Question 1

For the reaction 2X(g)  + Y(g)  c = 1.00 ×103 at 500 K. If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z? A)  2.2 M B)  3.2 M C)  3.5 M D)  4.5 M E)  7.1 M" class="answers-bank-image d-inline" rel="preload" > 2Z(g) , Kc = 1.00 ×103 at 500 K. If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?

Accepted Answer

A)   2.2 M
B)   3.2 M
C)   3.5 M
D)   4.5 M
E)   7.1 MF) A) and E)
G) All of the above

Question 2

5.00 mol of ammonia are introduced into a 5.00-L reactor vessel in which it partially dissociates at high temperatures.
2NH3(g)  3H2(g) + N2(g)
At equilibrium at a particular temperature, 1.00 mole of ammonia remains. Calculate Kc for the reaction.

Accepted Answer

Question 3

A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H2(g)  + N2(g)  2(g)  + N2(g)    2NH3(g)  A)  There will be no effect. B)  More ammonia will be produced at the expense of hydrogen and nitrogen. C)  Hydrogen and nitrogen will be produced at the expense of ammonia. D)  The equilibrium constant will increase. E)  The equilibrium constant will decrease." class="answers-bank-image d-inline" rel="preload" > 2NH3(g)

Accepted Answer

A)   There will be no effect.
B)   More ammonia will be produced at the expense of hydrogen and nitrogen.
C)   Hydrogen and nitrogen will be produced at the expense of ammonia.
D)   The equilibrium constant will increase.
E)   The equilibrium constant will decrease.F) A) and E)
G) A) and D)

Question 4

For the equilibrium A2(g)  2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Kc and time as equilibrium is established? A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > 2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Kc and time as equilibrium is established?

Accepted Answer

A)   2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Kc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Kc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Kc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Kc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2(g)    2A(g) , if a sample of A2(g)  is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Kc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) C) and D)
G) B) and E)

Question 5

Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position, regardless of the physical state of the substance involved.

Accepted Answer

A) True 
 B)False

Question 6

Consider the reaction N2(g) + 3H2(g)  2NH3(g). If nitrogen is added to the system at equilibrium, what will happen to the ammonia concentration?

Accepted Answer

The ammoni...

Question 7

Nitrosyl chloride (NOCl)  decomposes at elevated temperatures according to the equation 2NOCl(g)  2(g) . What is KP for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol. (R = 8.314 J/K • mol)  A)  1.60 × 10-2 B)  2.10 × 10-7 C)  62.8 D)  4.90 × 106 E)  3.20 × 109" class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + Cl2(g) . What is KP for this reaction at 227°C?
For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol. (R = 8.314 J/K • mol)

Accepted Answer

A)   1.60 × 10-2
B)   2.10 × 10-7
C)   62.8
D)   4.90 × 106
E)   3.20 × 109F) A) and C)
G) A) and D)

Question 8

Phosgene, COCl2, a poisonous gas, decomposes as follows. COCl2(g)  2, a poisonous gas, decomposes as follows. COCl2(g)    CO(g)  + Cl2(g) . At 900.ºC, Kc = 0.083. What is KP at this temperature? (R = 0.08206 L • atm/K • mol)  A)  0.125 B)  8.0 C)  6.1 D)  0.16 E)  0.083" class="answers-bank-image d-inline" rel="preload" > CO(g)  + Cl2(g) .
At 900.ºC, Kc = 0.083. What is KP at this temperature? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)   0.125
B)   8.0
C)   6.1
D)   0.16
E)   0.083F) C) and D)
G) A) and D)

Question 9

The following reactions occur at 500 K. Arrange them in order of increasing tendency to proceed to completion (least completion → greatest completion) .

Accepted Answer

A)   2 
B)   3 
C)   3 
D)   4 
E)   4 < 3 < 1 < 2F) C) and D)
G) A) and D)

Question 10

When a reaction reaches ________, the concentration of the reactants and products will no longer change.

Accepted Answer

The answer of When a reaction reaches ________, the concentration...

Question 11

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g)  + O2(g)  2(g)  + O2(g)    2NO(g)  The equilibrium constant KP for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen? A)  0.15 atm B)  0.31 atm C)  3.08 atm D)  7.69 atm E)  7.85 atm" class="answers-bank-image d-inline" rel="preload" > 2NO(g) 
The equilibrium constant KP for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?

Accepted Answer

A)   0.15 atm
B)   0.31 atm
C)   3.08 atm
D)   7.69 atm
E)   7.85 atmF) A) and B)
G) B) and E)

Question 12

Hydrogen iodide decomposes according to the equation 2HI(g)  2(g)  + I2(g) , for which Kc = 0.0156 at 400ºC. Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC. What is the concentration of H2 at equilibrium? A)  0.275 M B)  0.138 M C)  0.0275 M D)  0.0550 M E)  0.220 M" class="answers-bank-image d-inline" rel="preload" > H2(g)  + I2(g) , for which Kc = 0.0156 at 400ºC. Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC. What is the concentration of H2 at equilibrium?

