Question 1

Given the following reaction at equilibrium, if Kc = 6.34 x 105 at 230.0°C, Kp = __________. 2NO (g) + O2 (g)  c = 6.34 x 105 at 230.0°C, Kp = __________. 2NO (g) + O2 (g)    2NO2 (g)  A) 3.67 × 10-2 B) 1.53 × 104 C) 6.44 × 105 D) 2.61 × 106 E) 2.62 × 107" class="answers-bank-image d-inline" rel="preload" > 2NO2 (g)

Accepted Answer

A)  3.67 × 10-2
B)  1.53 × 104
C)  6.44 × 105
D)  2.61 × 106
E)  2.62 × 107

Question 2

The value of Keq for the equilibrium H2 (g) + I2 (g)  eq for the equilibrium H2 (g) + I2 (g)    2 HI (g)  Is 794 at 25 °C. What is the value of Keq for the equilibrium below? 1/2 H2 (g) + 1/2 I2 (g)    HI (g)  A) 397 B) 0.035 C) 28 D) 1588 E) 0.0013" class="answers-bank-image d-inline" rel="preload" > 2 HI (g) 
Is 794 at 25 °C. What is the value of Keq for the equilibrium below?
1/2 H2 (g) + 1/2 I2 (g)  eq for the equilibrium H2 (g) + I2 (g)    2 HI (g)  Is 794 at 25 °C. What is the value of Keq for the equilibrium below? 1/2 H2 (g) + 1/2 I2 (g)    HI (g)  A) 397 B) 0.035 C) 28 D) 1588 E) 0.0013" class="answers-bank-image d-inline" rel="preload" > HI (g)

Accepted Answer

A)  397
B)  0.035
C)  28
D)  1588
E)  0.0013

Question 3

A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2 (g) + Br2 (g)  2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2 (g) + Br2 (g)    2IBr (g)  When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is __________. A) 11 B) 4.0 C) 110 D) 6.1 E) 2.8" class="answers-bank-image d-inline" rel="preload" > 2IBr (g) 
When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is __________.

Accepted Answer

A)  11
B)  4.0
C)  110
D)  6.1
E)  2.8

Question 4

Of the following equilibria, only __________ will shift to the right in response to a decrease in volume.

Accepted Answer

A)  H2 (g) + Cl2 (g)  2 (g) + Cl2 (g)    2 HCl (g)  
B)  2 SO3 (g)    2 SO2 (g) + O2 (g)  
C)  N2 (g) + 3 H2 (g)    2 NH3 (g)  
D)  2 Fe2O3 (s)    4 Fe (s) + 3 O2 (g)  
E)  2HI (g)    H2 (g) + I2 (g) " class="answers-bank-image d-inline" rel="preload" > 2 HCl (g) 
B)  2 SO3 (g)  2 (g) + Cl2 (g)    2 HCl (g)  
B)  2 SO3 (g)    2 SO2 (g) + O2 (g)  
C)  N2 (g) + 3 H2 (g)    2 NH3 (g)  
D)  2 Fe2O3 (s)    4 Fe (s) + 3 O2 (g)  
E)  2HI (g)    H2 (g) + I2 (g) " class="answers-bank-image d-inline" rel="preload" > 2 SO2 (g) + O2 (g) 
C)  N2 (g) + 3 H2 (g)  2 (g) + Cl2 (g)    2 HCl (g)  
B)  2 SO3 (g)    2 SO2 (g) + O2 (g)  
C)  N2 (g) + 3 H2 (g)    2 NH3 (g)  
D)  2 Fe2O3 (s)    4 Fe (s) + 3 O2 (g)  
E)  2HI (g)    H2 (g) + I2 (g) " class="answers-bank-image d-inline" rel="preload" > 2 NH3 (g) 
D)  2 Fe2O3 (s)  2 (g) + Cl2 (g)    2 HCl (g)  
B)  2 SO3 (g)    2 SO2 (g) + O2 (g)  
C)  N2 (g) + 3 H2 (g)    2 NH3 (g)  
D)  2 Fe2O3 (s)    4 Fe (s) + 3 O2 (g)  
E)  2HI (g)    H2 (g) + I2 (g) " class="answers-bank-image d-inline" rel="preload" > 4 Fe (s) + 3 O2 (g) 
E)  2HI (g)  2 (g) + Cl2 (g)    2 HCl (g)  
B)  2 SO3 (g)    2 SO2 (g) + O2 (g)  
C)  N2 (g) + 3 H2 (g)    2 NH3 (g)  
D)  2 Fe2O3 (s)    4 Fe (s) + 3 O2 (g)  
E)  2HI (g)    H2 (g) + I2 (g) " class="answers-bank-image d-inline" rel="preload" > H2 (g) + I2 (g)

