Question 1

If the reaction quotient Q has a smaller value than the related equilibrium constant, K, ________

Accepted Answer

A)  the reaction is at equilibrium.
B)  the reaction will continue to make more products.
C)  the reaction will consume products and make reactants.
D)  the reaction will release heat to achieve equilibrium.
E)  the value of K will decrease until it is equal to Q.F) B) and C)
G) B) and E)

Question 2

Under what conditions are the values of Kc and Kp for a given gas-phase equilibrium the same?

Accepted Answer

A)  if there is no change in the moles of gas in the reaction
B)  if there is no change in the temperature during the reaction
C)  if the coefficients of the reactants and products are the same
D)  if the pressure remains constant
E)  if either Kc or Kp  1F) B) and E)
G) A) and B)

Question 3

A series of four equilibrium steps can be defined for the following overall reaction: Cu2  4NH3 2  4NH3   [Cu(NH3) 4]2Koverall Cu2  NH3   [Cu(NH3) ]2K1 [Cu(NH3) ]2  NH3   [Cu(NH3) 2]2K2 Etc)  What is true about K4? A) K4  Koverall B) K4  K1K2K3 C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > [Cu(NH3) 4]2Koverall
Cu2  NH3 2  4NH3   [Cu(NH3) 4]2Koverall Cu2  NH3   [Cu(NH3) ]2K1 [Cu(NH3) ]2  NH3   [Cu(NH3) 2]2K2 Etc)  What is true about K4? A) K4  Koverall B) K4  K1K2K3 C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > [Cu(NH3) ]2K1
[Cu(NH3) ]2  NH3 2  4NH3   [Cu(NH3) 4]2Koverall Cu2  NH3   [Cu(NH3) ]2K1 [Cu(NH3) ]2  NH3   [Cu(NH3) 2]2K2 Etc)  What is true about K4? A) K4  Koverall B) K4  K1K2K3 C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > [Cu(NH3) 2]2K2
Etc) 
What is true about K4?

Accepted Answer

A)  K4  Koverall
B)  K4  K1K2K3
C)   2  4NH3   [Cu(NH3) 4]2Koverall Cu2  NH3   [Cu(NH3) ]2K1 [Cu(NH3) ]2  NH3   [Cu(NH3) 2]2K2 Etc)  What is true about K4? 
A)  K4  Koverall 
B)  K4  K1K2K3 
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2  4NH3   [Cu(NH3) 4]2Koverall Cu2  NH3   [Cu(NH3) ]2K1 [Cu(NH3) ]2  NH3   [Cu(NH3) 2]2K2 Etc)  What is true about K4? 
A)  K4  Koverall 
B)  K4  K1K2K3 
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2  4NH3   [Cu(NH3) 4]2Koverall Cu2  NH3   [Cu(NH3) ]2K1 [Cu(NH3) ]2  NH3   [Cu(NH3) 2]2K2 Etc)  What is true about K4? 
A)  K4  Koverall 
B)  K4  K1K2K3 
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) B) and C)
G) B) and D)

Question 4

Coal (C)  can be heated with steam (H2O)  at high temperatures to produce a mixture of hydrogen and carbon monoxide gases. Methanol, which is a useful fuel, can be produced from these gases by the reaction below. At a particular high temperature, the equilibrium concentrations are the following: [H2]  0.095 mol/L, [CO]  0.035 mol/L, and [CH3OH]  0.065 mol/L. What is the value of the equilibrium constant, Kc, for this reaction at this temperature?
2H2(g)   CO(g)  2O)  at high temperatures to produce a mixture of hydrogen and carbon monoxide gases. Methanol, which is a useful fuel, can be produced from these gases by the reaction below. At a particular high temperature, the equilibrium concentrations are the following: [H2]  0.095 mol/L, [CO]  0.035 mol/L, and [CH3OH]  0.065 mol/L. What is the value of the equilibrium constant, Kc, for this reaction at this temperature? 2H2(g)   CO(g)    CH3OH(g)  A) 4.70 B) 290 C) 206 D) 19.5 E) 4.86" class="answers-bank-image d-inline" rel="preload" > CH3OH(g)

