Question 1

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 2

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

Question 3

The Keq for the equilibrium below is 0.112 at 700.0 °C. SO2 (g)  + eq for the equilibrium below is 0.112 at 700.0 °C. SO2 (g)  +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? 2SO2 (g)  + O2 (g)    2SO3 (g)  A) 1.25 × 10-2 B) 2.24 × 10-1 C) 7.97 × 101 D) 4.46 E) 0.112" class="answers-bank-image d-inline" rel="preload" > O2 (g)  eq for the equilibrium below is 0.112 at 700.0 °C. SO2 (g)  +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? 2SO2 (g)  + O2 (g)    2SO3 (g)  A) 1.25 × 10-2 B) 2.24 × 10-1 C) 7.97 × 101 D) 4.46 E) 0.112" class="answers-bank-image d-inline" rel="preload" > SO3 (g) 
What is the value of Keq at this temperature for the following reaction?
2SO2 (g)  + O2 (g)  eq for the equilibrium below is 0.112 at 700.0 °C. SO2 (g)  +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? 2SO2 (g)  + O2 (g)    2SO3 (g)  A) 1.25 × 10-2 B) 2.24 × 10-1 C) 7.97 × 101 D) 4.46 E) 0.112" class="answers-bank-image d-inline" rel="preload" > 2SO3 (g)

Accepted Answer

A)  1.25 × 10-2
B)  2.24 × 10-1
C)  7.97 × 101
D)  4.46
E)  0.112

Question 4

The value of Keq for the equilibrium H2 (g)  + I2 (g)  eq for the equilibrium H2 (g)  + I2 (g)    2HI (g)  Is 54.0 at 427 °C. What is the value of Keq for the equilibrium below? HI (g)      H2 (g)  +   I2(g)  A) 27 B) 7.35 C) 0.136 D) 2.92 × 103 E) 3.43 × 10-4" class="answers-bank-image d-inline" rel="preload" > 2HI (g) 
Is 54.0 at 427 °C. What is the value of Keq for the equilibrium below?
HI (g)  eq for the equilibrium H2 (g)  + I2 (g)    2HI (g)  Is 54.0 at 427 °C. What is the value of Keq for the equilibrium below? HI (g)      H2 (g)  +   I2(g)  A) 27 B) 7.35 C) 0.136 D) 2.92 × 103 E) 3.43 × 10-4" class="answers-bank-image d-inline" rel="preload" > eq for the equilibrium H2 (g)  + I2 (g)    2HI (g)  Is 54.0 at 427 °C. What is the value of Keq for the equilibrium below? HI (g)      H2 (g)  +   I2(g)  A) 27 B) 7.35 C) 0.136 D) 2.92 × 103 E) 3.43 × 10-4" class="answers-bank-image d-inline" rel="preload" > H2 (g)  + eq for the equilibrium H2 (g)  + I2 (g)    2HI (g)  Is 54.0 at 427 °C. What is the value of Keq for the equilibrium below? HI (g)      H2 (g)  +   I2(g)  A) 27 B) 7.35 C) 0.136 D) 2.92 × 103 E) 3.43 × 10-4" class="answers-bank-image d-inline" rel="preload" > I2(g)

Accepted Answer

A)  27
B)  7.35
C)  0.136
D)  2.92 × 103
E)  3.43 × 10-4

Question 5

The value of Keq for the following reaction is 0.25: SO2 (g)  + NO2 (g)  eq for the following reaction is 0.25: SO2 (g)  + NO2 (g)    SO3 (g)  + NO (g)  The value of Keq at the same temperature for the reaction below is ________. 3SO2 (g)  + 3NO2 (g)    3SO3 (g)  + 3NO (g)  A) 1.6 × 10-2 B) 7.5 × 10-1 C) 8.3 × 10-2 D) 6.4 × 101 E) 0.25" class="answers-bank-image d-inline" rel="preload" > SO3 (g)  + NO (g) 
The value of Keq at the same temperature for the reaction below is ________.
3SO2 (g)  + 3NO2 (g)  eq for the following reaction is 0.25: SO2 (g)  + NO2 (g)    SO3 (g)  + NO (g)  The value of Keq at the same temperature for the reaction below is ________. 3SO2 (g)  + 3NO2 (g)    3SO3 (g)  + 3NO (g)  A) 1.6 × 10-2 B) 7.5 × 10-1 C) 8.3 × 10-2 D) 6.4 × 101 E) 0.25" class="answers-bank-image d-inline" rel="preload" > 3SO3 (g)  + 3NO (g)