Question 5

Consider the following reaction at equilibrium: 2NH3 (g)  3 (g)    N2 (g) + 3H2 (g)  Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with __________. A) some removal of NH3 from the reaction vessel (V and T constant)  B) a decrease in the total pressure (T constant)  C) addition of some N2 to the reaction vessel (V and T constant)  D) a decrease in the total volume of the reaction vessel (T constant)  E) an increase in total pressure by the addition of helium gas (V and T constant) " class="answers-bank-image d-inline" rel="preload" > N2 (g) + 3H2 (g) 
Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with __________.

Accepted Answer

A)  some removal of NH3 from the reaction vessel (V and T constant) 
B)  a decrease in the total pressure (T constant) 
C)  addition of some N2 to the reaction vessel (V and T constant) 
D)  a decrease in the total volume of the reaction vessel (T constant) 
E)  an increase in total pressure by the addition of helium gas (V and T constant)

Question 6

Given the following reaction at equilibrium, if Kp = 0.990 at 250.0°C, Kc = __________. PCl5 (g)  p = 0.990 at 250.0°C, Kc = __________. PCl5 (g)    PCl3 (g) + Cl2 (g)  A) 3.90 × 10-6 B) 2.31 × 10-2 C) 0.990 D) 42.9 E) 42.5" class="answers-bank-image d-inline" rel="preload" > PCl3 (g) + Cl2 (g)

Accepted Answer

A)  3.90 × 10-6
B)  2.31 × 10-2
C)  0.990
D)  42.9
E)  42.5

Question 7

The equilibrium constant for the gas phase reaction 2SO2 (g) + O2 (g)  2 (g) + O2 (g)    2SO3 (g)  Is Keq = 2.80 × 102 at 999 K. At equilibrium, __________. A) products predominate B) reactants predominate C) roughly equal amounts of products and reactants are present D) only products are present E) only reactants are present" class="answers-bank-image d-inline" rel="preload" > 2SO3 (g) 
Is Keq = 2.80 × 102 at 999 K. At equilibrium, __________.

Accepted Answer

A)  products predominate
B)  reactants predominate
C)  roughly equal amounts of products and reactants are present
D)  only products are present
E)  only reactants are present

Question 8

Given the following reaction: CO (g) + 2H2(g)  2(g)    CH3OH (g)  In an experiment, 0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. Keq at the temperature of the experiment is __________. A) 2.80 B) 0.357 C) 14.5 D) 17.5 E) none of the above" class="answers-bank-image d-inline" rel="preload" > CH3OH (g) 
In an experiment, 0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. Keq at the temperature of the experiment is __________.

Accepted Answer

A)  2.80
B)  0.357
C)  14.5
D)  17.5
E)  none of the above

Question 9

Consider the following equilibrium. 2SO2 (g) + O2 (g)  2 (g) + O2 (g)    2SO3 (g)  The equilibrium cannot be established when __________ is/are placed in a 1.0-L container. A) 0.25 mol SO2 (g) and 0.25 mol O2 (g)  B) 0.75 mol SO2 (g)  C) 0.25 mol of SO2 (g) and 0.25 mol of SO3 (g)  D) 0.50 mol O2 (g) and 0.50 mol SO3 (g)  E) 1.0 mol SO3 (g) " class="answers-bank-image d-inline" rel="preload" > 2SO3 (g) 
The equilibrium cannot be established when __________ is/are placed in a 1.0-L container.

