Question 1

If one starts with pure NO2(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO2(g)  2(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO2(g)     2NO(g) + O2(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO2. A) 0.152 atm B) 0.174 atm C) 0.200 atm D) 0.326 atm E) The total pressure cannot be calculated because Kp is not given" class="answers-bank-image d-inline" rel="preload" >  2NO(g) + O2(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO2.

Accepted Answer

A)  0.152 atm
B)  0.174 atm
C)  0.200 atm
D)  0.326 atm
E)  The total pressure cannot be calculated because Kp is not givenF) A) and E)
G) A) and B)

Question 2

When the reaction 2H2S(g)  2S(g)     2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.012. Starting with pure H2S at 1065°, what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(g) ? A) 1.06 atm B) 1.86 atm C) 0.94 atm D) 0.90 atm E) 1.52 atm" class="answers-bank-image d-inline" rel="preload" >  2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.012. Starting with pure H2S at 1065°, what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(g) ?

Accepted Answer

A)  1.06 atm
B)  1.86 atm
C)  0.94 atm
D)  0.90 atm
E)  1.52 atmF) C) and D)
G) A) and C)

Question 3

Consider the following equilibrium,
4NH3(g)+ 3O2(g)  2N2(g)+ 6H2O(g)+ 1531 kJ
State whether the concentrations of the reactants would increase, decrease, or remain constant when the temperature is increased.

Accepted Answer

Question 4

Sodium carbonate, Na2CO3(s) , can be prepared by heating sodium bicarbonate, NaHCO3(s) . 2NaHCO3(s)  2CO3(s) , can be prepared by heating sodium bicarbonate, NaHCO3(s) . 2NaHCO3(s)   Na2CO3(s) + CO2(g) + H2O(g) Kp = 0.23 at 100ºC If a sample of NaHCO3 is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be? A) 0.46 atm B) 0.96 atm C) 0.23 atm D) 0.48 atm E) 0.11 atm" class="answers-bank-image d-inline" rel="preload" >Na2CO3(s) + CO2(g) + H2O(g) Kp = 0.23 at 100ºC
If a sample of NaHCO3 is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?

Accepted Answer

A)  0.46 atm
B)  0.96 atm
C)  0.23 atm
D)  0.48 atm
E)  0.11 atmF) All of the above
G) A) and B)

Question 5

The data below refer to the following reaction:
2NO(g)+ Br2(g)  2NOBr(g)  Find the concentration of NOBr when the system reaches equilibrium.

Accepted Answer

Question 6

At 700 K, the reaction 2SO2(g) + O2(g)  2(g) + O2(g)   2SO3(g) has the equilibrium constant Kc = 4.3 * 106 , and the following concentrations are present: [SO2] = 0.10 M; [SO3] = 10. M; [O2] = 0.10 M. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written) , left to right or right to left, will the reaction proceed to reach equilibrium? A) Yes, the mixture is at equilibrium. B) No, left to right C) No, right to left D) There is not enough information to be able to predict the direction." class="answers-bank-image d-inline" rel="preload" >2SO3(g) has the equilibrium constant Kc = 4.3 * 106 , and the following concentrations are present: [SO2] = 0.10 M; [SO3] = 10. M; [O2] = 0.10 M. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written) , left to right or right to left, will the reaction proceed to reach equilibrium?

Accepted Answer

A)  Yes, the mixture is at equilibrium.
B)  No, left to right
C)  No, right to left
D)  There is not enough information to be able to predict the direction.E) A) and C)
F) All of the above

Question 7

Kp for the reaction of SO2(g) with O2 to produce SO3(g) is 3 * 1024 . Calculate Kc for this equilibrium at 25ºC. (The relevant reaction is 2SO2(g) + O2(g)  p for the reaction of SO2(g) with O2 to produce SO3(g) is 3 * 1024 . Calculate Kc for this equilibrium at 25ºC. (The relevant reaction is 2SO2(g) + O2(g)     2SO3(g) .)  A) 3 * 1024 B) 5 * 1021 C) 2 * 1020 D) 5 * 1022 E) 7 * 1025" class="answers-bank-image d-inline" rel="preload" >  2SO3(g) .)