Accepted Answer

A)  4.70
B)  290
C)  206
D)  19.5
E)  4.86F) A) and C)
G) C) and E)

Question 5

How would an increase in temperature affect the following equilibrium? N2(g)   3H2(g)  2(g)   3H2(g)    2NH3(g)    H°  92.0 kJ/mol A) More product would form and K would increase. B) More product would form but K would remain constant. C) K would be unaffected by a temperature change. D) More reactants would form but K would remain constant. E) More reactants would form and K would decrease." class="answers-bank-image d-inline" rel="preload" > 2NH3(g)  2(g)   3H2(g)    2NH3(g)    H°  92.0 kJ/mol A) More product would form and K would increase. B) More product would form but K would remain constant. C) K would be unaffected by a temperature change. D) More reactants would form but K would remain constant. E) More reactants would form and K would decrease." class="answers-bank-image d-inline" rel="preload" > H°  92.0 kJ/mol

Accepted Answer

A)  More product would form and K would increase.
B)  More product would form but K would remain constant.
C)  K would be unaffected by a temperature change.
D)  More reactants would form but K would remain constant.
E)  More reactants would form and K would decrease.F) A) and B)
G) B) and D)

Question 6

Carbon dioxide and argon, which is a noble or inert gas, are placed in a vessel and heated. Equilibrium is reached at some particular temperature. Carbon dioxide dissociates by the following reaction. 2CO2(g)  2(g)    2CO(g)   O2(g)  What is the result of increasing the pressure by adding more argon? I. The equilibrium shifts to produce more carbon dioxide and reduce the pressure. II. The equilibrium shifts to remove carbon dioxide and reduce the pressure. III. The equilibrium does not change because argon is not involved in the reaction. IV. The equilibrium does not change because the concentrations are not affected. A) I only B) II only C) III only D) IV only E) III and IV" class="answers-bank-image d-inline" rel="preload" > 2CO(g)   O2(g) 
What is the result of increasing the pressure by adding more argon?
I. The equilibrium shifts to produce more carbon dioxide and reduce the pressure.
II. The equilibrium shifts to remove carbon dioxide and reduce the pressure.
III. The equilibrium does not change because argon is not involved in the reaction.
IV. The equilibrium does not change because the concentrations are not affected.

Accepted Answer

A)  I only
B)  II only
C)  III only
D)  IV only
E)  III and IVF) A) and E)
G) A) and D)

Question 7

The forward rate constant, kf, and reverse rate constant, kr, for a chemical reaction are not equal. Which of the following must be true?

Accepted Answer

A)  The reaction will be unable to achieve equilibrium.
B)  kf and kr will become equal as equilibrium is approached, owing to concentration changes.
C)  kf and kr will become equal as equilibrium is approached, owing to temperature changes.
D)  kf and kr will remain unequal but the rates will become equal, owing to concentration changes.
E)  kf and kr will remain unequal but the rates will become equal, owing to temperature changes.F) A) and B)
G) A) and C)

