Question 1

The equilibrium constant, KP, has a value of 6.5 × 10-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g)  + Cl2(g)  P, has a value of 6.5 × 10-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g)  + Cl2(g)    2NOCl(g)  What is the value of Kc? (R = 0.08206 L • atm/K • mol)  A)  2.5 × 10-7 B)  6.5 × 10-4 C)  1.6 × 10-2 D)  1.7 E)  None of these choices is correct." class="answers-bank-image d-inline" rel="preload" > 2NOCl(g) 
What is the value of Kc? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)   2.5 × 10-7
B)   6.5 × 10-4
C)   1.6 × 10-2
D)   1.7
E)   None of these choices is correct.F) A) and B)
G) A) and C)

Question 2

When the substances in the equation below are at equilibrium, at pressure, P, and temperature, T, the equilibrium can be shifted to favor the products by CuO(s)  + H2(g)  2(g)    H2O(g)  + Cu(s)  ΔHºrxn = -2.0 kJ/mol A)  increasing the pressure by means of a moving piston at constant T. B)  increasing the pressure by adding an inert gas such as nitrogen. C)  decreasing the temperature. D)  allowing some gases to escape at constant P and T. E)  adding a more copper." class="answers-bank-image d-inline" rel="preload" > H2O(g)  + Cu(s)  ΔHºrxn = -2.0 kJ/mol

Accepted Answer

A)   increasing the pressure by means of a moving piston at constant T.
B)   increasing the pressure by adding an inert gas such as nitrogen.
C)   decreasing the temperature.
D)   allowing some gases to escape at constant P and T.
E)   adding a more copper.F) C) and D)
G) A) and B)

Question 3

A 6.0-L vessel was found to contain 1.0 mol BrCl3, 2.0 mol Br2 and 6.0 mol Cl2 at equilibrium. What is the equilibrium constant, Kc, for this equilibrium mixture for the reaction
2BrCl3(g)  3, 2.0 mol Br2 and 6.0 mol Cl2 at equilibrium. What is the equilibrium constant, Kc, for this equilibrium mixture for the reaction 2BrCl3(g)    Br2(g)  + 3Cl2(g) ? A)  0.014 B)  108 C)  18 D)  12 E)  432" class="answers-bank-image d-inline" rel="preload" > Br2(g)  + 3Cl2(g) ?

Accepted Answer

A)   0.014
B)   108
C)   18
D)   12
E)   432F) A) and C)
G) A) and D)

Question 4

Suppose 15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25°C, the flask is sealed, and the system is allowed to reach equilibrium. What is the partial pressure of ammonia in this flask if KP = 0.108 at 25°C for the following reaction? NH4HS(s)  P = 0.108 at 25°C for the following reaction? NH4HS(s)    NH3(g)  + H2S(g)  A)  0.657 atm B)  1.25 atm C)  0.329 atm D)  14.4 atm E)  2.50 atm" class="answers-bank-image d-inline" rel="preload" > NH3(g)  + H2S(g)

Accepted Answer

A)   0.657 atm
B)   1.25 atm
C)   0.329 atm
D)   14.4 atm
E)   2.50 atmF) A) and B)
G) A) and C)

Question 5

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. What is the equilibrium partial pressure of NO2? A)  0.152 atm B)  0.174 atm C)  0.200 atm D)  0.326 atm E)  0.500 atm" class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + O2(g)  reaches equilibrium is 0.674 atm. What is 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)   0.500 atmF) A) and D)
G) A) and B)

Question 6

Consider the equilibrium reaction: N2O4(g)  2O4(g)    2NO2(g)  Which of the following correctly describes the relationship between Kc and KP for the reaction? A)  KP = Kc B)  KP = RT × Kc C)  KP = (RT × Kc ) -1 D)  KP = Kc/RT E)  KP = RT/Kc" class="answers-bank-image d-inline" rel="preload" > 2NO2(g)  Which of the following correctly describes the relationship between Kc and KP for the reaction?