Accepted Answer

A)  3 * 1024
B)  5 * 1021
C)  2 * 1020
D)  5 * 1022
E)  7 * 1025F) C) and E)
G) B) and E)

Question 8

For the common allotropes of carbon (graphite and diamond) , C(gr)  →\rarr→  C(dia) with equilibrium constant K = 0.32. The molar volumes of graphite and diamond are, respectively, 5.30 cm3/mol and 3.42 cm3/mol;  Δ\DeltaΔ Hf of diamond is 1.90 kJ/mol. This data suggests that the formation of diamond is favored at

Accepted Answer

A)  low temperatures and low pressures.
B)  high temperatures and low pressures.
C)  low temperatures and high pressures.
D)  high temperatures and high pressures. E) C) and D)
F) B) and D)

Question 9

Consider the following equilibrium,
4NH3(g)+ 3O2(g)  2N2(g)+ 6H2O(g)+ 1531 kJ
State whether the concentrations of the products would increase, decrease, or remain constant after ammonia was added to the system.

Accepted Answer

Question 10

3. 2NO2  3. 2NO2     2NO + O2 Kp = 5.9 *10 -5 A) 2    2NO + O2 Kp = 5.9 *10 -5

Accepted Answer

A)  2 
B)  1 
C)  2 
D)  3 
E)  3 < 1 < 2F) C) and D)
G) None of the above

Question 11

Consider the following equilibria: 2SO3(g)  3(g)    2SO2(g) + O2(g) Kc = 2.3 * 10-7 2NO3(g)    2NO2(g) + O2(g) Kc = 1.4  * 10-3  Calculate the equilibrium constant for the reaction SO2(g) + NO3(g)  \rarr SO3(g) + NO2(g)  A) 78 B) 1.3 * 10-2 C) 1.6 * 10-4 D) 3.2 * 10-10 E) 6.1 * 103 " class="answers-bank-image d-inline" rel="preload" > 2SO2(g) + O2(g) Kc = 2.3 * 10-7
2NO3(g)   2NO2(g) + O2(g) Kc = 1.4  * 10-3
 Calculate the equilibrium constant for the reaction
SO2(g) + NO3(g)  →\rarr→ SO3(g) + NO2(g)

Accepted Answer

A)  78
B)  1.3 * 10-2
C)  1.6 * 10-4
D)  3.2 * 10-10
E)  6.1 * 103 F) B) and D)
G) A) and E)

Question 12

Ethanol and acetic acid react to form ethyl acetate and water according to the following chemical equation:
C2H5OH(l)+ CH3COOH(l)  CH3COOC2H5(l)+ H2O(l)
When two moles each of ethanol and acetic acid are combined, equilibrium is reached when two-thirds of a mole of each of the reactants remains. Calculate the equilibrium constant for this reaction assuming total volume does not change during the course of the reaction. (Note: since water is not the solvent, but rather a product of the reaction, [H2O] changes during the course of the reaction, so it should be included in the equilibrium constant expression.)

Accepted Answer

Question 13

Consider the following equilibrium,
4NH3(g)+ 3O2(g)  2N2(g)+ 6H2O(g)+ 1531 kJ
State whether the concentrations of the products would increase, decrease, or remain constant after nitrogen gas was removed from the system.

Accepted Answer

Question 14

The reaction A(g) + 2B(g)   C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate Kc for this reaction. A) 0.060 B) 5.1 C) 17 D) 19 E) 25" class="answers-bank-image d-inline" rel="preload" >  C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate Kc for this reaction.

Accepted Answer

A)  0.060
B)  5.1
C)  17
D)  19
E)  25F) B) and D)
G) A) and E)

Question 15

Consider the following equilibrium,
4NH3(g)+ 3O2(g)  2N2(g)+ 6H2O(g)+ 1531 kJ
State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

Accepted Answer

Question 16

The equilibrium constant for the chemical equation
2NO(g)+ O2(g)  2NO2(g)
is two times the equilibrium constant for the chemical equation
NO(g)+ 1/2O2(g)  NO2(g).

Accepted Answer

A) True 
 B)False

Question 17

At 250ºC, the equilibrium constant Kp for the reaction PCl5(g)  p for the reaction PCl5(g)     PCl3(g) + Cl2(g) is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. Calculate the pressure of PCl5 after the system has reached equilibrium. A) 1.50 atm B) 1.24 atm C) 4.24 atm D) 0.94 atm E) 1.12 atm" class="answers-bank-image d-inline" rel="preload" >  PCl3(g) + Cl2(g) is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. Calculate the pressure of PCl5 after the system has reached equilibrium.

