Deck 16: Principles of Reactivity: Chemical Equilibria

Question 1

When gaseous carbon monoxide and hydrogen are combined in a sealed vessel and heated they will eventually form an equilibrium mixture of reactants and products according to the balanced chemical equilibrium below.CO(g)+ 3H₂(g) CH₄(g)+ H₂O(g)
In one such reaction 3 moles of one reactant were combined with 1 mole of the other reactant in a fixed volume vessel and heated to 1200 K.Analysis of the reaction mixture at various times gave the results below.Which component of the reaction mixture is represented by curve C?

A) hydrogen
B) carbon monoxide
C) either methane or water
D) either hydrogen or carbon monoxide
E) not enough information to decide

Answer 1

either methane or water

Question 2

Ozone is formed from oxygen.3 O₂(g) 2 O₃(g)
Calculate the value of K_p,given that K_c = 2.5 $\times$ 10^-29 at 298 K.(R = 0.08206 L.atm/mol.K)

A) 1.0 $\times$ 10^-30
B) 2.1 $\times$ 10^-30
C) 2.5 $\times$ 10^-29
D) 3.3 $\times$ 10^-28
E) 6.1 $\times$ 10^-28

Answer 2

1.0 $\times$ 10^-30

Question 3

Write the expression for K for the reaction below.

A)
B)
C)
D)
E)

Answer 3

Question 4

Which of the following statements is/are CORRECT?
1)For a chemical system,if the reaction quotient (Q)is greater than K,reactant must be converted to products to reach equilibrium.
2)For a chemical system at equilibrium,the forward and reverse rates of reaction are equal.
3)For a chemical system at equilibrium,the concentrations of products divided by the concentrations of reactants equals one.

A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1,2,and 3

Question 5

For the reaction NO(g)+ ½ O₂(g) NO₂(g)at 750°C,what is the relationship between K_c and K_p?

A) K_c = K_p
B) K_c = K_p $\times$ (RT)^-½
C) K_c = K_p = 1.0
D) K_c = K_p $\times$ (RT)^¾
E) K_c = K_p $\times$ (RT)^½

Question 6

Write a balanced chemical equation which corresponds to the following equilibrium constant expression.

A) PbF₂(aq) Pb(s)+ F₂(aq)
B) PbF₂(s) Pb²⁺(aq)+ 2 F^-(aq)
C) Pb²⁺(aq)+ 2 F^-(aq) PbF₂(s)
D) Pb(s)+ F₂(aq) PbF₂(aq)
E) PbF⁺(aq)+ F^-(aq) PbF₂(aq)

Question 7

For which one of the following reactions does K_p equal K_c?

A) 2 CO₂(g) 2 CO(g)+ O₂(g)
B) CH₄(g)+ 2 O₂(g) CO₂(g)+ 2 H₂O(g)
C) C(s)+ H₂O(g) H₂(g)+ CO(g)
D) NH₃(g) 3/2 H₂(g)+ 1/2 N₂(g)
E) 2 O₃(g) 3 O₂(g)

Question 8

What is the K_c expression for the following equilibrium?

A)
B)
C)
D)
E)

Question 9

Write the expression for K_p for the reaction below.

A)
B)
C)
D)
E)

Question 10

Which expression correctly describes the equilibrium constant K_c for the following reaction?

A)
B)
C)
D)
E)

Question 11

What balanced equation is the following equilibrium expression derived from?

A) H₂(g)+ I₂(g) HI(g)
B) HI(g) H₂(g)+ I₂(g)
C) H₂(aq)+ I₂(aq) HI(aq)
D) HI(aq) H₂(aq)+ I₂(aq)
E) 2HI(g) H₂(g)+ I₂(g)

Question 12

Which of the following statements is/are CORRECT?
1)Product concentrations appear in the numerator of an equilibrium constant expression.
2)A reaction favors the formation of products if K >> 1.
3)Stoichiometric coefficients are used as exponents in an equilibrium constant expression.

A) 1 only
B) 2 only
C) 3 only
D) 2 and 3
E) 1,2,and 3

Question 13

For which of the following equilibria does K_c = K_p?

