Question 1

Consider the reaction PCl5(g)  5(g)    PCl3(g) + Cl2(g)  At a certain temperature,if the initial concentration of PCl5(g) is 3.0 M,at equilibrium the concentration of Cl2(g) is 0.80 M.Calculate the value of Kc at this temperature. A) 0.21 B) 0.29 C) 0.64 D) 3.4 E) 0.46" class="answers-bank-image d-inline" rel="preload" > PCl3(g) + Cl2(g) 
At a certain temperature,if the initial concentration of PCl5(g) is 3.0 M,at equilibrium the concentration of Cl2(g) is 0.80 M.Calculate the value of Kc at this temperature.

Accepted Answer

A)  0.21
B)  0.29
C)  0.64
D)  3.4
E)  0.46F) A) and C)
G) D) and E)

Question 2

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47  106 at 298 K.Calculate the temperature at which K = 0.0100.For this reaction,H = 92.38 kJmol1.

Accepted Answer

A)  241 K
B)  332 K
C)  59 K
D)  390 K
E)  117 KF) C) and D)
G) A) and C)

Question 3

At 600C,the equilibrium constant for the reaction 2HgO(s)  C,the equilibrium constant for the reaction 2HgO(s)    2Hg(l) + O2(g)  Is 2.8.Calculate the equilibrium constant for the reaction   1/2O2(g) + Hg(l)    HgO(s)  A) (1.7)  B) 1.1 C) 0.60 D) 0.36 E) 1.7" class="answers-bank-image d-inline" rel="preload" > 2Hg(l) + O2(g) 
Is 2.8.Calculate the equilibrium constant for the reaction C,the equilibrium constant for the reaction 2HgO(s)    2Hg(l) + O2(g)  Is 2.8.Calculate the equilibrium constant for the reaction   1/2O2(g) + Hg(l)    HgO(s)  A) (1.7)  B) 1.1 C) 0.60 D) 0.36 E) 1.7" class="answers-bank-image d-inline" rel="preload" > 1/2O2(g) + Hg(l)  C,the equilibrium constant for the reaction 2HgO(s)    2Hg(l) + O2(g)  Is 2.8.Calculate the equilibrium constant for the reaction   1/2O2(g) + Hg(l)    HgO(s)  A) (1.7)  B) 1.1 C) 0.60 D) 0.36 E) 1.7" class="answers-bank-image d-inline" rel="preload" > HgO(s)

Accepted Answer

A)  (1.7) 
B)  1.1
C)  0.60
D)  0.36
E)  1.7F) A) and D)
G) C) and E)

Question 4

The equilibrium constant,K,for the reaction 2HgO(s)  2(g)  Is 1.2  1030.Calculate K for the reaction 1/2O2(g) + Hg(l)    HgO(s) . A) (1.1  1015 )  B) 8.3  1029  C) 4.2  1029  D) 9.1  1014  E) 1.1  1015 " class="answers-bank-image d-inline" rel="preload" > 2Hg(l) + O2(g) 
Is 1.2  1030.Calculate K for the reaction
1/2O2(g) + Hg(l)  2(g)  Is 1.2  1030.Calculate K for the reaction 1/2O2(g) + Hg(l)    HgO(s) . A) (1.1  1015 )  B) 8.3  1029  C) 4.2  1029  D) 9.1  1014  E) 1.1  1015 " class="answers-bank-image d-inline" rel="preload" > HgO(s) .

Accepted Answer

A)  (1.1  1015 ) 
B)  8.3  1029 
C)  4.2  1029 
D)  9.1  1014 
E)  1.1  1015 F) B) and C)
G) A) and D)

Question 5

From a plot of Gibbs free energy versus progress of reaction,the sign of F1F1F1S1F1F1F10Gr at any point along the curve is given by the slope of the curve.True or false?

Accepted Answer

A) True 
 B)False

Question 6

For a pure solid or liquid,the molar free energy always has its standard value.True or false?

Accepted Answer

A) True 
 B)False

Question 7

Given: C(s) + CO2(g)  2(g)    2CO(g)  At equilibrium at a certain temperature,the partial pressures of CO(g) and CO2(g) are 1.44 atm and 0.820 atm,respectively.Calculate the value of K for this reaction. A) 2.53 B) 10.1 C) 1.76 D) 3.08 E) 3.51" class="answers-bank-image d-inline" rel="preload" > 2CO(g)  At equilibrium at a certain temperature,the partial pressures of CO(g) and CO2(g) are 1.44 atm and 0.820 atm,respectively.Calculate the value of K for this reaction.