Accepted Answer

A)  1.6 × 10-2
B)  7.5 × 10-1
C)  8.3 × 10-2
D)  6.4 × 101
E)  0.25

Question 6

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

Accepted Answer

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

Question 7

Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)  2 (g)  A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.16 mol of NOBr. How many moles of NO and Br2, respectively, are in the flask at equilibrium? A) 0.48, 0.24 B) 0.48, 0.48 C) 0.16, 0.08 D) 0.16, 0.16 E) 0.24, 0.42" class="answers-bank-image d-inline" rel="preload" > 2NO (g)  + Br2 (g) 
A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.16 mol of NOBr. How many moles of NO and Br2, respectively, are in the flask at equilibrium?

Accepted Answer

A)  0.48, 0.24
B)  0.48, 0.48
C)  0.16, 0.08
D)  0.16, 0.16
E)  0.24, 0.42

Question 8

Exactly 3.5 moles if N2O4 is placed in an empty 2.0-L container and allowed to reach equilibrium described by the equation
N2O4 (g)⇌ 2NO2 (g)
If at equilibrium the N2O4 is 25% dissociated, what is the value of the equilibrium constant for the reaction?

Accepted Answer

Question 9

The value of Keq for the equilibrium H2 (g)  + I2 (g)  eq for the equilibrium H2 (g)  + I2 (g)    2HI (g)  Is 794 at 25 °C. What is the value of Keq for the equilibrium below?   H2 (g)  +   I2 (g)    HI (g)  A) 397 B) 0.035 C) 28 D) 1588 E) 0.0013" class="answers-bank-image d-inline" rel="preload" > 2HI (g) 
Is 794 at 25 °C. What is the value of Keq for the equilibrium below? eq for the equilibrium H2 (g)  + I2 (g)    2HI (g)  Is 794 at 25 °C. What is the value of Keq for the equilibrium below?   H2 (g)  +   I2 (g)    HI (g)  A) 397 B) 0.035 C) 28 D) 1588 E) 0.0013" class="answers-bank-image d-inline" rel="preload" > H2 (g)  + eq for the equilibrium H2 (g)  + I2 (g)    2HI (g)  Is 794 at 25 °C. What is the value of Keq for the equilibrium below?   H2 (g)  +   I2 (g)    HI (g)  A) 397 B) 0.035 C) 28 D) 1588 E) 0.0013" class="answers-bank-image d-inline" rel="preload" > I2 (g)  eq for the equilibrium H2 (g)  + I2 (g)    2HI (g)  Is 794 at 25 °C. What is the value of Keq for the equilibrium below?   H2 (g)  +   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 10

What role did Karl Bosch play in development of the Haber-Bosch process?

Accepted Answer

A)  He discovered the reaction conditions necessary for formation of ammonia.
B)  He originally isolated ammonia from camel dung and found a method for purifying it.
C)  Haber was working in his lab with his instructor at the time he worked out the process.
D)  He developed the equipment necessary for industrial production of ammonia.
E)  He was the German industrialist who financed the research done by Haber.

Question 11

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 12

For an exothermic reaction, increasing the reaction temperature results in a(n)________ in K.

Accepted Answer

The answer of For an exothermic reaction, increasing the reaction...