Question 8

Given the following reactions and associated equilibrium constants 1  3.1       K2  4.5 what is the equilibrium constant for the following reaction? SO3(g)   NO(g)    SO2(g)   NO2(g)  Knew  ? A) 1.45 B) 7.17  10-2 C) 14.0 D) 6.89  10-1 E) 163" class="answers-bank-image d-inline" rel="preload" > 1  3.1       K2  4.5 what is the equilibrium constant for the following reaction? SO3(g)   NO(g)    SO2(g)   NO2(g)  Knew  ? A) 1.45 B) 7.17  10-2 C) 14.0 D) 6.89  10-1 E) 163" class="answers-bank-image d-inline" rel="preload" > 1  3.1       K2  4.5 what is the equilibrium constant for the following reaction? SO3(g)   NO(g)    SO2(g)   NO2(g)  Knew  ? A) 1.45 B) 7.17  10-2 C) 14.0 D) 6.89  10-1 E) 163" class="answers-bank-image d-inline" rel="preload" > K1  3.1 1  3.1       K2  4.5 what is the equilibrium constant for the following reaction? SO3(g)   NO(g)    SO2(g)   NO2(g)  Knew  ? A) 1.45 B) 7.17  10-2 C) 14.0 D) 6.89  10-1 E) 163" class="answers-bank-image d-inline" rel="preload" > 1  3.1       K2  4.5 what is the equilibrium constant for the following reaction? SO3(g)   NO(g)    SO2(g)   NO2(g)  Knew  ? A) 1.45 B) 7.17  10-2 C) 14.0 D) 6.89  10-1 E) 163" class="answers-bank-image d-inline" rel="preload" > 1  3.1       K2  4.5 what is the equilibrium constant for the following reaction? SO3(g)   NO(g)    SO2(g)   NO2(g)  Knew  ? A) 1.45 B) 7.17  10-2 C) 14.0 D) 6.89  10-1 E) 163" class="answers-bank-image d-inline" rel="preload" > K2  4.5 what is the equilibrium constant for the following reaction?
SO3(g)   NO(g)  1  3.1       K2  4.5 what is the equilibrium constant for the following reaction? SO3(g)   NO(g)    SO2(g)   NO2(g)  Knew  ? A) 1.45 B) 7.17  10-2 C) 14.0 D) 6.89  10-1 E) 163" class="answers-bank-image d-inline" rel="preload" > SO2(g)   NO2(g)  Knew  ?

Accepted Answer

A)  1.45
B)  7.17  10-2
C)  14.0
D)  6.89  10-1
E)  163F) C) and D)
G) B) and E)

Question 9

Water can decompose at an elevated temperature to give hydrogen and oxygen according to the equation below. At a particular temperature, the partial pressures of H2O, H2, and O2 are 0.055 atm, 0.0065 atm, and 0.0045 atm, respectively, at equilibrium. What is the value of the equilibrium constant, KP, for this reaction at this temperature? 2H2O(g)  2O, H2, and O2 are 0.055 atm, 0.0065 atm, and 0.0045 atm, respectively, at equilibrium. What is the value of the equilibrium constant, KP, for this reaction at this temperature? 2H2O(g)    2H2(g)   O2(g)  A) 5.3  104 B) 3.5  106 C) 6.3  105 D) 1.6  104 E) 3.0  104" class="answers-bank-image d-inline" rel="preload" > 2H2(g)   O2(g)

Accepted Answer

A)  5.3  104
B)  3.5  106
C)  6.3  105
D)  1.6  104
E)  3.0  104F) B) and C)
G) B) and D)

Question 10

The sulfide ion, S2, reacts with water as a weak base: S2  H2O 2, reacts with water as a weak base: S2  H2O   SH  OH K  1.0 If sodium sulfide were dissolved in water to make a solution of 0.50 M, what would be the resulting concentration of OH? A) 0.50 M B) 0.37 M C) 0.63 M D) 1.0 M E) 0.19 M" class="answers-bank-image d-inline" rel="preload" > SH  OH K  1.0
If sodium sulfide were dissolved in water to make a solution of 0.50 M, what would be the resulting concentration of OH?

Accepted Answer

A)  0.50 M
B)  0.37 M
C)  0.63 M
D)  1.0 M
E)  0.19 MF) A) and D)
G) C) and E)

Question 11

In the following reaction, which of the statements is true, given the concentrations of each species? N2(g)   3 H2(g)  2(g)   3 H2(g)    2 NH3(g)  K  9.60 [N2]  [H2]  0.100 M and [NH3]  0.352 M A) The reaction is at equilibrium. B) More ammonia must form to achieve equilibrium. C) More nitrogen and hydrogen must form to achieve equilibrium. D) More nitrogen must be consumed to achieve equilibrium. E) Equilibrium cannot be established in the system." class="answers-bank-image d-inline" rel="preload" > 2 NH3(g)  K  9.60
[N2]  [H2]  0.100 M and [NH3]  0.352 M