A) N₂(g)+ 3H₂(g) 2NH₃(g)
B) CO(g)+ H₂O(g) CO₂(g)+ H₂(g)
C) CO(g)+ 3H₂(g) CH₄(g)+ H₂O(g)
D) CaO(s)+ CO₂(g) CaCO₃(s)
E) HBr(g) ½H₂(g)+ ½Br₂(l)

Question 14

Write a balanced chemical equation which corresponds to the following equilibrium constant expression.

A) HNO₂(aq)+ H₂O( ) NO₂^-(aq)+ H₃O⁺(aq)
B) NO₂^-(aq)+ H₃O⁺(aq) HNO₂(aq)+ H₂O( )
C) NO₂^-(aq)+ H₃O⁺(aq) HNO₂(aq)
D) H⁺(aq)+ OH^-(aq) H₂O( )
E) HNO₂(aq) NO₂^-(aq)+ H₃O⁺(aq)

Question 15

Given the following chemical equilibrium,
COCl₂(g)
CO(g)+ Cl₂(g)
Calculate the value of K_c,given that K_p = 6.5 $\times$ 10¹¹ at 298 K.(R = 0.08206 L.atm/mol.K)

A) 1.5 $\times$ 10^-12
B) 3.8 $\times$ 10^-11
C) 1.1 $\times$ 10⁹
D) 2.7 $\times$ 10¹⁰
E) 1.6 $\times$ 10¹³

Question 16

For which of the following reactions are the numerical values of Kp and Kc the same?
1. 2SO₂(g) + O₂(g) 2SO3(g)
2. N2(g) + O2(g) 11ea8937_ab81_0f67_a16d_5b4ecfd630df_TB4499_11 2NO(g)
3. H₂(g)+ I₂(g) 11ea8937_ab81_0f67_a16d_5b4ecfd630df_TB4499_11 2HI(g)

A) 1 only
B) 2 only
C) 1 and 2
D) 2 and 3
E) 1,2,and 3

Question 17

What is the K_c equilibrium-constant expression for the following equilibrium?

A)
B)
C)
D)
E)

Question 18

What is the expression for K_c for the following equilibrium?

A)
B)
C)
D)
E)

Question 19

Write the expression for K for the reaction of hydrofluoric acid with water.

A)
B)
C)
D)
E)

Question 20

What is the balanced equation for the following equilibrium expression?

A) 6SO₂(g)+ 3O₂(g) 6SO₃(g)
B) 6SO₃(g) 6SO₂(g)+ 3O₂(g)
C) 6SO₃(aq) 6SO₂(aq)+ 3O₂(aq)
D) 6SO₂(aq)+ 3O₂(aq) 6SO₃(aq)
E) SO₂(g)+ O₂(g) SO₃(g)

Question 21

If the reaction quotient,Q,is greater than K in a gas phase reaction,then

A) the chemical system has reached equilibrium.
B) the temperature must be increased for the reaction to proceed in the forward direction.
C) the reaction will proceed in the forward direction until equilibrium is established.
D) the reaction will proceed in the backward direction until equilibrium is established.
E) the reaction will proceed in the direction that increases the number of gas phase particles.

Question 22

At a high temperature,equal concentrations of 0.160 mol/L of H₂(g)and I₂(g)are initially present in a flask.The H₂ and I₂ react according to the balanced equation below.

When equilibrium is reached,the concentration of H₂(g)has decreased to 0.036 mol/L.What is the equilibrium constant,K_c,for the reaction?

A) 3.4
B) 4.0
C) 12
D) 22
E) 48

Question 23

Consider the reaction
A(aq) 2 B(aq)where K_c = 4.1 at 25 ^$\circ$ C.If 0.50 M A(aq)and 1.5 M B(aq)are initially present in a 1.0 L flask at 25 ^$\circ$ C,what change in concentrations (if any)will occur in time?

A) [A] will decrease and [B] will decrease.
B) [A] will decrease and [B] will increase.
C) [A] will increase and [B] will decrease.
D) [A] will increase and [B] will increase.
E) [A] and [B] remain unchanged.

Question 24

Exactly 1.0 mol N₂O₄ is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N₂O₄(g) 2NO₂(g).If at equilibrium the N₂O₄ is 28.0% dissociated,what is the value of the equilibrium constant,K_c,for the reaction under these conditions?