Accepted Answer

A)  2.53
B)  10.1
C)  1.76
D)  3.08
E)  3.51F) B) and E)
G) B) and D)

Question 8

Write the equilibrium constant for 2NaBr(aq) + Pb(ClO4) 2(aq)  4) 2(aq)    PbBr2(s) + 2NaClO4(aq) . A) K = [Pb2+][Br]2  B) K = 1/([Pb2+][Br]2)  C) K = [NaClO4]2/([NaBr]2[Pb(ClO4) 2] D) K = [PbBr2]/([Pb2+][Br]2)  E) K = 1/([Pb(ClO4) 2][NaBr]2) " class="answers-bank-image d-inline" rel="preload" > PbBr2(s) + 2NaClO4(aq) .

Accepted Answer

A)  K = [Pb2+][Br]2 
B)  K = 1/([Pb2+][Br]2) 
C)  K = [NaClO4]2/([NaBr]2[Pb(ClO4) 2]
D)  K = [PbBr2]/([Pb2+][Br]2) 
E)  K = 1/([Pb(ClO4) 2][NaBr]2) F) A) and C)
G) B) and E)

Question 9

For any reaction at equilibrium,F1F1F1S1F1F1F10G < 0.True or false?

Accepted Answer

A) True 
 B)False

Question 10

If a reaction mixture that is not at equilibrium contains more products than reactants,F1F1F1S1F1F1F10G > 0 for the forward reaction.True or false?

Accepted Answer

A) True 
 B)False

Question 11

At 600C,Kc = 2.8 for the reaction 2HgO(s)  C,Kc = 2.8 for the reaction 2HgO(s)    2Hg(l) + O2(g)  Calculate K at 600C for this reaction. A) 6800 B) 200 C) 1.4  104  D) 2.8 E) 138" class="answers-bank-image d-inline" rel="preload" > 2Hg(l) + O2(g) 
Calculate K at 600C for this reaction.

Accepted Answer

A)  6800
B)  200
C)  1.4  104 
D)  2.8
E)  138F) B) and D)
G) A) and E)

Question 12

Consider the reaction 4NH3(g) + 3O2(g)  3(g) + 3O2(g)    2N2(g) + 6H2O(g) ,K = 1080 at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is A) 6 M. B) 0 M. C) 3 M. D) 12 M. E) 18 M." class="answers-bank-image d-inline" rel="preload" > 2N2(g) + 6H2O(g) ,K = 1080 at a certain temperature.
Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

Accepted Answer

A)  6 M.
B)  0 M.
C)  3 M.
D)  12 M.
E)  18 M.F) A) and D)
G) A) and B)

Question 13

Consider the reaction Ni(s) + 4CO(g)  4(g)  At 30C and PCO = 1 atm,Ni reacts with CO(g) to form Ni(CO) 4(g) .At 200C,Ni(CO) 4(g) decomposes to Ni(s) and CO(g) .This means A) adding an inert gas like argon favors the forward reaction. B) the activation energy for the forward reaction is greater than for the reverse reaction. C) the forward reaction is endothermic. D) K at 30C is greater than K at 200C. E) a decrease in pressure favors the forward reaction." class="answers-bank-image d-inline" rel="preload" > Ni(CO) 4(g) 
At 30C and PCO = 1 atm,Ni reacts with CO(g) to form Ni(CO) 4(g) .At 200C,Ni(CO) 4(g) decomposes to Ni(s) and CO(g) .This means

Accepted Answer

A)  adding an inert gas like argon favors the forward reaction.
B)  the activation energy for the forward reaction is greater than for the reverse reaction.
C)  the forward reaction is endothermic.
D)  K at 30C is greater than K at 200C.
E)  a decrease in pressure favors the forward reaction.F) All of the above
G) D) and E)

Question 14

For the reaction NH3(g) + H2S(g)  3(g) + H2S(g)    NH4HS(s)  Kc = 9.7 at 900 K.If the initial concentrations of NH3(g) and H2S(g) are 2.0 M,what is the equilibrium concentration of NH3(g) ? A) 1.9 M B) 1.7 M C) 0.20 M D) 0.10 M E) 0.32 M" class="answers-bank-image d-inline" rel="preload" > NH4HS(s) 
Kc = 9.7 at 900 K.If the initial concentrations of NH3(g) and H2S(g) are 2.0 M,what is the equilibrium concentration of NH3(g) ?

Accepted Answer

A)  1.9 M
B)  1.7 M
C)  0.20 M
D)  0.10 M
E)  0.32 MF) C) and D)
G) A) and D)

Question 15

Given: 2SO2(g) + O2(g)  2(g) + O2(g)    2SO3(g)  At equilibrium at a certain temperature,the concentrations of SO3(g) ,SO2(g) ,and O2(g) are 0.12 M,0.86 M,and 0.33 M,respectively.Calculate the value of Kc for this reaction. A) 1.31 B) 0.42 C) 0.014 D) 0.059 E) 0.87" class="answers-bank-image d-inline" rel="preload" > 2SO3(g)  At equilibrium at a certain temperature,the concentrations of SO3(g) ,SO2(g) ,and O2(g) are 0.12 M,0.86 M,and 0.33 M,respectively.Calculate the value of Kc for this reaction.