Accepted Answer

A)   0.275 M
B)   0.138 M
C)   0.0275 M
D)   0.0550 M
E)   0.220 MF) B) and D)
G) A) and D)

Question 13

At 400ºC, Kc = 64 for the equilibrium H2(g)  + I2(g)  c = 64 for the equilibrium H2(g)  + I2(g)    2HI(g) . If 3.00 mol H2 and 3.00 mol I2 are introduced into an empty 4.0-L vessel, what is the equilibrium concentration of HI at 400ºC? A)  0.15 M B)  1.2 M C)  2.4 M D)  4.8 M E)  5.8 M" class="answers-bank-image d-inline" rel="preload" > 2HI(g) . If 3.00 mol H2 and 3.00 mol I2 are introduced into an empty 4.0-L vessel, what is the equilibrium concentration of HI at 400ºC?

Accepted Answer

A)   0.15 M
B)   1.2 M
C)   2.4 M
D)   4.8 M
E)   5.8 MF) A) and D)
G) A) and C)

Question 14

The reaction 2H2O2(g)  2O2(g)    2H2O(g)  + O2(g)  is exothermic, ΔHºrxn = -210 kJ/mol. Which one of the following is correct? A)  KP at 800 K is smaller than KP at 1200 K. B)  Temperature does not affect KP C)  KP depends only on the pressure. D)  KP at 1200 K is smaller than KP at 800 K. E)  KP depends on total pressure as well as temperature." class="answers-bank-image d-inline" rel="preload" > 2H2O(g)  + O2(g)  is exothermic, ΔHºrxn = -210 kJ/mol. Which one of the following is correct?

Accepted Answer

A)   KP at 800 K is smaller than KP at 1200 K.
B)   Temperature does not affect KP
C)   KP depends only on the pressure.
D)   KP at 1200 K is smaller than KP at 800 K.
E)   KP depends on total pressure as well as temperature.F) None of the above
G) C) and D)

Question 15

Which equation is correct?

Accepted Answer

A)   ΔG = ΔG° - RT logKeq
B)   ΔG = ΔG° + RT lnQ
C)   ΔG = RT lnQ
D)   ΔG = -RT logQ
E)   ΔG = -RT logKeqF) D) and E)
G) C) and E)

Question 16

For the reaction 2NOCl(g)  2(g) , Kc = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 - reaction vessel in order that the equilibrium concentration of NOCl is 1.00 M? A)  1.26 M B)  2.25 M C)  2.50 M D)  3.52 M E)  11.0 M" class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + Cl2(g) , Kc = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 - reaction vessel in order that the equilibrium concentration of NOCl is 1.00 M?

Accepted Answer

A)   1.26 M
B)   2.25 M
C)   2.50 M
D)   3.52 M
E)   11.0 MF) B) and D)
G) B) and C)

Question 17

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)  3.3 M B)  2.7 M C)  0.20 M D)  0.083 M E)  0.058 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)   3.3 M
B)   2.7 M
C)   0.20 M
D)   0.083 M
E)   0.058 MF) All of the above
G) A) and E)

Question 18

At what temperature is KP = 4.00 for the reaction N2O4(g)  P = 4.00 for the reaction N2O4(g)    2NO2(g) ?   (R = 8.314 J/K • mol)  A)  197°C B)  56°C C)  36°C D)  79°C E)  476°C" class="answers-bank-image d-inline" rel="preload" > 2NO2(g) ? P = 4.00 for the reaction N2O4(g)    2NO2(g) ?   (R = 8.314 J/K • mol)  A)  197°C B)  56°C C)  36°C D)  79°C E)  476°C" class="answers-bank-image d-inline" rel="preload" > (R = 8.314 J/K • mol)

Accepted Answer

A)   197°C
B)   56°C
C)   36°C
D)   79°C
E)   476°CF) D) and E)
G) C) and E)

Question 19

Consider the reaction N2(g)  + O2(g)  2(g)  + O2(g)    2NO(g) , for which Kc = 0.10 at 2000ºC. Starting with initial concentrations of 0.040 M for N2 and 0.040 M for O2 what is the equilibrium concentration of NO? A)  0.0096 M B)  0.011 M C)  0.019 M D)  0.080 M E)  0.10 M" class="answers-bank-image d-inline" rel="preload" > 2NO(g) , for which Kc = 0.10 at 2000ºC. Starting with initial concentrations of 0.040 M for N2 and 0.040 M for O2 what is the equilibrium concentration of NO?