Question 13

Consider the following reaction at equilibrium. 2CO2 (g)  2 (g)    2CO (g)  + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________. A) at high temperature and high pressure B) at high temperature and low pressure C) at low temperature and low pressure D) at low temperature and high pressure E) in the presence of solid carbon" class="answers-bank-image d-inline" rel="preload" > 2CO (g)  + O2 (g) ΔH° = -514 kJ
Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________.

Accepted Answer

A)  at high temperature and high pressure
B)  at high temperature and low pressure
C)  at low temperature and low pressure
D)  at low temperature and high pressure
E)  in the presence of solid carbon

Question 14

The expression for Kp for the reaction below is ________. 4CuO (s)  + CH4 (g)  p for the reaction below is ________. 4CuO (s)  + CH4 (g)    CO2 (g)  + 4Cu (s)  + 2H2O (g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > CO2 (g)  + 4Cu (s)  + 2H2O (g)

Accepted Answer

A)   p for the reaction below is ________. 4CuO (s)  + CH4 (g)    CO2 (g)  + 4Cu (s)  + 2H2O (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   p for the reaction below is ________. 4CuO (s)  + CH4 (g)    CO2 (g)  + 4Cu (s)  + 2H2O (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   p for the reaction below is ________. 4CuO (s)  + CH4 (g)    CO2 (g)  + 4Cu (s)  + 2H2O (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   p for the reaction below is ________. 4CuO (s)  + CH4 (g)    CO2 (g)  + 4Cu (s)  + 2H2O (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   p for the reaction below is ________. 4CuO (s)  + CH4 (g)    CO2 (g)  + 4Cu (s)  + 2H2O (g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 15

Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC2H3O2 (aq)  2H3O2 (aq)    C2H3O2- (aq)  + H+ (aq)  At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: [HC2H3O2] = 0.0990 M, [C2H3O2-] = 1.33 × 10-3 M and [H+] = 1.33 × 10-3 M. The equilibrium constant, Keq, for the ionization of acetic acid at 25 °C is ________. A) 5.71 × 104 B) 0.100 C) 1.75 × 10-7 D) 1.79 × 10-5 E) 5.71 × 106" class="answers-bank-image d-inline" rel="preload" > C2H3O2- (aq)  + H+ (aq) 
At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations:
[HC2H3O2] = 0.0990 M, [C2H3O2-] = 1.33 × 10-3 M and [H+] = 1.33 × 10-3 M. The equilibrium constant, Keq, for the ionization of acetic acid at 25 °C is ________.

Accepted Answer

A)  5.71 × 104
B)  0.100
C)  1.75 × 10-7
D)  1.79 × 10-5
E)  5.71 × 106

Question 16

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? 5N2O4(g)  2O4(g)    10NO2 (g)  A) [NO2]10/[N2O4]5 B) [N2O4]10/[NO2]5 C) [NO2]5/[N2O4]10 D) [NO2]5/[N2O4]5 E) [N2O4]5/[NO2]5" class="answers-bank-image d-inline" rel="preload" > 10NO2 (g)

Accepted Answer

A)  [NO2]10/[N2O4]5
B)  [N2O4]10/[NO2]5
C)  [NO2]5/[N2O4]10
D)  [NO2]5/[N2O4]5
E)  [N2O4]5/[NO2]5

Question 17

Consider the following reaction at equilibrium: 2CO2 (g)  2 (g)    2CO (g)  + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that an increase in temperature will ________. A) increase the partial pressure of O2 (g)  B) decrease the partial pressure of CO2 (g)  C) decrease the value of the equilibrium constant D) increase the value of the equilibrium constant E) increase the partial pressure of CO" class="answers-bank-image d-inline" rel="preload" > 2CO (g)  + O2 (g) ΔH° = -514 kJ
Le Châtelier's principle predicts that an increase in temperature will ________.

