Question 1

When the reaction 2H2S(g)  2S(g)    2H2(g) + S2(g) is carried out at 1065°C,KP = 0.012.Starting with pure H2S at 1065°C,what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(g) ? A) 1.06 atm B) 1.86 atm C) 0.94 atm D) 0.90 atm E) 1.52 atm" class="answers-bank-image d-inline" rel="preload" > 2H2(g) + S2(g) is carried out at 1065°C,KP = 0.012.Starting with pure H2S at 1065°C,what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(g) ?

Accepted Answer

A)  1.06 atm
B)  1.86 atm
C)  0.94 atm
D)  0.90 atm
E)  1.52 atmF) All of the above
G) B) and D)

Question 2

Suppose 50.0 g of N2O4 is introduced into an evacuated 2.00-L vessel and allowed to come to equilibrium with its decomposition product,N2O4(g)  2O4 is introduced into an evacuated 2.00-L vessel and allowed to come to equilibrium with its decomposition product,N2O4(g)    2NO2(g) .For this reaction Kc = 0.133.Once the system has reached equilibrium,5.00 g of NO2 is injected into the vessel,and the system is allowed to equilibrate once again.What is the mass of N2O4 in the final equilibrium mixture? A) 39.5 g B) 35.3 g C) 30.3 g D) 25.2 g E) 43.7 g" class="answers-bank-image d-inline" rel="preload" > 2NO2(g) .For this reaction Kc = 0.133.Once the system has reached equilibrium,5.00 g of NO2 is injected into the vessel,and the system is allowed to equilibrate once again.What is the mass of N2O4 in the final equilibrium mixture?

Accepted Answer

A)  39.5 g
B)  35.3 g
C)  30.3 g
D)  25.2 g
E)  43.7 gF) B) and D)
G) B) and C)

Question 3

A temperature increase favors an endothermic reaction.

Accepted Answer

A) True 
 B)False

Question 4

The solubility product constant,Ksp,at 25°C for AgI(s) in water has the value 8.3 × 10-17. Calculate ΔG at 25°C for the process AgI(s)  sp,at 25°C for AgI(s) in water has the value 8.3 × 10-17. Calculate ΔG at 25°C for the process AgI(s)    Ag+(aq) + I-(aq) where [Ag+] = 9.1 × 10-9 M and [I-] = 9.1 × 10-9 M.(R = 8.314 J/K • mol)  A) +4.4 kJ/mol B) +91.7 kJ/mol C) 0.0 kJ/mol D) -91.7 kJ/mol E) -4.4 kJ/mol" class="answers-bank-image d-inline" rel="preload" > Ag+(aq) + I-(aq) where [Ag+] = 9.1 × 10-9
M and [I-] = 9.1 × 10-9 M.(R = 8.314 J/K • mol)

Accepted Answer

A)  +4.4 kJ/mol
B)  +91.7 kJ/mol
C)  0.0 kJ/mol
D)  -91.7 kJ/mol
E)  -4.4 kJ/molF) B) and D)
G) A) and B)

Question 5

Which is the correct equilibrium constant expression for the following reaction? FeO(s) + H2(g)  2(g)    Fe(s) + H2O(g)  A) Kc = [H2O]/[H2] B) Kc = [Fe] [H2O]/[Fe2O3] C) Kc = [Fe2O3] [H2]/[Fe][H2O] D) Kc = [Fe][H2O]/[Fe2O3] [H2] E) Kc = [H2]/[H2O]" class="answers-bank-image d-inline" rel="preload" > Fe(s) + H2O(g)

Accepted Answer

A)  Kc = [H2O]/[H2]
B)  Kc = [Fe] [H2O]/[Fe2O3]
C)  Kc = [Fe2O3] [H2]/[Fe][H2O]
D)  Kc = [Fe][H2O]/[Fe2O3] [H2]
E)  Kc = [H2]/[H2O]F) A) and B)
G) A) and C)

Question 6

What is defined as a fraction with equilibrium product concentrations in the numerator and equilibrium reactant concentrations in the denominator and each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?