Accepted Answer

A)   KP = Kc
B)   KP = RT × Kc
C)   KP = (RT × Kc ) -1
D)   KP = Kc/RT
E)   KP = RT/KcF) B) and D)
G) B) and C) B

Question 7

Find the temperature at which KP = 42.0 for the reaction H2(g)  + I2(g)  P = 42.0 for the reaction H2(g)  + I2(g)    2HI(g) . [Given: at 25°C, for H2(g) , ΔH°f = 0, S° = 131.0 J/mol • K; for I2(g) , ΔH°f = 62.26 kJ/mol, S° = 260.6 J/mol • K; for HI(g) , ΔH°f = 25.9 kJ/mol, S° = 206.3 J/mol • K; assume that ΔH° and ΔS° are independent of temperature.] A)  1040 K B)  168 K C)  539 K D)  1400 K E)  34,200 K" class="answers-bank-image d-inline" rel="preload" > 2HI(g) . [Given: at 25°C, for H2(g) , ΔH°f = 0, S° = 131.0 J/mol • K; for I2(g) , ΔH°f = 62.26 kJ/mol, S° = 260.6 J/mol • K; for HI(g) , ΔH°f = 25.9 kJ/mol, S° = 206.3 J/mol • K; assume that ΔH° and ΔS° are independent of temperature.]

Accepted Answer

A)   1040 K
B)   168 K
C)   539 K
D)   1400 K
E)   34,200 KF) A) and C)
G) A) and D) A

Question 8

Suppose 75.0 g of PCl5(g)  is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl5(g)  5(g)  is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl5(g)    PCl3(g)  + Cl2(g)  If KP = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium? (R = 0.0821 atm • L/mol • K)  A)  2.88 atm B)  2.28 atm C)  4.54 atm D)  7.43 atm E)  9.69 atm" class="answers-bank-image d-inline" rel="preload" > PCl3(g)  + Cl2(g) 
If KP = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium? (R = 0.0821 atm • L/mol • K)

Accepted Answer

A)   2.88 atm
B)   2.28 atm
C)   4.54 atm
D)   7.43 atm
E)   9.69 atmF) A) and B)
G) A) and C)

Question 9

a. State Le Châtelier's principle.
b. The following reaction is at equilibrium in a closed container:
2Fe(OH)3(s)  Fe2O3(s) + 3H2O(g); ΔH°rxn > 0
What effects, if any, will the following actions have on the position of equilibrium? In each case, state the direction of any shift in equilibrium, and give your reasons in one sentence.
(i) adding more Fe(OH)3
(ii) raising the temperature
(iii) adding a more water vapor

Accepted Answer

a. If a stress is applied to a system at...

Question 10

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 is injected into a 2.00-L reaction vessel at 400ºC. What is the concentration of HI at equilibrium? A)  0.138 M B)  0.220 M C)  0.550 M D)  0.275 M E)  0.0275 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 is injected into a 2.00-L reaction vessel at 400ºC. What is the concentration of HI at equilibrium?

Accepted Answer

A)   0.138 M
B)   0.220 M
C)   0.550 M
D)   0.275 M
E)   0.0275 MF) A) and E)
G) A) and B)

Question 11

Which is the correct equilibrium constant expression for the following reaction? 2C6H6(g)  + 15O2(g)  6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > 12CO2(g)  + 6H2O(g)

Accepted Answer

A)   6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   6H6(g)  + 15O2(g)    12CO2(g)  + 6H2O(g)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) C) and E)
G) B) and D) B