Accepted Answer

A)   0.0096 M
B)   0.011 M
C)   0.019 M
D)   0.080 M
E)   0.10 MF) A) and C)
G) A) and E)

Question 20

During a chemical reaction, what defines when the concentrations of the reactants and products reach a constant level?

Accepted Answer

A)   Elementary process
B)   Reversible reaction
C)   Rate law
D)   Rate constant
E)   EquilibriumF) A) and E)
G) A) and D)

Exam 15: Chemical Equilibrium

For the equilibrium A₂(g) 2A(g) , if a sample of A₂(g) is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between K_c and time as equilibrium is established?

Correct Answer
verified

5.00 mol of ammonia are introduced into a 5.00-L reactor vessel in which it partially dissociates at high temperatures. 2NH₃(g) 3H₂(g) + N₂(g) At equilibrium at a particular temperature, 1.00 mole of ammonia remains. Calculate K_c for the reaction.

Correct Answer
verified

Phosgene, COCl₂, a poisonous gas, decomposes as follows. COCl₂(g) CO(g) + Cl₂(g) . At 900.ºC, K_c = 0.083. What is K_P at this temperature? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H₂(g) + N₂(g) 2NH₃(g)

Correct Answer
verified

At 400ºC, K_c = 64 for the equilibrium H₂(g) + I₂(g) 2HI(g) . If 3.00 mol H₂ and 3.00 mol I₂ are introduced into an empty 4.0-L vessel, what is the equilibrium concentration of HI at 400ºC?

Correct Answer
verified

Consider the reaction N₂(g) + 3H₂(g) 2NH₃(g). If nitrogen is added to the system at equilibrium, what will happen to the ammonia concentration?

Correct Answer
verified
The ammoni...
View Answer

For the reaction 2X(g) + Y(g) 2Z(g) , K_c = 1.00 ×10³ at 500 K. If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?

Correct Answer
verified

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

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g) + Cl₂(g) . What is K_P for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol. (R = 8.314 J/K • mol)

Correct Answer
verified

The reaction 2H₂O₂(g) 2H₂O(g) + O₂(g) is exothermic, ΔHº_rxn=-210 kJ/mol. Which one of the following is correct?

Correct Answer
verified

Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position, regardless of the physical state of the substance involved.

Correct Answer
verified

During a chemical reaction, what defines when the concentrations of the reactants and products reach a constant level?

Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + I₂(g) , for which K_c = 0.0156 at 400ºC. Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC. What is the concentration of H₂ at equilibrium?

Correct Answer
verified

At what temperature is K_P = 4.00 for the reaction N₂O₄(g) 2NO₂(g) ? (R = 8.314 J/K • mol)

Correct Answer
verified

Consider the reaction N₂(g) + O₂(g) 2NO(g) , for which K_c = 0.10 at 2000ºC. Starting with initial concentrations of 0.040 M for N₂ and 0.040 M for O₂ what is the equilibrium concentration of NO?

Correct Answer
verified

For the reaction 2NOCl(g) 2NO(g) + Cl₂(g) , K_c = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 - reaction vessel in order that the equilibrium concentration of NOCl is 1.00 M?

Correct Answer
verified

When a reaction reaches ________, the concentration of the reactants and products will no longer change.

Correct Answer
verified

Correct Answer
verified

The following reactions occur at 500 K. Arrange them in order of increasing tendency to proceed to completion (least completion → greatest completion) .

Correct Answer
verified

Which equation is correct?

Correct Answer
verified

Exam 15: Chemical Equilibrium

For the equilibrium A2(g) 2A(g) , if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between Kc and time as equilibrium is established?

Correct AnswerverifiedShow Answer

5.00 mol of ammonia are introduced into a 5.00-L reactor vessel in which it partially dissociates at high temperatures. 2NH3(g) 3H2(g) + N2(g) At equilibrium at a particular temperature, 1.00 mole of ammonia remains. Calculate Kc for the reaction.

Correct AnswerverifiedShow Answer

Phosgene, COCl2, a poisonous gas, decomposes as follows. COCl2(g) CO(g) + Cl2(g) . At 900.ºC, Kc = 0.083. What is KP at this temperature? (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g) 2NH3(g)

Correct AnswerverifiedShow Answer

At 400ºC, Kc = 64 for the equilibrium H2(g) + I2(g) 2HI(g) . If 3.00 mol H2 and 3.00 mol I2 are introduced into an empty 4.0-L vessel, what is the equilibrium concentration of HI at 400ºC?

Correct AnswerverifiedShow Answer

Consider the reaction N2(g) + 3H2(g) 2NH3(g). If nitrogen is added to the system at equilibrium, what will happen to the ammonia concentration?