Accepted Answer

A)  Reversibility expression
B)  Reaction expression
C)  Equilibrium expression
D)  Product quotient
E)  Mass actionF) None of the above
G) B) and C)

Question 7

Suppose 75.0 g of PCl5(g) is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g) ,and the system is allowed to reach equilibrium at 250ºC. PCl5(g)  5(g) is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g) ,and the system is 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 = 0.08206 L • atm/K • mol)  A) 6.83 atm B) 8.86 atm C) 5.38 atm D) 3.47 atm E) 1.68 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 = 0.08206 L • atm/K • mol)

Accepted Answer

A)  6.83 atm
B)  8.86 atm
C)  5.38 atm
D)  3.47 atm
E)  1.68 atmF) A) and D)
G) B) and E)

Question 8

Consider the reaction N2(g)+ 3H2(g)  2NH3(g).If nitrogen is added to the system at equilibrium,what will happen to the ammonia concentration?

Accepted Answer

The ammoni...

Question 9

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) None of the above
G) C) and D)

Question 10

At 450°C,tert-butyl alcohol decomposes into water and isobutene. (CH3) 3COH(g)  3) 3COH(g)    (CH3) 2CCH2(g) + H2O(g)  A reaction vessel contains these compounds at equilibrium.What will happen if the volume of the container is reduced by 50% at constant temperature? A) The forward reaction will proceed in order to reestablish equilibrium. B) The reverse reaction will proceed in order to reestablish equilibrium. C) No change occurs. D) The equilibrium constant will increase. E) The equilibrium constant will decrease." class="answers-bank-image d-inline" rel="preload" > (CH3) 2CCH2(g) + H2O(g) 
A reaction vessel contains these compounds at equilibrium.What will happen if the volume of the container is reduced by 50% at constant temperature?

Accepted Answer

A)  The forward reaction will proceed in order to reestablish equilibrium.
B)  The reverse reaction will proceed in order to reestablish equilibrium.
C)  No change occurs.
D)  The equilibrium constant will increase.
E)  The equilibrium constant will decrease.F) All of the above
G) B) and C)

Question 11

For the equilibrium A2(g)  2(g)    2A(g) ,if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Qc and time as equilibrium is established? A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > 2A(g) ,if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Qc and time as equilibrium is established?

Accepted Answer

A)   2(g)    2A(g) ,if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Qc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2(g)    2A(g) ,if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Qc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2(g)    2A(g) ,if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Qc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2(g)    2A(g) ,if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Qc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2(g)    2A(g) ,if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Qc and time as equilibrium is established? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) A) and B)
G) D) and E)

Question 12

Consider the reaction N2(g) + O2(g)  2(g) + O2(g)    2NO(g) ,for which Kc = 0.10 at 2000ºC.Starting with initial concentrations of 0.040 M for N2 and 0.040 M for O2 ,what is the equilibrium concentration of NO? A) 0.0096 M B) 0.011 M C) 0.019 M D) 0.080 M E) 0.10 M" class="answers-bank-image d-inline" rel="preload" > 2NO(g) ,for which Kc = 0.10 at 2000ºC.Starting with initial concentrations of 0.040 M for N2 and 0.040 M for O2 ,what is the equilibrium concentration of NO?

Accepted Answer

A)  0.0096 M
B)  0.011 M
C)  0.019 M
D)  0.080 M
E)  0.10 MF) A) and B)
G) C) and D)

Question 13

For the following reaction at equilibrium,which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g)  2(g) ,ΔHºrxn = 30 kJ/mol A) Increase the total pressure by decreasing the volume B) Add more NO C) Remove Br2 D) Lower the temperature E) Remove NOBr selectively" class="answers-bank-image d-inline" rel="preload" > 2NO(g) + Br2(g) ,ΔHºrxn = 30 kJ/mol

Accepted Answer

A)  Increase the total pressure by decreasing the volume
B)  Add more NO
C)  Remove Br2
D)  Lower the temperature
E)  Remove NOBr selectivelyF) A) and E)
G) B) and E)