A) 0.44
B) 2.3
C) 0.31
D) 0.78
E) 0.11

Question 25

Which of the following is always true for a reaction where K_c is at 25 ^$\circ$ C?

A) The reaction mixture contains mostly products at equilibrium.
B) The reaction mixture contains mostly reactants at equilibrium.
C) The rate of reaction is very fast.
D) There are approximately equal moles of reactants and products at equilibrium.
E) Both A and C.

Question 26

For the reaction TlSCN(s) Tl⁺(aq)+ SCN^-(aq),K_c =
At 25 ^$\circ$ C.Which of the following concerning a 125 mL solution containing
M Tl⁺,
M SCN^- and a large excess of TlSCN(s)is/are correct?
1)The mixture is at equilibrium.
2)Additional TlSCN(s)must precipitate to attain equilibrium.
3)The reaction quotient (Q)is greater than one.

A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 2 and 3

Question 27

Which of the following statements about the reaction quotient,Q,is false?

A) The value of Q can be used to predict equilibrium concentrations.
B) It has the same expression as K_c.
C) Its value is calculated using nonequilibrium concentrations.
D) If Q > K_c,the reaction must move to equilibrium by forming more reactants.
E) If Q < K_c,the reaction must move to equilibrium by forming more products.

Question 28

At a given temperature,0.0664 mol N₂O₄(g)is placed in a 1.00 L flask.After reaching equilibrium,the concentration of NO₂(g)is 6.1 $\times$ 10^-3 M.What is K_c for the reaction below?

A) 3.7 $\times$ 10^-5
B) 1.4 $\times$ 10^-4
C) 5.9 $\times$ 10^-4
D) 9.6 $\times$ 10^-2
E) 1.8 $\times$ 10³

Question 29

Consider the following reaction:

Given that 1.00 mol of HF(g),0.389 mol of H₂(g),and 0.750 mol of F₂(g)are mixed in a 5.00-L flask,determine the reaction quotient,Q.

A) Q = 0.0729
B) Q = 0.292
C) Q = 0.0584
D) Q = 2.14
E) none of these

Question 30

At 25 ^$\circ$ C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below?

A) 5.40 $\times$ 10^-13
B) 5.40 $\times$ 10^-11
C) 1.90 $\times$ 10^-8
D) 7.35 $\times$ 10^-7
E) 1.90 $\times$ 10^-6

Question 31

The reaction quotient,Q,for a system is .If the equilibrium constant for the system at some temperature is
,what will happen as the reaction mixture returns to equilibrium?

A) The equilibrium constant will increase until it equals the reaction quotient.
B) There will be a net gain in both product(s)and reactant(s).
C) There will be a net gain in product(s).
D) There will be a net gain in reactant(s).
E) The equilibrium constant will decrease until it equals the reaction quotient.

Question 32

An aqueous mixture of phenol and ammonia has initial concentrations of 0.200 M C₆H₅OH(aq)and 0.120 M NH₃(aq).At equilibrium,the C₆H₅O^-(aq)concentration is 0.050 M.Calculate K for the reaction.
C₆H₅OH(aq)+ NH₃(aq) C₆H₅O^- + NH₄⁺(aq)

A) 0.10
B) 0.24
C) 2.1
D) 4.2
E) 4.8

Question 33

Excess Ag₂SO₄(s)is placed in water at 25 ^$\circ$ C.At equilibrium,the solution contains 0.029 M Ag⁺(aq).What is the equilibrium constant for the reaction below?

A) 1.8 $\times$ 10^-7
B) 6.1 $\times$ 10^-6
C) 1.2 $\times$ 10^-5
D) 2.4 $\times$ 10^-5
E) 8.4 $\times$ 10^-4

Question 34

A 2.5 L flask is filled with 0.25 mol SO₃,0.20 mol SO₂,and 0.40 mol O₂,and allowed to reach equilibrium.Assume the temperature of the mixture is chosen so that K_c = 0.12.Predict the effect on the concentration of SO₃ as equilibrium is achieved by using Q,the reaction quotient.
2 SO₃(g) 2 SO₂(g)+ O₂(g)

A) [SO₃] will decrease because Q > K.
B) [SO₃] will decrease because Q < K.
C) [SO₃] will increase because Q < K.
D) [SO₃] will increase because Q > K.
E) [SO₃] will remain the same because Q = K.

