfite(aq) + chloric acid (aq) ⇌ sodium chlorite(aq) + sulfur dioxide(g) + water(l).

A)
B)
C)
D)
E)

Question 72

For the reaction: 3 Fe(s) + 4 H2O(g) ⇌ Fe3O4(s) + 4 H2(g)
Write the expression for Kp.

A)
B)
C)
D)
E)

Question 73

For the reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g), Kc = 6.9 × 1024 at 25°C. If a reaction vessel is filled with these gases, such that [SO2] = 6.0 M, [O2] = 6.0 M and [SO3] = 6.0 M, in which direction will the reaction proceed?

A) The reaction proceeds to the right.
B) The reaction proceeds to the left.
C) The reaction is already at equilibrium.
D) The reaction volume must be specified to answer this question.
E) The value of Kp must be specified to answer this question.

Question 74

Two moles of NH3 are initially present for the reaction: 2 NH3(g) ⇌ N2(g) + 3 H2(g)
At equilibrium there is 1.00 mol NH3. How many moles of H2 are present at equilibrium?

A) 3.00
B) 1.00
C) 1.50
D) 0.67
E) 0.75

Question 75

Given the following reactions, 2PCl3(g) ⇌ 2P(g) + 3Cl2(g) Kc = 0.0667
PCl3(g) + Cl2(g) ⇌ PCl5(g) Kc = 4.0
Calculate Kc for the reaction below.
2P(g) + 5Cl2(g) ⇌ 2PCl5(g)

A) 240
B) 1.1
C) 60
D) 23

Question 76

For the reaction: 3 Fe(s) + 4 H2O(g) ⇌ Fe3O4(s) + 4 H2(g) write the expression for Kc in terms of Kp.

A) Kc = Kp
B) Kc =
C) Kc = KpRT
D) Kc = Kp2
E) Kc =

Question 77

Write the equilibrium constant expression for the reaction: 3 Sn(s) + 4 HNO3(aq) + H2O(l) ⇌ 3 H2SnO3(s) + 4 NO(g)

A) Kc =
B) Kc =
C) Kc =
D) Kc =
E) Kc =

Question 78

Consider the following hypothetical equilibrium reaction: A2(g) + B2(g) ⇌ 2AB(g) where Kc = The equilibrium constant for the reaction: 2 A2(g) + 2 B2(g) ⇔ 4 AB(g) is ________.

A)
B) Kc4
C)
D)
E) Kc2

Question 79

For the reaction: 3 Fe(s) + 4 H2O(g) ⇌ Fe3O4(s) + 4 H2(g) what is the effect of adding Fe(s)?

A) The reaction shifts to the right.
B) There is no change.
C) The reaction shifts to the left.
D) The Kp is decreased.
E) The Kp is doubled.

Question 80

In the reaction: 2 N2O(g) + N2H4(g) ⇌ 3 N2(g) + 2 H2O(g),
One starts with 0.10 mol N2O and 0.25 mol N2H4 in a 10.0 L container. If there are 0.06 mol N2O at equilibrium, how many moles of N2 are present?

A) 0.02
B) 0.04
C) 0.06
D) 0.09
E) 0.07