Question 14

The equilibrium constant for the reaction AgBr(s)  +(aq) + Br- (aq) is the solubility product constant,Ksp = 7.7 × 10-13 at 25°C.Calculate ΔG for the reaction when [Ag+] = 1.0 × 10-2 M and [Br-] = 1.0 × 10-3 M.Is the reaction spontaneous or nonspontaneous at these concentrations? (R = 8.314 J/K • mol)  A) ΔG = 69.1 kJ/mol,nonspontaneous B) ΔG = -69.1 kJ/mol,spontaneous C) ΔG = 97.5 kJ/mol,spontaneous D) ΔG = 40.6 kJ/mol,nonspontaneous E) ΔG = -97.5 kJ/mol,nonspontaneous" class="answers-bank-image d-inline" rel="preload" > Ag+(aq) + Br- (aq) is the solubility product constant,Ksp = 7.7 × 10-13 at 25°C.Calculate ΔG for the reaction when [Ag+] = 1.0 × 10-2 M and [Br-] = 1.0 × 10-3 M.Is the reaction spontaneous or nonspontaneous at these concentrations? (R = 8.314 J/K • mol)

Accepted Answer

A)  ΔG = 69.1 kJ/mol,nonspontaneous
B)  ΔG = -69.1 kJ/mol,spontaneous
C)  ΔG = 97.5 kJ/mol,spontaneous
D)  ΔG = 40.6 kJ/mol,nonspontaneous
E)  ΔG = -97.5 kJ/mol,nonspontaneousF) A) and D)
G) A) and B)

Question 15

At equilibrium,the rate of the forward reaction is equal to the rate of the reverse reaction.

Accepted Answer

A) True 
 B)False

Question 16

Nitrogen dioxide decomposes according to the reaction 2NO2(g)  2(g)    2NO(g) + O2(g)  Where KP = 4.48 × 10-13 at 25°C.What is the value for Kc?(R = 0.08206 L • atm/K • mol)  A) 1.83 × 10-14 B) 4.48 × 10-14 C) 9.19 × 10-13 D) 2.18 × 10-13 E) 1.10 × 10-11" class="answers-bank-image d-inline" rel="preload" > 2NO(g) + O2(g) 
Where KP = 4.48 × 10-13 at 25°C.What is the value for Kc?(R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  1.83 × 10-14
B)  4.48 × 10-14
C)  9.19 × 10-13
D)  2.18 × 10-13
E)  1.10 × 10-11F) C) and D)
G) B) and C)

Question 17

Suppose 25.0 g of HI(g) is injected into a 4.00-L reaction vessel that contains 20.0 g of I2(g) . When the system comes to equilibrium at 400.ºC,what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol) 
2HI(g)  2(g) . When the system comes to equilibrium at 400.ºC,what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol)  2HI(g)    H2(g) + I2(g) ,Kc = 0.0156 at 400.ºC A) 2.70 atm B) 13.0 atm C) 2.43 atm D) 0.815 atm E) 3.79 atm" class="answers-bank-image d-inline" rel="preload" > H2(g) + I2(g) ,Kc = 0.0156 at 400.ºC

Accepted Answer

A)  2.70 atm
B)  13.0 atm
C)  2.43 atm
D)  0.815 atm
E)  3.79 atmF) C) and D)
G) A) and B)

Question 18

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 B)
G) B) and E)

Question 19

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.What is KP for the reaction H2(g) + I2(g)  P for the reaction H2(g) + I2(g)    2HI(g) at this temperature? A) 0.35 B) 0.59 C) 1.0 D) 1.7 E) 2.9" class="answers-bank-image d-inline" rel="preload" > 2HI(g) at this temperature?

Accepted Answer

A)  0.35
B)  0.59
C)  1.0
D)  1.7
E)  2.9F) B) and D)
G) D) and E)

Question 20

For the reaction of A + B C + D + heat,the reverse reaction is exothermic.

Accepted Answer

A) True 
 B)False

Exam 15: Chemical Equilibrium

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) 2NO(g) + O₂(g) Where K_P = 4.48 × 10^-13 at 25°C.What is the value for K_c?(R = 0.08206 L • atm/K • mol)

Correct Answer
verified

For the reaction of A + B C + D + heat,the reverse reaction is exothermic.

Correct Answer
verified

What is defined as a fraction with equilibrium product concentrations in the numerator and equilibrium reactant concentrations in the denominator and each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?