Question 35

A 10.0-g sample of solid NH₄Cl is heated in a 5.00-L container to 900.°C.At equilibrium the pressure of NH₃(g)is 1.47 atm.
NH₄Cl(s) NH₃(g)+ HCl(g)
The equilibrium constant,K_p,for the reaction is:

A) 2.16
B) 7.78
C) 1.47
D) 2.94
E) none of these

Question 36

If the reaction quotient,Q,is equal to K in a gas phase reaction,then

A) the chemical system has reached equilibrium.
B) the temperature must be increased for the reaction to proceed in the forward direction.
C) the reaction will proceed in the forward direction until equilibrium is established.
D) the reaction will proceed in the backward direction until equilibrium is established.
E) the reaction will proceed in the direction that increases the number of gas phase particles.

Question 37

When 0.20 mole HF is dissolved in water to a volume of 1.00 L,5.8% of the HF dissociates to form F^-(aq).What is the equilibrium constant for the reaction?

A) 1.3 $\times$ 10^-4
B) 7.1 $\times$ 10^-4
C) 1.2 $\times$ 10^-2
D) 1.7 $\times$ 10^-2
E) 6.2 $\times$ 10^-2

Question 38

Consider the following equilibrium:

Suppose 15.6 g each of CH₄,C₂H₆,C₅H₁₂,and C₆H₁₄ are placed in a 45.0-L reaction vessel at 500 K.Which of the following statements is correct?

A) Because Q_c < K_c,more products will be formed.
B) Because Q_c = 1,the system is at equilibrium.
C) Because Q_c = 1,more products will be formed.
D) Because Q_c = 1,more reactants will be formed.
E) Because Q_c > K_c,more reactants will be formed.

Question 39

What is the reaction quotient,Q,for the equilibrium
SCN^-(aq)
When 0.4257 L of
M Ag⁺ is combined with 0.2376 L of
M SCN^- in the presence of an excess of AgSCN(s)?

A)
B)
C)
D)
E)

Question 40

Nitrogen trifluoride decomposes at to form nitrogen and fluorine gases according to the following equation:

6.00-L reaction vessel is initially charged with 1.96 mol of NF₃ and allowed to come to equilibrium at 800 K.Once equilibrium is established,the reaction vessel is found to contain 0.0380 mol of N₂.What is the value of K_p at this temperature? (R = 0.0821 L.atm.mol.K)

A) 1.53 $\times$ 10^-5
B) 1.91 $\times$ 10^-3
C) 1.76 $\times$ 10^-3
D) 1.59 $\times$ 10^-5
E) 4.43 $\times$ 10^-7

Question 41

The equilibrium constant at 25 ^$\circ$ C for the dissolution of silver iodide is
8.5 $\times$ 10^-17.AgI(s) Ag⁺(aq)+ I^-(aq)
If an excess quantity of AgI(s)is added to water and allowed to equilibrate,what is the equilibrium concentration of I^-?

A) 7.2 $\times$ 10^-33 M
B) 4.3 $\times$ 10^-17 M
C) 8.5 $\times$ 10^-17 M
D) 6.5 $\times$ 10^-9 M
E) 9.2 $\times$ 10^-9 M

Question 42

The following reaction occurred when a 1.0-liter reaction vessel was initially charged with 2.0 moles of N₂(g)and 4.0 moles of H₂(g):

Once equilibrium was established,the concentration of NH₃(g)was determined to be 0.59 M at 700.°C.The value for K_c at 700.°C for the formation of ammonia is:

A) 3.5 $\times$ 10^-1
B) 6.8 $\times$ 10^-3
C) 1.1 $\times$ 10^-1
D) 6.6 $\times$ 10^-2
E) none of these

Question 43

Consider the following equilibrium:
CO₂(g)+ H₂(g) CO(g)+ H₂O(g); K_c = 1.6 at 1260 K
Suppose 0.038 mol CO₂ and 0.022 mol H₂ are placed in a 1.50-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g)? (R = 0.0821 L · atm/K·mol)

A) 9.9 atm
B) 1.1 atm
C) 4.1 atm
D) 2.6 atm
E) 1.5 atm

Question 44

The equilibrium constant,K_c,for the decomposition of ammonium hydrogen sulfide is 1.8 $\times$ 10^-4 at 25 ^$\circ$ C.NH₄HS(s) NH₃(g)+ H₂S(g)
If excess NH₄HS(s)is allowed to equilibrate at 25 ^$\circ$ C,what is the equilibrium concentration of NH₃?