Accepted Answer

A)  0.25 mol SO2 (g) and 0.25 mol O2 (g) 
B)  0.75 mol SO2 (g) 
C)  0.25 mol of SO2 (g) and 0.25 mol of SO3 (g) 
D)  0.50 mol O2 (g) and 0.50 mol SO3 (g) 
E)  1.0 mol SO3 (g)

Question 10

The equilibrium expression for Kp for the reaction below is __________. N2 (g) + O2 (g)  p for the reaction below is __________. N2 (g) + O2 (g)    2NO (g)  A)    B)    C)    D)    E) none of the above" class="answers-bank-image d-inline" rel="preload" > 2NO (g)

Accepted Answer

A)   p for the reaction below is __________. N2 (g) + O2 (g)    2NO (g)  
A)     
B)     
C)     
D)     
E)  none of the above" class="answers-bank-image d-inline" rel="preload" >
B)   p for the reaction below is __________. N2 (g) + O2 (g)    2NO (g)  
A)     
B)     
C)     
D)     
E)  none of the above" class="answers-bank-image d-inline" rel="preload" >
C)   p for the reaction below is __________. N2 (g) + O2 (g)    2NO (g)  
A)     
B)     
C)     
D)     
E)  none of the above" class="answers-bank-image d-inline" rel="preload" >
D)   p for the reaction below is __________. N2 (g) + O2 (g)    2NO (g)  
A)     
B)     
C)     
D)     
E)  none of the above" class="answers-bank-image d-inline" rel="preload" >
E)  none of the above

Question 11

If the value for the equilibrium constant is much greater than 1, then the equilibrium mixture contains mostly __________.

Accepted Answer

The answer of If the value for the equilibrium constant...

Question 12

Consider the following reaction at equilibrium: 2NH3 (g)  3 (g)    N2 (g) + 3H2 (g) ΔH° = +92.4 kJ Le Châtelier's principle predicts that adding N2 (g) to the system at equilibrium will result in __________. A) a decrease in the concentration of NH3 (g)  B) a decrease in the concentration of H2 (g)  C) an increase in the value of the equilibrium constant D) a lower partial pressure of N2 E) removal of all of the H2 (g) " class="answers-bank-image d-inline" rel="preload" > N2 (g) + 3H2 (g) ΔH° = +92.4 kJ
Le Châtelier's principle predicts that adding N2 (g) to the system at equilibrium will result in __________.

Accepted Answer

A)  a decrease in the concentration of NH3 (g) 
B)  a decrease in the concentration of H2 (g) 
C)  an increase in the value of the equilibrium constant
D)  a lower partial pressure of N2
E)  removal of all of the H2 (g)

Question 13

At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g)  2 (g) + Cl2 (g)    2BrCl (g)  Is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g) , 1.00 atm of Cl2 (g) , and 2.00 atm of BrCl (g) . Use Q to determine which of the statements below is true. A) The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial values. B) The equilibrium partial pressure of Br2 will be greater than 1.00 atm. C) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. D) The equilibrium partial pressure of BrCl (g) will be greater than 2.00 atm. E) The reaction will go to completion since there are equal amounts of Br2 and Cl2." class="answers-bank-image d-inline" rel="preload" > 2BrCl (g) 
Is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g) , 1.00 atm of Cl2 (g) , and 2.00 atm of BrCl (g) . Use Q to determine which of the statements below is true.

Accepted Answer

A)  The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial values.
B)  The equilibrium partial pressure of Br2 will be greater than 1.00 atm.
C)  At equilibrium, the total pressure in the vessel will be less than the initial total pressure.
D)  The equilibrium partial pressure of BrCl (g) will be greater than 2.00 atm.
E)  The reaction will go to completion since there are equal amounts of Br2 and Cl2.