Question 12

Iron(III)  oxide can be reduced by carbon monoxide. Fe2O3(s)  + 3CO(g)  2O3(s)  + 3CO(g)    2Fe(s)  + 3CO2(g)  Use the following thermodynamic data at 298 K to determine the equilibrium constant at this temperature. (R = 8.314 J/K • mol)    A)  7.0 × 10-6 B)  1.3 × 10-3 C)  2.2 × 104 D)  1.4 × 105 E)  > 2.0 × 105" class="answers-bank-image d-inline" rel="preload" > 2Fe(s)  + 3CO2(g) 
Use the following thermodynamic data at 298 K to determine the equilibrium constant at this temperature. (R = 8.314 J/K • mol)  2O3(s)  + 3CO(g)    2Fe(s)  + 3CO2(g)  Use the following thermodynamic data at 298 K to determine the equilibrium constant at this temperature. (R = 8.314 J/K • mol)    A)  7.0 × 10-6 B)  1.3 × 10-3 C)  2.2 × 104 D)  1.4 × 105 E)  > 2.0 × 105" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   7.0 × 10-6
B)   1.3 × 10-3
C)   2.2 × 104
D)   1.4 × 105
E)   > 2.0 × 105F) B) and E)
G) All of the above

Question 13

There are guidelines to help write equilibrium constants.

Accepted Answer

A) True 
 B)False

Question 14

In the gas phase, methyl isonitrile (CH3NC)  isomerizes to acetonitrile (CH3CN) , H3C-N≡C(g)  3NC)  isomerizes to acetonitrile (CH3CN) , H3C-N≡C(g)    H3C-C≡N(g)  With ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C. A)  1.68 × 10-10 B)  5.96 × 109 C)  2.16 × 1010 D)  4.63 × 10-11 E)  8.64 × 1012" class="answers-bank-image d-inline" rel="preload" > H3C-C≡N(g) 
With ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.

Accepted Answer

A)   1.68 × 10-10
B)   5.96 × 109
C)   2.16 × 1010
D)   4.63 × 10-11
E)   8.64 × 1012F) A) and E)
G) C) and D)

Question 15

Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C17H35COOH 17H35COOH   (C17H35COOH) 2; ΔH°rxn = -172 kJ/mol The equilibrium constant for this reaction at 28°C is 2.9 × 103. Estimate the equilibrium constant at 38°C. (R = 8.314 J/K• mol)  A)  4.7 × 105 B)  2.6 × 104 C)  1.9 × 103 D)  3.2 × 102 E)  18" class="answers-bank-image d-inline" rel="preload" > (C17H35COOH) 2; ΔH°rxn = -172 kJ/mol
The equilibrium constant for this reaction at 28°C is 2.9 × 103. Estimate the equilibrium constant at 38°C. (R = 8.314 J/K• mol)

Accepted Answer

A)   4.7 × 105
B)   2.6 × 104
C)   1.9 × 103
D)   3.2 × 102
E)   18F) C) and E)
G) A) and B)

Question 16

For the endothermic reaction A2(g)  2(g)    2A(g) , a snapshot of an equilibrium mixture of A(g)  and A2(g)  may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.)    What is the equilibrium constant Kc for this reaction at 298 K? (R = 0.08206 L • atm/K • mol)  A)  0.19 B)  0.67 C)  1.3 D)  2.7 E)  5.3" class="answers-bank-image d-inline" rel="preload" > 2A(g) , a snapshot of an equilibrium mixture of A(g)  and A2(g)  may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.)  2(g)    2A(g) , a snapshot of an equilibrium mixture of A(g)  and A2(g)  may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.)    What is the equilibrium constant Kc for this reaction at 298 K? (R = 0.08206 L • atm/K • mol)  A)  0.19 B)  0.67 C)  1.3 D)  2.7 E)  5.3" class="answers-bank-image d-inline" rel="preload" > What is the equilibrium constant Kc for this reaction at 298 K? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)   0.19
B)   0.67
C)   1.3
D)   2.7
E)   5.3F) A) and C)
G) B) and C)

