Question 1

A 2.5 L flask is filled with 0.25 atm SO3,0.20 atm SO2,and 0.40 atm O2,and allowed to reach equilibrium.Assume the temperature of the mixture is chosen so that Kp = 0.12.Predict the effect on the partial pressure of SO3 as equilibrium is achieved by using Q,the reaction quotient. 2 
SO3(g)  ⇌ 2 SO2(g) + O2(g)

Accepted Answer

A)   The partial pressure of SO3 will decrease because Q > K.
B)   The partial pressure of SO3 will decrease because Q 
C)   The partial pressure of SO3 will increase because Q 
D)   The partial pressure of SO3 will increase because Q > K.
E)   The partial pressure of SO3 will remain the same because Q = K.

Question 2

If the value of Q is less than Kp,then

Accepted Answer

A)   the system is in equilibrium.
B)   a catalyst is necessary to achieve equilibrium.
C)   the reaction will go left or right depending upon the reaction stoichiometry.
D)   the reaction will proceed to the right until equilibrium is established.
E)   the reaction will proceed to the left until equilibrium is established.

Question 3

Use the equilibrium constants for the following reactions at 700°C  2SO2(g) +O2(g) ⇌2SO3(g) 2NO(g) +O2(g) ⇌2NO2(g) K1=4.8K2=16\begin{array}{l}\begin{array}{lll}2 \mathrm{SO}_{2}(g) +\mathrm{O}_{2}(g)  ightleftharpoons 2 \mathrm{SO}_{3}(g) \2 \mathrm{NO}(g) +\mathrm{O}_{2}(g)  ightleftharpoons 2 \mathrm{NO}_{2}(g) \\end{array}\begin{array}{lll}K_{1}=4.8 \K_{2}=16\end{array}\end{array}2SO2​(g) +O2​(g) ⇌2SO3​(g) 2NO(g) +O2​(g) ⇌2NO2​(g) ​K1​=4.8K2​=16​​

To determine the equilibrium constant for the following reaction.
SO3(g) + NO(g)  ⇌ SO2(g) + NO2(g)

Accepted Answer

A)   0.30
B)   0.55
C)   0.85
D)   1.8
E)   3.3

Question 4

At a given temperature,the equilibrium constant (Kp) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.172.If 0.224 atm N2O4 is sealed in a flask,what partial pressure of NO2 will exist at equilibrium? 
N2O4(g)  ⇌ 2NO2(g)

Accepted Answer

A)   0.0385 atm
B)   0.158 atm
C)   0.196 atm
D)   0.257 atm
E)   0.379 atm

Question 5

Which of the following reactions is a heterogeneous equilibrium expression?

Accepted Answer

A)   2NO(g) + O2(g)  ⇌ 2NO2(g) 
B)   2NH3(g)  ⇌ N2(g) + 3H2(g) 
C)   2H2(g) + O2(g)  ⇌ 2H2O(g) 
D)   2S(s) + 3O2(g)  ⇌ 2SO3(g) 
E)   C2H4(g) + H2(g)  ⇌ C2H6(g)

Question 6

The value of the equilibrium constant for the following reaction is 
345. A + 2B ⇌ 3C + D
What is the value of the equilibrium constant for the reaction below?
2A + 4B ⇌ 6C + 2D

Accepted Answer

A)   K = 345
B)   K = (345) 2 = 1.19 × 105
C)   K = (345) 1/2 = 18.6
D)   K = (2 × 345) 2 = 4.76 × 105
E)   K = 2 × (345) 2 = 2.38 × 105

Question 7

Nitrogen can react with oxygen to form nitrogen monoxide.  N2( g) +O2( g) ⇌2NO(g) \mathrm{N}_{2}(\mathrm{~g}) +\mathrm{O}_{2}(\mathrm{~g})  ightleftharpoons 2 \mathrm{NO}(\mathrm{g}) N2​( g) +O2​( g) ⇌2NO(g)     \quad \quad \quad    K=1.0×1030 at 25∘CK=1.0 	imes 10^{30} 	ext { at } 25^{\circ} \mathrm{C}K=1.0×1030 at 25∘C 
When equilibrium is established,the partial pressures of nitrogen and oxygen are 1.2 atm and 3.1 atm,respectively.What is the equilibrium pressure of nitrogen monoxide?