A) 3.2 $\times$ 10^-8 M
B) 9.0 $\times$ 10^-5 M
C) 1.8 $\times$ 10^-4 M
D) 6.7 $\times$ 10^-3 M
E) 1.3 $\times$ 10^-2 M

Question 45

Nitrogen and oxygen gases may react to form nitrogen monoxide.
At 1500 ^$\circ$ C,K_c equals 1.0 $\times$ 10^-5.N₂(g)+ O₂(g) 2 NO(g)
If 0.030 mol N₂ and 0.030 mol O₂ are sealed in a 1.0 L flask at 1500 ^$\circ$ C,what is the concentration of NO(g)when equilibrium is established?

A) 3.0 $\times$ 10^-7 M
B) 4.7 $\times$ 10^-5 M
C) 9.5 $\times$ 10^-5 M
D) 3.0 $\times$ 10^-2 M
E) 9.1 $\times$ 10¹ M

Question 46

For the equilibrium PCl₅(g) PCl₃(g)+ Cl₂(g),K_c = 4.0 at 228°C.If pure PCl₅ is placed in a 1.00-L container and allowed to come to equilibrium,and the equilibrium concentration of PCl₅(g)is 0.26 M,what is the equilibrium concentration of PCl₃?

A) 0.13 M
B) 0.37 M
C) 0.26 M
D) 1.0 M
E) 0.017 M

Question 47

Consider the reaction H₂ + I₂ 2HI for which K_c = 43.6 at a high temperature.If an equimolar mixture of reactants gives the concentration of the product to be 0.50 M at equilibrium,determine the equilibrium concentration of the hydrogen.

A) 7.6 $\times$ 10^-2 M
B) 1.1 $\times$ 10^-1 M
C) 3.8 $\times$ 10^-2 M
D) 1.3 $\times$ 10¹ M
E) 5.7 $\times$ 10^-3 M

Question 48

A 2.50-mol sample of HI is placed in a 1.00-L vessel at 460°C,and the reaction system is allowed to come to equilibrium.The HI partially decomposes,forming 0.191 mol H₂ and 0.191 mol I₂ at equilibrium.What is the equilibrium constant K_c for the following reaction at 460°C?
½ H₂(g)+ ½ I₂(g) HI(g)

A) 1.23 $\times$ 10²
B) 8.10 $\times$ 10^-3
C) 1.72 $\times$ 10^-2
D) 11.1
E) 7.63

Question 49

Nitrosyl bromide decomposes according to the chemical equation below.2 NOBr(g) 2 NO(g)+ Br₂(g)
When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium,22% of the NOBr decomposes.What is the equilibrium constant,K_p,for the reaction?

A) 2.3 $\times$ 10^-3
B) 4.5 $\times$ 10^-3
C) 3.5 $\times$ 10^-2
D) 4.8 $\times$ 10^-2
E) 8.0 $\times$ 10^-2

Question 50

For the reaction given below,2.00 moles of A and 3.00 moles of B are placed in a 6.00-L container.
A(g)+ 2B(g) C(g)
At equilibrium,the concentration of A is 0.223 mol/L.What is the value of K_c?

A) 1.41
B) 1.77
C) 6.34
D) 0.223
E) 0.495

Question 51

Sulfuryl chloride decomposes to sulfur dioxide and chlorine.
SO₂Cl₂(g) SO₂(g)+ Cl₂(g)
K_c is 0.045 at 648 K.If an initial concentration of 0.075 M SO₂Cl₂ is allowed to equilibrate,what is the equilibrium concentration of Cl₂?