Accepted Answer

A)  increase the partial pressure of O2 (g) 
B)  decrease the partial pressure of CO2 (g) 
C)  decrease the value of the equilibrium constant
D)  increase the value of the equilibrium constant
E)  increase the partial pressure of CO

Question 18

Consider the following chemical reaction: CO (g)  + 2H2(g)  2(g)    CH3OH(g)  At equilibrium in a particular experiment, the concentrations of CO and H2 were 0.15 M and 0.36, M respectively. What is the equilibrium concentration of CH3OH? The value of Keq for this reaction is 14.5 at the temperature of the experiment. A) 14.5 B) 7.61 × 10-3 C) 2.82 × 10-1 D) 3.72 × 10-3 E) 1.34 × 10-3" class="answers-bank-image d-inline" rel="preload" > CH3OH(g) 
At equilibrium in a particular experiment, the concentrations of CO and H2 were 0.15 M and 0.36, M respectively. What is the equilibrium concentration of CH3OH? The value of Keq for this reaction is 14.5 at the temperature of the experiment.

Accepted Answer

A)  14.5
B)  7.61 × 10-3
C)  2.82 × 10-1
D)  3.72 × 10-3
E)  1.34 × 10-3

Question 19

A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g)  2(g)  + I2(g)  When the system comes to equilibrium at 425 °C, PHI = 0.708 atm, and PH2 = PI2 = 0.0960 atm. The value of Kp at this temperature is ________. A) 6.80 × 10-2 B) 1.30 × 10-2 C) 54.3 D) 1.84 × 10-2 E) Kp cannot be calculated for this gas reaction when the volume of the reaction vessel is not given." class="answers-bank-image d-inline" rel="preload" > H2(g)  + I2(g) 
When the system comes to equilibrium at 425 °C, PHI = 0.708 atm, and PH2 = PI2 = 0.0960 atm. The value of Kp at this temperature is ________.

Accepted Answer

A)  6.80 × 10-2
B)  1.30 × 10-2
C)  54.3
D)  1.84 × 10-2
E)  Kp cannot be calculated for this gas reaction when the volume of the reaction vessel is not given.

Question 20

At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles of gas in the system.

Accepted Answer

A) True 
 B)False

Exam 15: Chemical Equilibrium

The value of K_eq for the equilibrium H₂ (g) + I₂ (g) 2HI (g) Is 54.0 at 427 °C. What is the value of K_eq for the equilibrium below? HI (g) H₂ (g) + I₂(g)

Correct Answer
verified

Correct Answer
verified

The value of K_eq for the following reaction is 0.25: SO₂ (g) + NO₂ (g) SO₃ (g) + NO (g) The value of K_eq at the same temperature for the reaction below is ________. 3SO₂ (g) + 3NO₂ (g) 3SO₃ (g) + 3NO (g)

Correct Answer
verified

For an exothermic reaction, increasing the reaction temperature results in a(n)________ in K.

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

Correct Answer
verified

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

Correct Answer
verified

The K_eq for the equilibrium below is 0.112 at 700.0 °C. SO₂ (g) + O₂ (g) SO₃ (g) What is the value of K_eq at this temperature for the following reaction? 2SO₂ (g) + O₂ (g) 2SO₃ (g)

Correct Answer
verified

A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H₂(g) + I₂(g) When the system comes to equilibrium at 425 °C, P_HI = 0.708 atm, and P_H₂ = P_I₂ = 0.0960 atm. The value of K_p at this temperature is ________.

Correct Answer
verified

Consider the following reaction at equilibrium. 2CO₂ (g) 2CO (g) + O₂ (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________.

Correct Answer
verified

Exactly 3.5 moles if N₂O₄ is placed in an empty 2.0-L container and allowed to reach equilibrium described by the equation N₂O₄ (g)⇌ 2NO₂(g) If at equilibrium the N₂O₄ is 25% dissociated, what is the value of the equilibrium constant for the reaction?

Correct Answer
verified

Correct Answer
verified

Consider the following reaction at equilibrium: 2CO₂ (g) 2CO (g) + O₂ (g) ΔH° = -514 kJ Le Châtelier's principle predicts that an increase in temperature will ________.

Correct Answer
verified

What role did Karl Bosch play in development of the Haber-Bosch process?