Accepted Answer

A)   3.7 × 10−30 atm
B)   1.9 × 10−15 atm
C)   2.7 × 10−13 atm
D)   1.9 × 10−10 atm
E)   3.7 × 10−7 atm

Question 8

Use the equilibrium constants for the following reactions 
 2NO(g) ⇌N2(g) +O2(g) K1=2.4×10302NO(g) +O2(g) ⇌2NO2(g) K2=2.4×1012\begin{array}{ll}2 \mathrm{NO}(g)  ightleftharpoons \mathrm{N}_{2}(g) +\mathrm{O}_{2}(g)  & K_{1}=2.4 	imes 10^{30} \2 \mathrm{NO}(g) +\mathrm{O}_{2}(g)  ightleftharpoons 2 \mathrm{NO}_{2}(g)  & K_{2}=2.4 	imes 10^{12}\end{array}2NO(g) ⇌N2​(g) +O2​(g) 2NO(g) +O2​(g) ⇌2NO2​(g) ​K1​=2.4×1030K2​=2.4×1012​ 
To determine the equilibrium constant for the reaction below.
N2(g) + 2O2(g)  ⇌ 2NO2(g)

Accepted Answer

A)   1.7 × 10−43
B)   1.0 × 10−18
C)   5.8 × 1018
D)   2.4 × 1030
E)   5.8 × 1042

Question 9

For which of the following reactions does Kc equal Kp?

Accepted Answer

A)   Sn(s) + 2H2O(g)  ⇌ SnO2(s) + 2H2(g) 
B)   2C2H6(g) + 7O2(g)  ⇌ 4CO2(g) + 6H2O(g) 
C)   NH4Cl(s)  ⇌ NH3(g) + HCl(g) 
D)   N2(g) + 3H2(g)  ⇌ 2NH3(g) 
E)   CaCO3(s)  ⇌ CaO(s) + CO2(g)

Exam 12: Gaseous Chemical Equilibrium

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At a given temperature,the equilibrium constant (K_p) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.172.If 0.224 atm N₂O₄ is sealed in a flask,what partial pressure of NO₂ will exist at equilibrium? N₂O₄(g) ⇌ 2NO₂(g)

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Correct Answer
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The value of the equilibrium constant for the following reaction is 345. A + 2B ⇌ 3C + D What is the value of the equilibrium constant for the reaction below? 2A + 4B ⇌ 6C + 2D

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Correct Answer
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Which of the following reactions is a heterogeneous equilibrium expression?

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For which of the following reactions does K_c equal K_p?

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If the value of Q is less than K_p,then

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Exam 12: Gaseous Chemical Equilibrium

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Correct AnswerverifiedShow Answer

At a given temperature,the equilibrium constant (Kp) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.172.If 0.224 atm N2O4 is sealed in a flask,what partial pressure of NO2 will exist at equilibrium? N2O4(g) ⇌ 2NO2(g)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The value of the equilibrium constant for the following reaction is 345. A + 2B ⇌ 3C + D What is the value of the equilibrium constant for the reaction below? 2A + 4B ⇌ 6C + 2D

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which of the following reactions is a heterogeneous equilibrium expression?

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For which of the following reactions does Kc equal Kp?

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If the value of Q is less than Kp,then

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Correct Answer
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Correct Answer
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At a given temperature,the equilibrium constant (K_p) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.172.If 0.224 atm N₂O₄ is sealed in a flask,what partial pressure of NO₂ will exist at equilibrium? N₂O₄(g) ⇌ 2NO₂(g)

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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For which of the following reactions does K_c equal K_p?

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If the value of Q is less than K_p,then

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