Question 14

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? (NH4) 2Se (s)  4) 2Se (s)    2NH3 (g) + H2Se (g)  A) [NH3][H2Se] / [(NH4) 2Se] B) [(NH4) 2Se] / [NH3]2[H2Se] C) 1 / [(NH4) 2Se] D) [NH3]2[H2Se] E) [NH3]2[H2Se] / [(NH4) 2Se]" class="answers-bank-image d-inline" rel="preload" > 2NH3 (g) + H2Se (g)

Accepted Answer

A)  [NH3][H2Se] / [(NH4) 2Se]
B)  [(NH4) 2Se] / [NH3]2[H2Se]
C)  1 / [(NH4) 2Se]
D)  [NH3]2[H2Se]
E)  [NH3]2[H2Se] / [(NH4) 2Se]

Question 15

Which of the following statements is true?

Accepted Answer

A)  Q does not change with temperature.
B)  Keq does not change with temperature, whereas Q is temperature dependent.
C)  K does not depend on the concentrations or partial pressures of reaction components.
D)  Q does not depend on the concentrations or partial pressures of reaction components.
E)  Q is the same as Keq when a reaction is at equilibrium.

Question 16

At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 + O2 (g)  p) for the following reaction is 0.345. 2SO2 + O2 (g)    2SO3 (g)  At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is __________ atm. A) 82.0 B) 4.21 × 10-3 C) 192 D) 6.20 × 10-4 E) 40.2" class="answers-bank-image d-inline" rel="preload" > 2SO3 (g) 
At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is __________ atm.

Accepted Answer

A)  82.0
B)  4.21 × 10-3
C)  192
D)  6.20 × 10-4
E)  40.2

Question 17

At 200°C, the equilibrium constant (Kp) for the reaction below is 2.40 × 103. 2NO (g)  p) for the reaction below is 2.40 × 103. 2NO (g)    N2 (g) + O2 (g)  A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is __________ atm. A) 294 B) 35.7 C) 17.9 D) 6.00 E) 1.50 × 10-2" class="answers-bank-image d-inline" rel="preload" > N2 (g) + O2 (g) 
A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is __________ atm.

Accepted Answer

A)  294
B)  35.7
C)  17.9
D)  6.00
E)  1.50 × 10-2

Question 18

The value of Keq for the equilibrium H2 (g) + I2 (g)  eq for the equilibrium H2 (g) + I2 (g)    2 HI (g)  Is 794 at 25°C. At this temperature, what is the value of Keq for the equilibrium below? HI (g)    1/2 H2 (g) + 1/2 I2 (g)  A) 1588 B) 28 C) 397 D) 0.035 E) 0.0013" class="answers-bank-image d-inline" rel="preload" > 2 HI (g) 
Is 794 at 25°C. At this temperature, what is the value of Keq for the equilibrium below?
HI (g)  eq for the equilibrium H2 (g) + I2 (g)    2 HI (g)  Is 794 at 25°C. At this temperature, what is the value of Keq for the equilibrium below? HI (g)    1/2 H2 (g) + 1/2 I2 (g)  A) 1588 B) 28 C) 397 D) 0.035 E) 0.0013" class="answers-bank-image d-inline" rel="preload" > 1/2 H2 (g) + 1/2 I2 (g)

Accepted Answer

A)  1588
B)  28
C)  397
D)  0.035
E)  0.0013

Question 19

The effect of a catalyst on an equilibrium is to __________.

Accepted Answer

A)  increase the rate of the forward reaction only
B)  increase the equilibrium constant so that products are favored
C)  slow the reverse reaction only
D)  increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture
E)  shift the equilibrium to the right

Question 20

The Kp for the reaction below is 1.49 × 108 at 100.0°C: CO (g) + Cl2 (g)  p for the reaction below is 1.49 × 108 at 100.0°C: CO (g) + Cl2 (g)    COCl2 (g)  In an equilibrium mixture of the three gases, PCO = PCl2 = 2.22 × 10-4 atm. The partial pressure of the product, phosgene (COCl2) , is __________ atm. A) 7.34 B) 3.02 × 1015 C) 3.31 × 10-16 D) 3.31 × 104 E) 6.67 × 1011" class="answers-bank-image d-inline" rel="preload" > COCl2 (g) 
In an equilibrium mixture of the three gases, PCO = PCl2 = 2.22 × 10-4 atm. The partial pressure of the product, phosgene (COCl2) , is __________ atm.