Question 17

Solid ammonium hydrogen sulfide is introduced into a 2.00-L flask, and the flask is sealed. If this solid decomposes according to the equation NH4HS(s)  4HS(s)    NH3(g)  + H2S(g) , KP = 0.108 at 25°C, What is the minimum mass of ammonium hydrogen sulfide that must be present in the flask initially if equilibrium is to be established at 25°C? (R = 0.08206 L • atm/K • mol)  A)  0.917 g B)  1.37 g C)  2.74 g D)  0.581 g E)  0.452 g" class="answers-bank-image d-inline" rel="preload" > NH3(g)  + H2S(g) , KP = 0.108 at 25°C,
What is the minimum mass of ammonium hydrogen sulfide that must be present in the flask initially if equilibrium is to be established at 25°C? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)   0.917 g
B)   1.37 g
C)   2.74 g
D)   0.581 g
E)   0.452 gF) A) and B)
G) B) and D)

Question 18

What is the free energy change, ΔG°, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453°C? (R = 8.314 J/K• mol)  2HI(g)  2(g)  + I2(g) Kc = 0.020 at T = 453°C A)  6.4 kJ/mol B)  8.8 kJ/mol C)  15 kJ/mol D)  19 kJ/mol E)  24 kJ/mol" class="answers-bank-image d-inline" rel="preload" > H2(g)  + I2(g) Kc = 0.020 at T = 453°C

Accepted Answer

A)   6.4 kJ/mol
B)   8.8 kJ/mol
C)   15 kJ/mol
D)   19 kJ/mol
E)   24 kJ/molF) All of the above
G) D) and E)

Question 19

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the I2 concentration to increase? 2NOI(g)  2 concentration to increase? 2NOI(g)    2NO(g)  + I2(g) , ΔHºrxn = 45.3 kJ/mol A)  Add more NOI B)  Add more NO C)  Increase the pressure D)  Compress the gas mixture into a smaller volume E)  Decrease the temperature" class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + I2(g) , ΔHºrxn = 45.3 kJ/mol

Accepted Answer

A)   Add more NOI
B)   Add more NO
C)   Increase the pressure
D)   Compress the gas mixture into a smaller volume
E)   Decrease the temperatureF) D) and E)
G) None of the above

Question 20

When the following reaction is at equilibrium, which relationship is always true? 2NOCl(g)  2(g)  A)  [NO] [Cl2] = [NOCl] B)  [NO]2 [Cl2] = [NOCl]2 C)  [NOCl] = [NO] D)  2[NO] = [Cl2] E)  [NO]2 [Cl2] = Kc[NOCl]2" class="answers-bank-image d-inline" rel="preload" > 2NO(g)  + Cl2(g)

Accepted Answer

A)   [NO] [Cl2] = [NOCl]
B)   [NO]2 [Cl2] = [NOCl]2
C)   [NOCl] = [NO]
D)   2[NO] = [Cl2]
E)   [NO]2 [Cl2] = Kc[NOCl]2F) A) and E)
G) A) and B)

Exam 15: Chemical Equilibrium

The equilibrium constant, K_P, has a value of 6.5 × 10^-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl₂(g) 2NOCl(g) What is the value of K_c? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

When the substances in the equation below are at equilibrium, at pressure, P, and temperature, T, the equilibrium can be shifted to favor the products by CuO(s) + H₂(g) H₂O(g) + Cu(s) ΔHº_rxn = -2.0 kJ/mol

Correct Answer
verified

A 6.0-L vessel was found to contain 1.0 mol BrCl₃, 2.0 mol Br₂ and 6.0 mol Cl₂at equilibrium. What is the equilibrium constant, K_c, for this equilibrium mixture for the reaction 2BrCl₃(g) Br₂(g) + 3Cl₂(g) ?

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. What is the equilibrium partial pressure of NO₂?

Correct Answer
verified

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_P for the reaction?

Correct Answer
verified
B

Correct Answer
verified
A

Suppose 75.0 g of PCl₅(g) is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl₅(g) PCl₃(g) + Cl₂(g) If K_P = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium? (R = 0.0821 atm • L/mol • K)

Correct Answer
verified

Correct Answer
verified
a. If a stress is applied to a system at...
View Answer

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 is injected into a 2.00-L reaction vessel at 400ºC. What is the concentration of HI at equilibrium?