Accepted Answer

A)  1.50 atm
B)  1.24 atm
C)  4.24 atm
D)  0.94 atm
E)  1.12 atmF) A) and C)
G) C) and E)

Question 18

Consider the following reactions and their associated equilibrium constants: A + 2B 1  C   D + E K2  For the reaction A + 2B  \rarr  D + E, having equilibrium constant Kc, A) Kc = K1 + K2 B) Kc = K1/K2 C) Kc = K1  - K2 D) Kc = (K1) (K2)  E) Kc = K2/K1 " class="answers-bank-image d-inline" rel="preload" > C K1
 C  D + E K2
 For the reaction A + 2B  →\rarr→  D + E, having equilibrium constant Kc,

Accepted Answer

A)  Kc = K1 + K2
B)  Kc = K1/K2
C)  Kc = K1  - K2
D)  Kc = (K1) (K2) 
E)  Kc = K2/K1 F) A) and C)
G) B) and E)

Question 19

Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon dioxide.
CaCO3(s)  CaO(s)+ CO2(g)
KP for this reaction is 1.16 at 800°C. A 5.00 L vessel containing 10.0 g of CaCO3(s)was evacuated to remove the air, sealed, and then heated to 800°C. Ignoring the volume occupied by the solid, what will be the mass of the solid in the vessel once equilibrium is reached?

Accepted Answer

Question 20

For the nitrogen fixation reaction 3H2(g) + N2(g)  2(g) + N2(g)    2NH3(g) , Kc = 6.0 * 10-2 at 500°C. If 0.250 M H2 and 0.050 M NH3 are present at equilibrium, what is the equilibrium concentration of N2? A) 0.750 M B) 2.7 M C) 0.250 M D) 0.025 M E) 1.85 M" class="answers-bank-image d-inline" rel="preload" > 2NH3(g) , Kc = 6.0 * 10-2 at 500°C. If 0.250 M H2 and 0.050 M NH3 are present at equilibrium, what is the equilibrium concentration of N2?

Accepted Answer

A)  0.750 M
B)  2.7 M
C)  0.250 M
D)  0.025 M
E)  1.85 MF) A) and E)
G) B) and C)

Exam 15: Chemical Equilibrium

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant after nitrogen gas was removed from the system.

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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When the reaction 2H₂S(g) 2H₂(g) + S₂(g) is carried out at 1065°C, K_p = 0.012. Starting with pure H₂S at 1065°, what must the initial pressure of H₂S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H₂(g) ?

Correct Answer
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The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Find the concentration of NOBr when the system reaches equilibrium.

Correct Answer
verified

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

Correct Answer
verified

Correct Answer
verified

The reaction A(g) + 2B(g) C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate K_c for this reaction.

Correct Answer
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K_p for the reaction of SO₂(g) with O₂ to produce SO₃(g) is 3 * 10²⁴ . Calculate K_c for this equilibrium at 25ºC. (The relevant reaction is 2SO₂(g) + O₂(g) 2SO₃(g) .)

Correct Answer
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For the nitrogen fixation reaction 3H₂(g) + N₂(g) 2NH₃(g) , K_c = 6.0 * 10^-2 at 500°C. If 0.250 M H₂ and 0.050 M NH₃ are present at equilibrium, what is the equilibrium concentration of N₂?

Correct Answer
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Correct Answer
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The equilibrium constant for the chemical equation 2NO(g)+ O₂(g) 2NO₂(g) is two times the equilibrium constant for the chemical equation NO(g)+ ¹/₂O₂(g) NO₂(g).

Correct Answer
verified

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant after ammonia was added to the system.

Correct Answer
verified

Correct Answer
verified

If one starts with pure NO₂(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO₂(g) 2NO(g) + O₂(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO₂.

Correct Answer
verified

3. 2NO₂ 2NO + O₂ K_p = 5.9 *10^-5

Correct Answer
verified

At 250ºC, the equilibrium constant K_p for the reaction PCl₅(g) PCl₃(g) + Cl₂(g) is 1.80. Sufficient PCl₅ is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. Calculate the pressure of PCl₅ after the system has reached equilibrium.

Correct Answer
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Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant when the temperature is increased.

Correct Answer
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Correct Answer
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Exam 15: Chemical Equilibrium

Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant after nitrogen gas was removed from the system.