Correct Answer
verified

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 K_c for this reaction at 298 K? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

Correct Answer
verified

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g).If nitrogen is added to the system at equilibrium,what will happen to the ammonia concentration?

Correct Answer
verified
The ammoni...
View Answer

For the equilibrium A₂(g) 2A(g) ,if a sample of A₂(g) is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Q_c and time as equilibrium is established?

Correct Answer
verified

Which is the correct equilibrium constant expression for the following reaction? FeO(s) + H₂(g) Fe(s) + H₂O(g)

Correct Answer
verified

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.What is K_P for the reaction H₂(g) + I₂(g) 2HI(g) at this temperature?

Correct Answer
verified

Correct Answer
verified

A temperature increase favors an endothermic reaction.

Correct Answer
verified

Consider the reaction N₂(g) + O₂(g) 2NO(g) ,for which K_c = 0.10 at 2000ºC.Starting with initial concentrations of 0.040 M for N₂ and 0.040 M for O₂ ,what is the equilibrium concentration of NO?

Correct Answer
verified

When the reaction 2H₂S(g) 2H₂(g) + S₂(g) is carried out at 1065°C,K_P = 0.012.Starting with pure H₂S at 1065°C,what must the initial pressure of H₂S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H₂(g) ?

Correct Answer
verified

The solubility product constant,K_sp,at 25°C for AgI(s) in water has the value 8.3 × 10^-17. Calculate ΔG at 25°C for the process AgI(s) Ag⁺(aq) + I^-(aq) where [Ag⁺] = 9.1 × 10^-9 M and [I^-] = 9.1 × 10^-9 M.(R = 8.314 J/K • mol)

Correct Answer
verified

For the following reaction at equilibrium,which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g) + Br₂(g) ,ΔHº_rxn = 30 kJ/mol

Correct Answer
verified

Correct Answer
verified

At 450°C,tert-butyl alcohol decomposes into water and isobutene. (CH₃) 3COH(g) (CH₃) ₂CCH₂(g) + H₂O(g) A reaction vessel contains these compounds at equilibrium.What will happen if the volume of the container is reduced by 50% at constant temperature?

Correct Answer
verified

Suppose 25.0 g of HI(g) is injected into a 4.00-L reaction vessel that contains 20.0 g of I₂(g) . When the system comes to equilibrium at 400.ºC,what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol) 2HI(g) H₂(g) + I₂(g) ,K_c = 0.0156 at 400.ºC

Correct Answer
verified

At equilibrium,the rate of the forward reaction is equal to the rate of the reverse reaction.

Correct Answer
verified

Correct Answer
verified

Exam 15: Chemical Equilibrium

Nitrogen dioxide decomposes according to the reaction 2NO2(g) 2NO(g) + O2(g) Where KP = 4.48 × 10-13 at 25°C.What is the value for Kc?(R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

For the reaction of A + B C + D + heat,the reverse reaction is exothermic.

Correct AnswerverifiedShow Answer

What is defined as a fraction with equilibrium product concentrations in the numerator and equilibrium reactant concentrations in the denominator and each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?

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

Suppose 75.0 g of PCl5(g) is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g) ,and the system is 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 = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

Consider the reaction N2(g)+ 3H2(g) 2NH3(g).If nitrogen is added to the system at equilibrium,what will happen to the ammonia concentration?

Correct AnswerverifiedThe ammoni...View AnswerShow Answer

For the equilibrium A2(g) 2A(g) ,if a sample of A2(g) is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Qc and time as equilibrium is established?

Correct AnswerverifiedShow Answer

Which is the correct equilibrium constant expression for the following reaction? FeO(s) + H2(g) Fe(s) + H2O(g)

Correct AnswerverifiedShow Answer

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.What is KP for the reaction H2(g) + I2(g) 2HI(g) at this temperature?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A temperature increase favors an endothermic reaction.

Correct AnswerverifiedShow Answer

Consider the reaction N2(g) + O2(g) 2NO(g) ,for which Kc = 0.10 at 2000ºC.Starting with initial concentrations of 0.040 M for N2 and 0.040 M for O2 ,what is the equilibrium concentration of NO?