Correct AnswerverifiedThe ammoni...View AnswerShow Answer

For the reaction 2X(g) + Y(g) 2Z(g) , Kc = 1.00 ×103 at 500 K. If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g) + Cl2(g) . What is KP for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol. (R = 8.314 J/K • mol)

Correct AnswerverifiedShow Answer

The reaction 2H2O2(g) 2H2O(g) + O2(g) is exothermic, ΔHºrxn = -210 kJ/mol. Which one of the following is correct?

Correct AnswerverifiedShow Answer

Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position, regardless of the physical state of the substance involved.

Correct AnswerverifiedShow Answer

During a chemical reaction, what defines when the concentrations of the reactants and products reach a constant level?

Correct AnswerverifiedShow Answer

Hydrogen iodide decomposes according to the equation 2HI(g) H2(g) + I2(g) , for which Kc = 0.0156 at 400ºC. Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC. What is the concentration of H2 at equilibrium?

Correct AnswerverifiedShow Answer

At what temperature is KP = 4.00 for the reaction N2O4(g) 2NO2(g) ? (R = 8.314 J/K • mol)

Correct AnswerverifiedShow Answer

Consider the reaction N2(g) + O2(g) 2NO(g) , for which Kc = 0.10 at 2000ºC. Starting with initial concentrations of 0.040 M for N2 and 0.040 M for O2 what is the equilibrium concentration of NO?

Correct AnswerverifiedShow Answer

For the reaction 2NOCl(g) 2NO(g) + Cl2(g) , Kc = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 - reaction vessel in order that the equilibrium concentration of NOCl is 1.00 M?

Correct AnswerverifiedShow Answer

When a reaction reaches ________, the concentration of the reactants and products will no longer change.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The following reactions occur at 500 K. Arrange them in order of increasing tendency to proceed to completion (least completion → greatest completion) .

Correct AnswerverifiedShow Answer

Which equation is correct?

Correct AnswerverifiedShow Answer

For the equilibrium A₂(g) 2A(g) , if a sample of A₂(g) is placed in a sealed container and allowed to come to equilibrium, which graph best represents the relationship between K_c and time as equilibrium is established?

Correct Answer
verified

5.00 mol of ammonia are introduced into a 5.00-L reactor vessel in which it partially dissociates at high temperatures. 2NH₃(g) 3H₂(g) + N₂(g) At equilibrium at a particular temperature, 1.00 mole of ammonia remains. Calculate K_c for the reaction.

Correct Answer
verified

Phosgene, COCl₂, a poisonous gas, decomposes as follows. COCl₂(g) CO(g) + Cl₂(g) . At 900.ºC, K_c = 0.083. What is K_P at this temperature? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H₂(g) + N₂(g) 2NH₃(g)

Correct Answer
verified

At 400ºC, K_c = 64 for the equilibrium H₂(g) + I₂(g) 2HI(g) . If 3.00 mol H₂ and 3.00 mol I₂ are introduced into an empty 4.0-L vessel, what is the equilibrium concentration of HI at 400ºC?

Correct Answer
verified

Consider the reaction N₂(g) + 3H₂(g) 2NH₃(g). If nitrogen is added to the system at equilibrium, what will happen to the ammonia concentration?

Correct Answer
verified
The ammoni...
View Answer

For the reaction 2X(g) + Y(g) 2Z(g) , K_c = 1.00 ×10³ at 500 K. If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?

Correct Answer
verified

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

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g) + Cl₂(g) . What is K_P for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol. (R = 8.314 J/K • mol)

Correct Answer
verified

The reaction 2H₂O₂(g) 2H₂O(g) + O₂(g) is exothermic, ΔHº_rxn=-210 kJ/mol. Which one of the following is correct?

Correct Answer
verified

Correct Answer
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Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + I₂(g) , for which K_c = 0.0156 at 400ºC. Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC. What is the concentration of H₂ at equilibrium?

Correct Answer
verified

At what temperature is K_P = 4.00 for the reaction N₂O₄(g) 2NO₂(g) ? (R = 8.314 J/K • mol)

Correct Answer
verified

Consider the reaction N₂(g) + O₂(g) 2NO(g) , for which K_c = 0.10 at 2000ºC. Starting with initial concentrations of 0.040 M for N₂ and 0.040 M for O₂ what is the equilibrium concentration of NO?

Correct Answer
verified

For the reaction 2NOCl(g) 2NO(g) + Cl₂(g) , K_c = 8.0 at a certain temperature. What concentration of NOCl must be put into an empty 4.00 - reaction vessel in order that the equilibrium concentration of NOCl is 1.00 M?

Correct Answer
verified

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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