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Sodium carbonate, Na2CO3(s) , can be prepared by heating sodium bicarbonate, NaHCO3(s) . 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g) Kp = 0.23 at 100ºC If a sample of NaHCO3 is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

When the reaction 2H2S(g) 2H2(g) + S2(g) is carried out at 1065°C, Kp = 0.012. Starting with pure H2S at 1065°, what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(g) ?

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The data below refer to the following reaction: 2NO(g)+ Br2(g) 2NOBr(g) Find the concentration of NOBr when the system reaches equilibrium.

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Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The reaction A(g) + 2B(g) C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate Kc for this reaction.

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Kp for the reaction of SO2(g) with O2 to produce SO3(g) is 3 * 1024 . Calculate Kc for this equilibrium at 25ºC. (The relevant reaction is 2SO2(g) + O2(g) 2SO3(g) .)

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For the nitrogen fixation reaction 3H2(g) + N2(g) 2NH3(g) , Kc = 6.0 * 10-2 at 500°C. If 0.250 M H2 and 0.050 M NH3 are present at equilibrium, what is the equilibrium concentration of N2?

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Consider the following reactions and their associated equilibrium constants: A + 2B C K1 C 11ec7153_74a6_4277_88eb_656263c228fc_TB3244_11 D + E K2 For the reaction A + 2B →\rarr→ D + E, having equilibrium constant Kc,

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The equilibrium constant for the chemical equation 2NO(g)+ O2(g) 2NO2(g) is two times the equilibrium constant for the chemical equation NO(g)+ 1/2O2(g) NO2(g).

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Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant after ammonia was added to the system.

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Consider the following equilibria: 2SO3(g) 2SO2(g) + O2(g) Kc = 2.3 * 10-7 2NO3(g) 11ec7153_74a6_4277_88eb_656263c228fc_TB3244_11 2NO2(g) + O2(g) Kc = 1.4 * 10-3 Calculate the equilibrium constant for the reaction SO2(g) + NO3(g) →\rarr→ SO3(g) + NO2(g)

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If one starts with pure NO2(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO2(g) 2NO(g) + O2(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO2.

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3. 2NO2 2NO + O2 Kp = 5.9 *10 -5

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At 250ºC, the equilibrium constant Kp for the reaction PCl5(g) PCl3(g) + Cl2(g) is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. Calculate the pressure of PCl5 after the system has reached equilibrium.

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Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant when the temperature is increased.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant after nitrogen gas was removed from the system.

Correct Answer
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Correct Answer
verified

Correct Answer
verified

Correct Answer
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When the reaction 2H₂S(g) 2H₂(g) + S₂(g) is carried out at 1065°C, K_p = 0.012. Starting with pure H₂S at 1065°, what must the initial pressure of H₂S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H₂(g) ?

Correct Answer
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The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Find the concentration of NOBr when the system reaches equilibrium.

Correct Answer
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Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after ammonia was added to the system.

Correct Answer
verified

Correct Answer
verified

The reaction A(g) + 2B(g) C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate K_c for this reaction.

Correct Answer
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K_p for the reaction of SO₂(g) with O₂ to produce SO₃(g) is 3 * 10²⁴ . Calculate K_c for this equilibrium at 25ºC. (The relevant reaction is 2SO₂(g) + O₂(g) 2SO₃(g) .)

Correct Answer
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For the nitrogen fixation reaction 3H₂(g) + N₂(g) 2NH₃(g) , K_c = 6.0 * 10^-2 at 500°C. If 0.250 M H₂ and 0.050 M NH₃ are present at equilibrium, what is the equilibrium concentration of N₂?

Correct Answer
verified

Correct Answer
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The equilibrium constant for the chemical equation 2NO(g)+ O₂(g) 2NO₂(g) is two times the equilibrium constant for the chemical equation NO(g)+ ¹/₂O₂(g) NO₂(g).

Correct Answer
verified

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant after ammonia was added to the system.

Correct Answer
verified

Correct Answer
verified

If one starts with pure NO₂(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO₂(g) 2NO(g) + O₂(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO₂.

Correct Answer
verified

3. 2NO₂ 2NO + O₂ K_p = 5.9 *10^-5

Correct Answer
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At 250ºC, the equilibrium constant K_p for the reaction PCl₅(g) PCl₃(g) + Cl₂(g) is 1.80. Sufficient PCl₅ is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. Calculate the pressure of PCl₅ after the system has reached equilibrium.

Correct Answer
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Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant when the temperature is increased.

Correct Answer
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Correct Answer
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