Correct AnswerverifiedShow Answer

When the reaction 2H2S(g) 2H2(g) + S2(g) is carried out at 1065°C,KP = 0.012.Starting with pure H2S at 1065°C,what must the initial pressure of H2S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H2(g) ?

Correct AnswerverifiedShow Answer

The solubility product constant,Ksp,at 25°C for AgI(s) in water has the value 8.3 × 10-17. Calculate ΔG at 25°C for the process AgI(s) Ag+(aq) + I-(aq) where [Ag+] = 9.1 × 10-9 M and [I-] = 9.1 × 10-9 M.(R = 8.314 J/K • mol)

Correct AnswerverifiedShow Answer

For the following reaction at equilibrium,which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g) + Br2(g) ,ΔHºrxn = 30 kJ/mol

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

At 450°C,tert-butyl alcohol decomposes into water and isobutene. (CH3) 3COH(g) (CH3) 2CCH2(g) + H2O(g) A reaction vessel contains these compounds at equilibrium.What will happen if the volume of the container is reduced by 50% at constant temperature?

Correct AnswerverifiedShow Answer

Suppose 25.0 g of HI(g) is injected into a 4.00-L reaction vessel that contains 20.0 g of I2(g) . When the system comes to equilibrium at 400.ºC,what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol) 2HI(g) H2(g) + I2(g) ,Kc = 0.0156 at 400.ºC

Correct AnswerverifiedShow Answer

At equilibrium,the rate of the forward reaction is equal to the rate of the reverse reaction.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) 2NO(g) + O₂(g) Where K_P = 4.48 × 10^-13 at 25°C.What is the value for K_c?(R = 0.08206 L • atm/K • mol)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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 K_c for this reaction at 298 K? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

Correct Answer
verified

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g).If nitrogen is added to the system at equilibrium,what will happen to the ammonia concentration?

Correct Answer
verified
The ammoni...
View Answer

For the equilibrium A₂(g) 2A(g) ,if a sample of A₂(g) is placed in a sealed container and allowed to come to equilibrium,which graph best represents the relationship between Q_c and time as equilibrium is established?

Correct Answer
verified

Which is the correct equilibrium constant expression for the following reaction? FeO(s) + H₂(g) Fe(s) + H₂O(g)

Correct Answer
verified

The standard free energy of formation of gaseous hydrogen iodide is 1.30 kJ/mol at 25°C.What is K_P for the reaction H₂(g) + I₂(g) 2HI(g) at this temperature?

Correct Answer
verified

Correct Answer
verified

Correct Answer
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Consider the reaction N₂(g) + O₂(g) 2NO(g) ,for which K_c = 0.10 at 2000ºC.Starting with initial concentrations of 0.040 M for N₂ and 0.040 M for O₂ ,what is the equilibrium concentration of NO?

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When the reaction 2H₂S(g) 2H₂(g) + S₂(g) is carried out at 1065°C,K_P = 0.012.Starting with pure H₂S at 1065°C,what must the initial pressure of H₂S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H₂(g) ?

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The solubility product constant,K_sp,at 25°C for AgI(s) in water has the value 8.3 × 10^-17. Calculate ΔG at 25°C for the process AgI(s) Ag⁺(aq) + I^-(aq) where [Ag⁺] = 9.1 × 10^-9 M and [I^-] = 9.1 × 10^-9 M.(R = 8.314 J/K • mol)

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For the following reaction at equilibrium,which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g) + Br₂(g) ,ΔHº_rxn = 30 kJ/mol

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At 450°C,tert-butyl alcohol decomposes into water and isobutene. (CH₃) 3COH(g) (CH₃) ₂CCH₂(g) + H₂O(g) A reaction vessel contains these compounds at equilibrium.What will happen if the volume of the container is reduced by 50% at constant temperature?

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Suppose 25.0 g of HI(g) is injected into a 4.00-L reaction vessel that contains 20.0 g of I₂(g) . When the system comes to equilibrium at 400.ºC,what will be the total pressure inside the reaction vessel? (R = 0.08206 L • atm/K • mol) 2HI(g) H₂(g) + I₂(g) ,K_c = 0.0156 at 400.ºC

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