Accepted Answer

A)  1.31
B)  0.42
C)  0.014
D)  0.059
E)  0.87F) A) and E)
G) B) and C)

Question 16

Calculate G at 298 K for the reaction C2H5OH(l)  C2H5OH(g,0.0400 bar) 
Given G = 6.2 kJ at 298 K.

Accepted Answer

A)  14 kJ
B)  2.7 kJ
C)  (14 kJ) 
D)  (1.8 kJ) 
E)  1.8 kJF) A) and B)
G) A) and E)

Question 17

Consider the following
N2O4(g)  2NO2(g)
The equilibrium constant for this reaction will decrease with an increase in temperature.True or false?

Accepted Answer

A) True 
 B)False

Question 18

At the normal boiling point of chlorine,238.5 K,ΔH of vaporization is 20.4 kJF1F1F1S1F1F1F10molF1F1F1S1F1F1F101.For the reversible vaporization of 1 mol of chlorine at 238.5 K and a constant pressure of 1 atm,determine q,ΔS,and ΔG.

Accepted Answer

20.4 kJ<font face="symbol">F1F1...

Question 19

For the reaction 2NOCl(g)  2NO(g)+ Cl2(g),if,initially,[NOCl(g)] = 2.8 M,at equilibrium [NO(g)] = 1.2 M.Calculate the equilibrium concentration of NOCl(g).

Accepted Answer

Question 20

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47  106 at 298 K.Calculate the temperature at which K = 1.00.For this reaction,H = 92.38 kJmol1.

Accepted Answer

A)  193 K
B)  353 K
C)  466 K
D)  492 K
E)  219 KF) A) and B)
G) A) and C)

Exam 11: Chemical Equilibria

Given: 2SO2(g) + O2(g) 2SO3(g) At equilibrium at a certain temperature,the concentrations of SO3(g) ,SO2(g) ,and O2(g) are 0.12 M,0.86 M,and 0.33 M,respectively.Calculate the value of Kc for this reaction.

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Consider the reaction PCl5(g) PCl3(g) + Cl2(g) At a certain temperature,if the initial concentration of PCl5(g) is 3.0 M,at equilibrium the concentration of Cl2(g) is 0.80 M.Calculate the value of Kc at this temperature.

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For the reaction NH3(g) + H2S(g) NH4HS(s) Kc = 9.7 at 900 K.If the initial concentrations of NH3(g) and H2S(g) are 2.0 M,what is the equilibrium concentration of NH3(g) ?

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Write the equilibrium constant for 2NaBr(aq) + Pb(ClO4) 2(aq) PbBr2(s) + 2NaClO4(aq) .

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Consider the reaction 4NH3(g) + 3O2(g) 2N2(g) + 6H2O(g) ,K = 1080 at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

Correct AnswerverifiedShow Answer

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47  106 at 298 K.Calculate the temperature at which K = 0.0100.For this reaction,H = 92.38 kJmol1.

Correct AnswerverifiedShow Answer

Consider the following N2O4(g) 2NO2(g) The equilibrium constant for this reaction will decrease with an increase in temperature.True or false?

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Consider the reaction Ni(s) + 4CO(g) Ni(CO) 4(g) At 30C and PCO = 1 atm,Ni reacts with CO(g) to form Ni(CO) 4(g) .At 200C,Ni(CO) 4(g) decomposes to Ni(s) and CO(g) .This means

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At 600C,the equilibrium constant for the reaction 2HgO(s) 2Hg(l) + O2(g) Is 2.8.Calculate the equilibrium constant for the reaction 1/2O2(g) + Hg(l) HgO(s)

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If a reaction mixture that is not at equilibrium contains more products than reactants,G > 0 for the forward reaction.True or false?

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At 600C,Kc = 2.8 for the reaction 2HgO(s) 2Hg(l) + O2(g) Calculate K at 600C for this reaction.

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For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47  106 at 298 K.Calculate the temperature at which K = 1.00.For this reaction,H = 92.38 kJmol1.

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For any reaction at equilibrium,G < 0.True or false?

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The equilibrium constant,K,for the reaction 2HgO(s) 2Hg(l) + O2(g) Is 1.2  1030.Calculate K for the reaction 1/2O2(g) + Hg(l) HgO(s) .

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For a pure solid or liquid,the molar free energy always has its standard value.True or false?

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Calculate G at 298 K for the reaction C2H5OH(l)  C2H5OH(g,0.0400 bar) Given G = 6.2 kJ at 298 K.