Accepted Answer

A)  The reaction is at equilibrium.
B)  More ammonia must form to achieve equilibrium.
C)  More nitrogen and hydrogen must form to achieve equilibrium.
D)  More nitrogen must be consumed to achieve equilibrium.
E)  Equilibrium cannot be established in the system.F) C) and D)
G) B) and E)

Question 12

Which of the listed perturbations will change the position of equilibrium for the following reaction? List those that do as a sequence of letters (e.g., ACE) .
NH4CO2NH2(s)  4CO2NH2(s)    2NH3(g)   CO2(g)  A)  Increasing the quantity of NH4CO2NH2(s)  B)  Removing CO2(g)  C)  Increasing the total pressure by adding argon gas D)  Increasing the volume of the container E)  Increasing the temperature" class="answers-bank-image d-inline" rel="preload" > 2NH3(g)   CO2(g)

Accepted Answer

A)   Increasing the quantity of NH4CO2NH2(s) 
B)   Removing CO2(g) 
C)   Increasing the total pressure by adding argon gas
D)   Increasing the volume of the container
E)   Increasing the temperatureF) A) and B)
G) C) and E)

Question 13

Equilibrium constants can be expressed in terms of molar concentration, Kc, or partial pressure, KP. To relate these two equilibrium constants to each other, ________

Accepted Answer

A)  each concentration must be multiplied by the factor RT.
B)  each pressure must be multiplied by the factor RT.
C)  Kc must be multiplied by the factor RT.
D)  KP must be multiplied by the factor RT.
E)  nothing must be done because their values are equal.F) All of the above
G) D) and E)

Question 14

Identify whether or not perturbations A-D will affect the equilibrium concentrations of reactants and products in a gas-phase endothermic chemical reaction that involves one or more gases. If all have an effect on the equilibrium concentrations, select response E. Otherwise, identify the one that does not affect the equilibrium concentrations.

Accepted Answer

A)  adding reactants to a gas or solution reaction
B)  removing products from a gas or solution reaction
C)  decreasing the temperature
D)  increasing pressure by adding an inert gas to a reaction in the gas phase
E)  All of the above are perturbations to chemical equilibrium.F) A) and D)
G) A) and C)

Question 15

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH3), the value of Kp is 4.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012. What is the value of Kc for the same reaction?

Accepted Answer

2.8 F1F1F1...

Question 16

Which of the following is true for a chemical reaction at equilibrium?

Accepted Answer

A)  Only the forward reaction stops.
B)  Only the reverse reaction stops.
C)  Both the forward and reverse reactions stop.
D)  The rate constants for the forward and reverse reactions are equal.
E)  The rates of the forward and reverse reactions are equal.F) C) and E)
G) A) and C)

Question 17

Solid mercury(II)  oxide decomposes when heated to produce liquid mercury and oxygen. 2HgO(s)   O2(g)  An amount of mercury(II)  oxide is placed in a vessel at a particular temperature and allowed to reach equilibrium. How could the amount of liquid mercury in the vessel be increased? I. adding more mercury(II)  oxide II. removing some oxygen III. increasing the volume of the vessel A) I only B) II only C) III only D) I and II E) II and III" class="answers-bank-image d-inline" rel="preload" > 2Hg(l)   O2(g) 
An amount of mercury(II)  oxide is placed in a vessel at a particular temperature and allowed to reach equilibrium. How could the amount of liquid mercury in the vessel be increased?
I. adding more mercury(II)  oxide
II. removing some oxygen
III. increasing the volume of the vessel

Accepted Answer

A)  I only
B)  II only
C)  III only
D)  I and II
E)  II and IIIF) C) and D)
G) All of the above

Question 18

Hydrofluoric acid, HF, dissociates in water according to the following reaction.
HF(aq)  HF1F1F1S1F1F1F10(aq) F1F1F1S1F1F1F10 FF1F1F1S1F1F1F10(aq)
Kc F1F1F1S1F1F1F10 3.5 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104
What is the concentration of HF1F1F1S1F1F1F10 in a 0.0100 M solution of HF?