Correct Answer
verified

At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles of gas in the system.

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

The expression for K_p for the reaction below is ________. 4CuO (s) + CH₄ (g) CO₂ (g) + 4Cu (s) + 2H₂O (g)

Correct Answer
verified

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? 5N₂O4(g) 10NO₂ (g)

Correct Answer
verified

Exam 15: Chemical Equilibrium

The value of Keq for the equilibrium H2 (g) + I2 (g) 2HI (g) Is 54.0 at 427 °C. What is the value of Keq for the equilibrium below? HI (g) H2 (g) + I2(g)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The value of Keq for the following reaction is 0.25: SO2 (g) + NO2 (g) SO3 (g) + NO (g) The value of Keq at the same temperature for the reaction below is ________. 3SO2 (g) + 3NO2 (g) 3SO3 (g) + 3NO (g)

Correct AnswerverifiedShow Answer

For an exothermic reaction, increasing the reaction temperature results in a(n)________ in K.

Correct AnswerverifiedShow Answer

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 AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

The Keq for the equilibrium below is 0.112 at 700.0 °C. SO2 (g) + O2 (g) SO3 (g) What is the value of Keq at this temperature for the following reaction? 2SO2 (g) + O2 (g) 2SO3 (g)

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A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H2(g) + I2(g) When the system comes to equilibrium at 425 °C, PHI = 0.708 atm, and PH2 = PI2 = 0.0960 atm. The value of Kp at this temperature is ________.

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Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________.

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Exactly 3.5 moles if N2O4 is placed in an empty 2.0-L container and allowed to reach equilibrium described by the equation N2O4 (g)⇌ 2NO2 (g) If at equilibrium the N2O4 is 25% dissociated, what is the value of the equilibrium constant for the reaction?

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Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that an increase in temperature will ________.

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What role did Karl Bosch play in development of the Haber-Bosch process?

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At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles of gas in the system.

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

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

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

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The expression for Kp for the reaction below is ________. 4CuO (s) + CH4 (g) CO2 (g) + 4Cu (s) + 2H2O (g)

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Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? 5N2O4(g) 10NO2 (g)

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The value of K_eq for the equilibrium H₂ (g) + I₂ (g) 2HI (g) Is 54.0 at 427 °C. What is the value of K_eq for the equilibrium below? HI (g) H₂ (g) + I₂(g)

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The value of K_eq for the following reaction is 0.25: SO₂ (g) + NO₂ (g) SO₃ (g) + NO (g) The value of K_eq at the same temperature for the reaction below is ________. 3SO₂ (g) + 3NO₂ (g) 3SO₃ (g) + 3NO (g)

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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)

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The K_eq for the equilibrium below is 0.112 at 700.0 °C. SO₂ (g) + O₂ (g) SO₃ (g) What is the value of K_eq at this temperature for the following reaction? 2SO₂ (g) + O₂ (g) 2SO₃ (g)

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A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H₂(g) + I₂(g) When the system comes to equilibrium at 425 °C, P_HI = 0.708 atm, and P_H₂ = P_I₂ = 0.0960 atm. The value of K_p at this temperature is ________.

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Consider the following reaction at equilibrium. 2CO₂ (g) 2CO (g) + O₂ (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________.

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Exactly 3.5 moles if N₂O₄ is placed in an empty 2.0-L container and allowed to reach equilibrium described by the equation N₂O₄ (g)⇌ 2NO₂(g) If at equilibrium the N₂O₄ is 25% dissociated, what is the value of the equilibrium constant for the reaction?

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Consider the following reaction at equilibrium: 2CO₂ (g) 2CO (g) + O₂ (g) ΔH° = -514 kJ Le Châtelier's principle predicts that an increase in temperature will ________.

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

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

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The expression for K_p for the reaction below is ________. 4CuO (s) + CH₄ (g) CO₂ (g) + 4Cu (s) + 2H₂O (g)

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Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? 5N₂O4(g) 10NO₂ (g)

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