A) 0.0034 M
B) 0.030 M
C) 0.040 M
D) 0.058 M
E) 0.075 M

Question 52

In an experiment,0.42 mol H₂ and 0.42 mol I₂ are mixed in a 1.00-L container,and the reaction forms HI.If K_c = 49.for this reaction,what is the equilibrium concentration of HI?
I₂(g)+ H₂(g) 2HI(g)

A) 0.81 M
B) 0.74 M
C) 0.65 M
D) 0.105 M
E) 0.056 M

Question 53

A sample of solid NH₄NO₃ was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation:

At equilibrium the total pressure in the container was found to be 2.81 atm at a temperature of 500.°C.Calculate K_p.

A) 1.75
B) 0.877
C) 3.29
D) 88.8
E) 0.822

Question 54

At 25 ^$\circ$ C,the decomposition of dinitrogen tetraoxide
N₂O₄(g) 2 NO₂(g)
Has an equilibrium constant (K_p)of 0.144.At equilibrium,the total pressure of the system is 0.0758 atm.What is the partial pressure of each gas?

A) 0.0745 atm NO₂(g)and 0.0385 N₂O₄(g)
B) 0.0549 atm NO₂(g)and 0.0209 N₂O₄(g)
C) 0.0531 atm NO₂(g)and 0.0227 N₂O₄(g)
D) 0.0502 atm NO₂(g)and 0.0256 N₂O₄(g)
E) 0.0381 atm NO₂(g)and 0.0377 N₂O₄(g)

Question 55

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature.
3H₂ + N₂ 2NH₃
An analysis of the mixture at equilibrium revealed 2.1 mol N₂,3.2 mol H₂,and 1.8 mol NH₃.How many moles of H₂ were present at the beginning of the reaction?

A) 3.2
B) 4.8
C) 5.0
D) 5.9
E) 4.4

Question 56

For the equilibrium N₂O₄(g) 2NO₂(g),at 298 K,K_p = 0.15.For this reaction system,it is found that the partial pressure of N₂O₄ is 3.6 $\times$ 10^-2 atm at equilibrium.What is the partial pressure of NO₂ at equilibrium?

A) 4.9 atm
B) 24 atm
C) 0.0017 atm
D) 0.0054 atm
E) 0.073 atm

Question 57

At 800 K,the equilibrium constant,K_p,for the following reaction is
3.2 $\times$ 10^-7.2 H₂S(g) 2 H₂(g)+ S₂(g)
A reaction vessel at 800 K initially contains 3.00 atm of H₂S.If the reaction is allowed to equilibrate,what is the equilibrium pressure of S₂?

A) 8.5 $\times$ 10^-5 atm
B) 6.2 $\times$ 10^-3 atm
C) 9.0 $\times$ 10^-3 atm
D) 1.1 $\times$ 10^-2 atm
E) 1.4 $\times$ 10^-2 atm

Question 58

At 700 K,K_p for the following equilibrium is
5.6 $\times$ 10^-3.2HgO(s) 2Hg(l)+ O₂(g)
Suppose 51.2 g of mercury(II)oxide is placed in a sealed 3.00-L vessel at 700 K.What is the partial pressure of oxygen gas at equilibrium? (R = 0.0821 L · atm/(K · mol))

A) 0.075 atm
B) 0.0056 atm
C) 4.5 atm
D) 19 atm
E) 2.3 atm

Question 59

For the equilibrium PCl₅(g) PCl₃(g)+ Cl₂(g),K_c = 2.0 $\times$ 10¹ at 240°C.If pure PCl₅ is placed in a 1.00-L container and allowed to come to equilibrium,and the equilibrium concentration of PCl₃(g)is 0.23 M,what is the equilibrium concentration of PCl₅(g)?

A) 0.46 M
B) 0.12 M
C) 0.012 M
D) 0.0026 M
E) 9.3 M

Question 60

A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B.Gas A decomposes according to the following reaction:

The equilibrium concentration of gas C is 0.146 mol/L.Determine the value of the equilibrium constant,K_c.

A) 0.206
B) 0.163
C) 3.84 $\times$ 10^-3
D) 0.516
E) none of these

Question 61

Consider the following equilibrium at 25°C:
2ICl(g) I₂(g)+ Cl₂(g); $\Delta$ H = 27 kJ; K_p = 6.2 $\times$ 10^-6
Which of the following would be true if the temperature were increased to 100°C?
1)The value of K_p would increase.
2)The concentration of ICl(g)would increase.
3)The partial pressure of I₂ would increase.