Accepted Answer

A)  7.34
B)  3.02 × 1015
C)  3.31 × 10-16
D)  3.31 × 104
E)  6.67 × 1011

Exam 15: Chemical Equilibrium

The effect of a catalyst on an equilibrium is to __________.

Correct AnswerverifiedShow Answer

At 200°C, the equilibrium constant (Kp) for the reaction below is 2.40 × 103. 2NO (g) N2 (g) + O2 (g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is __________ atm.

Correct AnswerverifiedShow Answer

The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) Is 794 at 25°C. At this temperature, what is the value of Keq for the equilibrium below? HI (g) 1/2 H2 (g) + 1/2 I2 (g)

Correct AnswerverifiedShow Answer

Given the following reaction at equilibrium, if Kp = 0.990 at 250.0°C, Kc = __________. PCl5 (g) PCl3 (g) + Cl2 (g)

Correct AnswerverifiedShow Answer

The equilibrium expression for Kp for the reaction below is __________. N2 (g) + O2 (g) 2NO (g)

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Given the following reaction: CO (g) + 2H2(g) CH3OH (g) In an experiment, 0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. Keq at the temperature of the experiment is __________.

Correct AnswerverifiedShow Answer

Which of the following statements is true?

Correct AnswerverifiedShow Answer

At 400 K, the equilibrium constant for the reaction Br2 (g) + Cl2 (g) 2BrCl (g) Is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g) , 1.00 atm of Cl2 (g) , and 2.00 atm of BrCl (g) . Use Q to determine which of the statements below is true.

Correct AnswerverifiedShow Answer

A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2 (g) + Br2 (g) 2IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is __________.

Correct AnswerverifiedShow Answer

The equilibrium constant for the gas phase reaction 2SO2 (g) + O2 (g) 2SO3 (g) Is Keq = 2.80 × 102 at 999 K. At equilibrium, __________.

Correct AnswerverifiedShow Answer

If the value for the equilibrium constant is much greater than 1, then the equilibrium mixture contains mostly __________.

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Of the following equilibria, only __________ will shift to the right in response to a decrease in volume.

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Consider the following reaction at equilibrium: 2NH3 (g) N2 (g) + 3H2 (g) Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with __________.

Correct AnswerverifiedShow Answer

Consider the following reaction at equilibrium: 2NH3 (g) N2 (g) + 3H2 (g) ΔH° = +92.4 kJ Le Châtelier's principle predicts that adding N2 (g) to the system at equilibrium will result in __________.

Correct AnswerverifiedShow Answer

At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 + O2 (g) 2SO3 (g) At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is __________ atm.

Correct AnswerverifiedShow Answer

The Kp for the reaction below is 1.49 × 108 at 100.0°C: CO (g) + Cl2 (g) COCl2 (g) In an equilibrium mixture of the three gases, PCO = PCl2 = 2.22 × 10-4 atm. The partial pressure of the product, phosgene (COCl2) , is __________ atm.

Correct AnswerverifiedShow Answer

Given the following reaction at equilibrium, if Kc = 6.34 x 105 at 230.0°C, Kp = __________. 2NO (g) + O2 (g) 2NO2 (g)

Correct AnswerverifiedShow Answer

The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) Is 794 at 25 °C. What is the value of Keq for the equilibrium below? 1/2 H2 (g) + 1/2 I2 (g) HI (g)

Correct AnswerverifiedShow Answer

Consider the following equilibrium. 2SO2 (g) + O2 (g) 2SO3 (g) The equilibrium cannot be established when __________ is/are placed in a 1.0-L container.