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At the normal boiling point of chlorine,238.5 K,ΔH of vaporization is 20.4 kJmol1.For the reversible vaporization of 1 mol of chlorine at 238.5 K and a constant pressure of 1 atm,determine q,ΔS,and ΔG.

Correct Answerverified20.4 kJF1F1...View AnswerShow Answer

For the reaction 2NOCl(g) 2NO(g)+ Cl2(g),if,initially,[NOCl(g)] = 2.8 M,at equilibrium [NO(g)] = 1.2 M.Calculate the equilibrium concentration of NOCl(g).

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From a plot of Gibbs free energy versus progress of reaction,the sign of Gr at any point along the curve is given by the slope of the curve.True or false?

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Given: C(s) + CO2(g) 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g) and CO2(g) are 1.44 atm and 0.820 atm,respectively.Calculate the value of K for this reaction.

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Given: 2SO₂(g) + O₂(g) 2SO₃(g) At equilibrium at a certain temperature,the concentrations of SO₃(g) ,SO₂(g) ,and O₂(g) are 0.12 M,0.86 M,and 0.33 M,respectively.Calculate the value of K_c for this reaction.

Correct Answer
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Consider the reaction PCl₅(g) PCl₃(g) + Cl₂(g) At a certain temperature,if the initial concentration of PCl₅(g) is 3.0 M,at equilibrium the concentration of Cl₂(g) is 0.80 M.Calculate the value of K_c at this temperature.

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For the reaction NH₃(g) + H₂S(g) NH₄HS(s) K_c = 9.7 at 900 K.If the initial concentrations of NH₃(g) and H₂S(g) are 2.0 M,what is the equilibrium concentration of NH₃(g) ?

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Write the equilibrium constant for 2NaBr(aq) + Pb(ClO₄) ₂(aq) PbBr₂(s) + 2NaClO₄(aq) .

Correct Answer
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Consider the reaction 4NH₃(g) + 3O₂(g) 2N₂(g) + 6H₂O(g) ,K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

Correct Answer
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For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47  10^⁶ at 298 K.Calculate the temperature at which K = 0.0100.For this reaction,H = 92.38 kJmol^¹.

Correct Answer
verified

Consider the following N₂O₄(g) 2NO₂(g) The equilibrium constant for this reaction will decrease with an increase in temperature.True or false?

Correct Answer
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Consider the reaction Ni(s) + 4CO(g) Ni(CO) ₄(g) At 30C and P_CO = 1 atm,Ni reacts with CO(g) to form Ni(CO) ₄(g) .At 200C,Ni(CO) ₄(g) decomposes to Ni(s) and CO(g) .This means

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At 600C,the equilibrium constant for the reaction 2HgO(s) 2Hg(l) + O₂(g) Is 2.8.Calculate the equilibrium constant for the reaction 1/2O₂(g) + Hg(l) HgO(s)

Correct Answer
verified

Correct Answer
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At 600C,K_c = 2.8 for the reaction 2HgO(s) 2Hg(l) + O₂(g) Calculate K at 600C for this reaction.

Correct Answer
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For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47  10^⁶ at 298 K.Calculate the temperature at which K = 1.00.For this reaction,H = 92.38 kJmol^¹.

Correct Answer
verified

Correct Answer
verified

The equilibrium constant,K,for the reaction 2HgO(s) 2Hg(l) + O₂(g) Is 1.2  10^³⁰.Calculate K for the reaction 1/2O₂(g) + Hg(l) HgO(s) .

Correct Answer
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Correct Answer
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Calculate G at 298 K for the reaction C₂H₅OH(l)  C₂H₅OH(g,0.0400 bar) Given G = 6.2 kJ at 298 K.

Correct Answer
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At the normal boiling point of chlorine,238.5 K,ΔH of vaporization is 20.4 kJmol^¹.For the reversible vaporization of 1 mol of chlorine at 238.5 K and a constant pressure of 1 atm,determine q,ΔS,and ΔG.

Correct Answer
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20.4 kJF1F1...
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For the reaction 2NOCl(g) 2NO(g)+ Cl₂(g),if,initially,[NOCl(g)] = 2.8 M,at equilibrium [NO(g)] = 1.2 M.Calculate the equilibrium concentration of NOCl(g).

Correct Answer
verified

From a plot of Gibbs free energy versus progress of reaction,the sign of G_r at any point along the curve is given by the slope of the curve.True or false?

Correct Answer
verified

Given: C(s) + CO₂(g) 2CO(g) At equilibrium at a certain temperature,the partial pressures of CO(g) and CO₂(g) are 1.44 atm and 0.820 atm,respectively.Calculate the value of K for this reaction.

Correct Answer
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