A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1 and 3

Question 62

At a given temperature,K = 0.021 for the equilibrium:
PCl₅(g) PCl₃(g)+ Cl₂(g)
What is K for: Cl₂(g)+ PCl₃(g) PCl₅(g)?

A) 2300
B) 21
C) 0.00044
D) 48
E) 0.021

Question 63

Given the equilibrium constants for the equilibria,
2NH₄⁺(aq)+ 2H₂O(l) 2NH₃(aq)+ 2H₃O⁺(aq); K_c =
CH₃COOH(aq)+ H₂O(l) CH₃COO^-(aq)+ H₃O⁺(aq); K_c =
Determine K_c for the following equilibrium.
CH₃COOH(aq)+ NH₃(aq) CH₃COO^-(aq)+ NH₄⁺(aq)

A) 3.08 $\times$ 10⁴
B) 3.25 $\times$ 10^-5
C) 9.96 $\times$ 10^-15
D) 1.00 $\times$ 10¹⁴
E) 1.75 $\times$ 10^-5

Question 64

Assume that the following $\underline{\text{ endothermic }}$ chemical reaction is at equilibrium.
C(s)+ H₂O(g) H₂(g)+ CO(g)
Which of the following statements is/are CORRECT?
1)Increasing the concentration of H₂(g)will cause the reaction to proceed in the backward direction,increasing the equilibrium concentration of H₂O(g).
2)Decreasing the temperature will cause the reaction to proceed in the forward direction,increasing the equilibrium concentration of CO(g).
3)Increasing the amount of C(s)will cause the reaction to proceed in the forward direction,increasing the equilibrium concentration of CO(g).

A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1,2,and 3

Question 65

For the reaction N₂O₄(g) 2NO₂(g),K_p = 0.148 at a temperature of 298 K.What is K_p for the following reaction?
14NO₂(g) 7N₂O₄(g)

A) 6.43 $\times$ 10⁵
B) 1.04
C) 1.56 $\times$ 10^-6
D) 0.965
E) 6.76

Question 66

If K_c = 0.152 for A₂ + 2B 2AB,what is the value of K_c for the reaction
4AB 2A₂ + 4B?

A) 0.152
B) 0.304
C) 43.3
D) -0.152
E) 3.29

Question 67

The symbol Q is called the ________.

Question 68

The thermochemical equation for the formation of ammonia from elemental nitrogen and hydrogen is as follows.
N₂(g)+ 3 H₂(g) 2 NH₃(g) $~~~~~~~~$ $~~~~~~~~$ $\Delta$ H = -92.2 kJ
Given a system that is initially at equilibrium,which of the following actions cause the reaction to proceed to the left?

A) adding N₂(g)
B) removing NH₃(g)
C) adding a catalyst
D) decreasing the temperature
E) removing H₂(g)

Question 69

Given the following chemical equilibria,
N₂(g)+ O₂(g) 2 NO(g) $~~~~~~~~$ $~~~~~~~~$ K₁
N₂(g)+ 3 H₂(g) 2 NH₃(g) $~~~~~~~~$ $~~ ~~~$ K₂
H₂(g)+ 1/2 O₂(g) H₂O(g) $~~~~~~~~$ $~~~~ ~$ K₃
Determine the method used to calculate the equilibrium constant for the reaction below.
4 NH₃(g)+ 5 O₂(g) 4 NO(g)+ 6 H₂O(g) $~~~~~~~~$ K _c

A)
B)
C)
D)
E)

Question 70

A flask contains the following chemical system at equilibrium.
CuCO₃(s) Cu²⁺(aq)+ 2 CO₃^2-(aq)
Addition of which of the following substances will increase the solubility of CuCO₃(s)in water?
1)aqueous hydrochloric acid
2)aqueous sodium carbonate
3)solid copper(II)carbonate

A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 1,2,and 3

Question 71

Which of the following equilibria would not be affected by pressure changes at constant temperature?