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Which of the following expressions is the correct equilibrium-constant expression for the reaction below? (NH4) 2Se (s) 2NH3 (g) + H2Se (g)

Correct AnswerverifiedShow Answer

Correct Answer
verified

At 200°C, the equilibrium constant (K_p) for the reaction below is 2.40 × 10³. 2NO (g) N₂ (g) + O₂ (g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O₂ is __________ atm.

Correct Answer
verified

The value of K_eq for the equilibrium H₂ (g) + I₂ (g) 2 HI (g) Is 794 at 25°C. At this temperature, what is the value of K_e_q for the equilibrium below? HI (g) 1/2 H₂ (g) + 1/2 I₂ (g)

Correct Answer
verified

Given the following reaction at equilibrium, if K_p = 0.990 at 250.0°C, K_c = __________. PCl₅ (g) PCl₃ (g) + Cl₂ (g)

Correct Answer
verified

The equilibrium expression for K_p for the reaction below is __________. N₂ (g) + O₂ (g) 2NO (g)

Correct Answer
verified

Given the following reaction: CO (g) + 2H₂(g) CH₃OH (g) In an experiment, 0.42 mol of CO and 0.42 mol of H₂ were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. K_eq at the temperature of the experiment is __________.

Correct Answer
verified

Correct Answer
verified

At 400 K, the equilibrium constant for the reaction Br₂ (g) + Cl₂ (g) 2BrCl (g) Is K_p = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br₂(g) , 1.00 atm of Cl₂ (g) , and 2.00 atm of BrCl (g) . Use Q to determine which of the statements below is true.

Correct Answer
verified

A sealed 1.0 L flask is charged with 0.500 mol of I₂ and 0.500 mol of Br₂. An equilibrium reaction ensues: I₂ (g) + Br₂ (g) 2IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of K_eq is __________.

Correct Answer
verified

The equilibrium constant for the gas phase reaction 2SO₂ (g) + O₂ (g) 2SO₃ (g) Is K_eq = 2.80 × 10² at 999 K. At equilibrium, __________.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Consider the following reaction at equilibrium: 2NH₃ (g) N₂ (g) + 3H₂ (g) Le Châtelier's principle predicts that the moles of H₂ in the reaction container will increase with __________.

Correct Answer
verified

Consider the following reaction at equilibrium: 2NH₃ (g) N₂ (g) + 3H₂ (g) ΔH° = +92.4 kJ Le Châtelier's principle predicts that adding N₂ (g) to the system at equilibrium will result in __________.

Correct Answer
verified

At 900.0 K, the equilibrium constant (K_p) for the following reaction is 0.345. 2SO₂ + O₂ (g) 2SO₃ (g) At equilibrium, the partial pressure of SO₂ is 35.0 atm and that of O₂ is 15.9 atm. The partial pressure of SO₃ is __________ atm.

Correct Answer
verified

The K_p for the reaction below is 1.49 × 10⁸ at 100.0°C: CO (g) + Cl₂ (g) COCl₂ (g) In an equilibrium mixture of the three gases, PCO = PCl₂ = 2.22 × 10^-4 atm. The partial pressure of the product, phosgene (COCl₂) , is __________ atm.

Correct Answer
verified

Given the following reaction at equilibrium, if K_c = 6.34 x 10⁵at 230.0°C, K_p = __________. 2NO (g) + O₂ (g) 2NO₂ (g)

Correct Answer
verified

The value of K_eq for the equilibrium H₂ (g) + I₂ (g) 2 HI (g) Is 794 at 25 °C. What is the value of K_eq for the equilibrium below? 1/2 H₂ (g) + 1/2 I₂ (g) HI (g)

Correct Answer
verified

Consider the following equilibrium. 2SO₂ (g) + O₂ (g) 2SO₃ (g) The equilibrium cannot be established when __________ is/are placed in a 1.0-L container.

Correct Answer
verified

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? (NH₄) ₂Se (s) 2NH₃ (g) + H₂Se (g)

Correct Answer
verified