Correct Answer
verified

Which is the correct equilibrium constant expression for the following reaction? 2C₆H₆(g) + 15O₂(g) 12CO₂(g) + 6H₂O(g)

Correct Answer
verified
B

Iron(III) oxide can be reduced by carbon monoxide. Fe₂O₃(s) + 3CO(g) 2Fe(s) + 3CO₂(g) Use the following thermodynamic data at 298 K to determine the equilibrium constant at this temperature. (R = 8.314 J/K • mol)

Correct Answer
verified

There are guidelines to help write equilibrium constants.

Correct Answer
verified

In the gas phase, methyl isonitrile (CH₃NC) isomerizes to acetonitrile (CH₃CN) , H₃C-N≡C(g) H₃C-C≡N(g) With ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.

Correct Answer
verified

Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C₁₇H₃₅COOH (C₁₇H₃₅COOH) ₂; ΔH°_rxn = -172 kJ/mol The equilibrium constant for this reaction at 28°C is 2.9 × 10³. Estimate the equilibrium constant at 38°C. (R = 8.314 J/K• mol)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the free energy change, ΔG°, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453°C? (R = 8.314 J/K• mol) 2HI(g) H₂(g) + I₂(g) K_c = 0.020 at T = 453°C

Correct Answer
verified

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the I₂ concentration to increase? 2NOI(g) 2NO(g) + I₂(g) , ΔHº_rxn= 45.3 kJ/mol

Correct Answer
verified

When the following reaction is at equilibrium, which relationship is always true? 2NOCl(g) 2NO(g) + Cl₂(g)

Correct Answer
verified

Exam 15: Chemical Equilibrium

The equilibrium constant, KP, has a value of 6.5 × 10-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl2(g) 2NOCl(g) What is the value of Kc? (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

When the substances in the equation below are at equilibrium, at pressure, P, and temperature, T, the equilibrium can be shifted to favor the products by CuO(s) + H2(g) H2O(g) + Cu(s) ΔHºrxn = -2.0 kJ/mol

Correct AnswerverifiedShow Answer

A 6.0-L vessel was found to contain 1.0 mol BrCl3, 2.0 mol Br2 and 6.0 mol Cl2 at equilibrium. What is the equilibrium constant, Kc, for this equilibrium mixture for the reaction 2BrCl3(g) Br2(g) + 3Cl2(g) ?

Correct AnswerverifiedShow Answer

Suppose 15.00 g of solid ammonium hydrogen sulfide is introduced into a 500.-mL flask at 25°C, the flask is sealed, and the system is allowed to reach equilibrium. What is the partial pressure of ammonia in this flask if KP = 0.108 at 25°C for the following reaction? NH4HS(s) NH3(g) + H2S(g)

Correct AnswerverifiedShow Answer

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. What is the equilibrium partial pressure of NO2?

Correct AnswerverifiedShow Answer

Consider the equilibrium reaction: N2O4(g) 2NO2(g) Which of the following correctly describes the relationship between Kc and KP for the reaction?

Correct AnswerverifiedB

Correct AnswerverifiedA

Suppose 75.0 g of PCl5(g) is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl5(g) PCl3(g) + Cl2(g) If KP = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium? (R = 0.0821 atm • L/mol • K)

Correct AnswerverifiedShow Answer

Correct Answerverifieda. If a stress is applied to a system at...View AnswerShow 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 is injected into a 2.00-L reaction vessel at 400ºC. What is the concentration of HI at equilibrium?

Correct AnswerverifiedShow Answer

Which is the correct equilibrium constant expression for the following reaction? 2C6H6(g) + 15O2(g) 12CO2(g) + 6H2O(g)

Correct AnswerverifiedB

Iron(III) oxide can be reduced by carbon monoxide. Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g) Use the following thermodynamic data at 298 K to determine the equilibrium constant at this temperature. (R = 8.314 J/K • mol)

Correct AnswerverifiedShow Answer

There are guidelines to help write equilibrium constants.