A) CO₂(g)+ H₂(g) CO(g)+ H₂O(g)
B) CO(g)+ O₂(g) CO₂(g)
C) 2Hg(l)+ O₂(g) 2HgO(s)
D) 2H₂(g)+ O₂(g) 2H₂O(l)
E) CaCO₃(s) CaO(s)+ CO₂(g)

Question 72

Consider the following equilibrium:
PCl₅(g) PCl₃(g)+ Cl₂(g); $~~~~~~~~$ $\Delta$ H = 92 kJ
The concentration of PCl₃ at equilibrium may be increased by

A) decreasing the temperature.
B) adding Cl₂ to the system.
C) adding PCl₅ to the system.
D) increasing the pressure.
E) adding a catalyst.

Question 73

Given the following equilibria,
PbBr₂(s) Pb²⁺(aq)+ 2 Br^-(aq) $~~~~~~~~$ $~~~~~~~~~~~~$ K₁ = 6.6 $\times$ 0 10^-6
Pb(OH)₂(s) Pb²⁺(aq)+ 2 OH^-(aq) $~~~~~~~~$ $~~~~~~~~$ K₂ = 1.4 $\times$ 10^-15
Determine the equilibrium constant,K_c,for the following reaction.
PbBr₂(s)+ 2 OH^-(aq) Pb(OH)₂(s)+ 2 Br^-(aq)

A) 9.2 $\times$ 10^-21
B) 2.1 $\times$ 10^-10
C) 6.6 $\times$ 10^-6
D) 4.7 $\times$ 10⁹
E) 1.1 $\times$ 10²⁰

Question 74

Given the following equilibria,
Ni²⁺(aq)+ 2 OH^-(aq) Ni(OH)₂(s) $~~~~~~~~$ K₁ = 1.8 $\times$ 10¹⁵
Ni²⁺(aq)+ 4 CN^-(aq) Ni(CN)₄^2-(aq) $~~ ~~$ K₂ = 2.0 $\times$ 10³¹
Determine the equilibrium constant,K_c,for the following reaction.
Ni(OH)₂(s)+ 4 CN^-(aq) Ni(CN)₄^2-(aq)+ 2 OH^-(aq)

A) 2.8 $\times$ 10^-47
B) 9.0 $\times$ 10^-17
C) 1.8 $\times$ 10¹⁵
D) 1.1 $\times$ 10¹⁶
E) 3.6 $\times$ 10⁴⁶

Question 75

In which of the following reactions does a decrease in the volume of the reaction vessel at constant temperature favor formation of the products?

A) 2H₂(g)+ O₂(g) 2H₂O(g)
B) NO₂(g)+ CO(g) NO(g)+ CO₂(g)
C) H₂(g)+ I₂(g) 2HI(g)
D) 2O₃(g) 3O₂(g)
E) MgCO₃(s) MgO(s)+ CO₂(g)

Question 76

Assume that the following chemical reaction is at equilibrium.
2 ICl(g) I₂(g)+ Cl₂(g) $~~~~~~~~$ $~~~~~~~~$ $\Delta$ H ^$\circ$ = +26.9 kJ

At 25 ^$\circ$ C,K_p = 2.0 $\times$ 10⁵.If the temperature is increase to 45 ^$\circ$ C,which statement applies?

A) K_p will decrease and the reaction will proceed in the backward direction.
B) K_p will decrease and the reaction will proceed in the forward direction.
C) K_p will remain unchanged and the reaction will proceed in the forward direction.
D) K_p will increase and the reaction will proceed in the backward direction.
E) K_p will increase and the reaction will proceed in the forward direction.

Question 77

When the pressure of an equilibrium mixture of SO₂,O₂,and SO₃ is doubled at constant temperature,what the effect on K_p?
2SO₂(g)+ O₂(g) 2SO₃(g)

A) K_p is halved.
B) K_p is doubled.
C) K_p is unchanged.
D) K_p is tripled.
E) K_p is decreased by a third.

Question 78

In 1913,the Haber-Bosch process was patented.The product of the Haber-Bosch process is ________.

Question 79

Given the equilibrium constants for the following reactions:
4Cu(s)+ O₂(g) 2Cu₂O(s),K₁
4CuO(s) 2Cu₂O(s)+ O₂(g),K₂
What is K for the system
2Cu(s)+ O₂(g) 2CuO(s)
Equivalent to?

A)
B)
C) (K₁)(K₂)
D)
E)

Question 80

If a stress is applied to an equilibrium system,the system will respond in such a way as to relieve that stress.This is a statement of ________ principle.