Correct AnswerverifiedShow Answer

In the gas phase, methyl isonitrile (CH3NC) isomerizes to acetonitrile (CH3CN) , H3C-N≡C(g) H3C-C≡N(g) With ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.

Correct AnswerverifiedShow Answer

Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C17H35COOH (C17H35COOH) 2; ΔH°rxn = -172 kJ/mol The equilibrium constant for this reaction at 28°C is 2.9 × 103. Estimate the equilibrium constant at 38°C. (R = 8.314 J/K• mol)

Correct AnswerverifiedShow Answer

For the endothermic reaction A2(g) 2A(g) , a snapshot of an equilibrium mixture of A(g) and A2(g) may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) What is the equilibrium constant Kc for this reaction at 298 K? (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the free energy change, ΔG°, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453°C? (R = 8.314 J/K• mol) 2HI(g) H2(g) + I2(g) Kc = 0.020 at T = 453°C

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For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the I2 concentration to increase? 2NOI(g) 2NO(g) + I2(g) , ΔHºrxn = 45.3 kJ/mol

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When the following reaction is at equilibrium, which relationship is always true? 2NOCl(g) 2NO(g) + Cl2(g)

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The equilibrium constant, K_P, has a value of 6.5 × 10^-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl₂(g) 2NOCl(g) What is the value of K_c? (R = 0.08206 L • atm/K • mol)

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When the substances in the equation below are at equilibrium, at pressure, P, and temperature, T, the equilibrium can be shifted to favor the products by CuO(s) + H₂(g) H₂O(g) + Cu(s) ΔHº_rxn = -2.0 kJ/mol

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A 6.0-L vessel was found to contain 1.0 mol BrCl₃, 2.0 mol Br₂ and 6.0 mol Cl₂at equilibrium. What is the equilibrium constant, K_c, for this equilibrium mixture for the reaction 2BrCl₃(g) Br₂(g) + 3Cl₂(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. What is the equilibrium partial pressure of NO₂?

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Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_P for the reaction?

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B

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A

Suppose 75.0 g of PCl₅(g) is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl₅(g) PCl₃(g) + Cl₂(g) If K_P = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium? (R = 0.0821 atm • L/mol • K)

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a. If a stress is applied to a system at...
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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 is injected into a 2.00-L reaction vessel at 400ºC. What is the concentration of HI at equilibrium?

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Which is the correct equilibrium constant expression for the following reaction? 2C₆H₆(g) + 15O₂(g) 12CO₂(g) + 6H₂O(g)

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B

Iron(III) oxide can be reduced by carbon monoxide. Fe₂O₃(s) + 3CO(g) 2Fe(s) + 3CO₂(g) Use the following thermodynamic data at 298 K to determine the equilibrium constant at this temperature. (R = 8.314 J/K • mol)

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In the gas phase, methyl isonitrile (CH₃NC) isomerizes to acetonitrile (CH₃CN) , H₃C-N≡C(g) H₃C-C≡N(g) With ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.

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Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C₁₇H₃₅COOH (C₁₇H₃₅COOH) ₂; ΔH°_rxn = -172 kJ/mol The equilibrium constant for this reaction at 28°C is 2.9 × 10³. Estimate the equilibrium constant at 38°C. (R = 8.314 J/K• mol)

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What is the free energy change, ΔG°, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453°C? (R = 8.314 J/K• mol) 2HI(g) H₂(g) + I₂(g) K_c = 0.020 at T = 453°C

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For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the I₂ concentration to increase? 2NOI(g) 2NO(g) + I₂(g) , ΔHº_rxn= 45.3 kJ/mol

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When the following reaction is at equilibrium, which relationship is always true? 2NOCl(g) 2NO(g) + Cl₂(g)

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