Accepted Answer

Use the quadratic fo...

Question 19

If the reaction quotient Q has a larger value than the related equilibrium constant, K, ________

Accepted Answer

A)  the reaction is at equilibrium.
B)  the reaction will continue to make more products.
C)  the reaction will consume products and make reactants.
D)  the reaction will release heat to achieve equilibrium.
E)  the value of K will increase until it is equal to Q.F) D) and E)
G) B) and C)

Question 20

For the following reaction, Kp = 137 at 3.50 102K. What is the value of Kc? 2C4H10(l)   3O2(g)  p = 137 at 3.50 102K. What is the value of Kc? 2C4H10(l)   3O2(g)    8CO2(g)   10H2O(g)  A) 7.03106 B) 5.79103 C) 4.77 D) 3.24106 E) 2.67109" class="answers-bank-image d-inline" rel="preload" > 8CO2(g)   10H2O(g)

Accepted Answer

A)  7.03106
B)  5.79103
C)  4.77
D)  3.24106
E)  2.67109F) D) and E)
G) A) and B)

Exam 14: Chemical Equilibrium: How Much Product Does a Reaction Really Make

The forward rate constant, k_f, and reverse rate constant, k_r, for a chemical reaction are not equal. Which of the following must be true?

Correct Answer
verified

Hydrofluoric acid, HF, dissociates in water according to the following reaction. HF(aq) H^(aq)  F^(aq) K_c  3.5  10^⁴ What is the concentration of H^ in a 0.0100 M solution of HF?

Correct Answer
verified
Use the quadratic fo...
View Answer

The sulfide ion, S²^, reacts with water as a weak base: S²^  H₂O SH^  OH^K  1.0 If sodium sulfide were dissolved in water to make a solution of 0.50 M, what would be the resulting concentration of OH^?

Correct Answer
verified

Equilibrium constants can be expressed in terms of molar concentration, K_c, or partial pressure, K_P. To relate these two equilibrium constants to each other, ________

Correct Answer
verified

Correct Answer
verified

If the reaction quotient Q has a larger value than the related equilibrium constant, K, ________

Correct Answer
verified

Correct Answer
verified

Given the following reactions and associated equilibrium constants K₁ 3.1 K₂ 4.5 what is the equilibrium constant for the following reaction? SO₃(g)  NO(g) SO₂(g)  NO₂(g) K_new ?

Correct Answer
verified

Which of the listed perturbations will change the position of equilibrium for the following reaction? List those that do as a sequence of letters (e.g., ACE) . NH₄CO₂NH₂(s) 2NH₃(g)  CO₂(g)

Correct Answer
verified

Correct Answer
verified

How would an increase in temperature affect the following equilibrium? N₂(g)  3H₂(g) 2NH₃(g) H^°  92.0 kJ/mol

Correct Answer
verified

Under what conditions are the values of K_c and K_p for a given gas-phase equilibrium the same?

Correct Answer
verified

Which of the following is true for a chemical reaction at equilibrium?

Correct Answer
verified

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH₃), the value of K_p is 4.5  10^¹². What is the value of K_c for the same reaction?

Correct Answer
verified
2.8 F1F1F1...
View Answer

A series of four equilibrium steps can be defined for the following overall reaction: Cu²^  4NH₃ [Cu(NH₃) ₄]²^K_overall Cu²^  NH₃ [Cu(NH₃) ]²^K₁ [Cu(NH₃) ]²^  NH₃ [Cu(NH₃) ₂]²^K₂ Etc) What is true about K₄?

Correct Answer
verified

In the following reaction, which of the statements is true, given the concentrations of each species? N₂(g)  3 H₂(g) 2 NH₃(g) K  9.60 [N₂]  [H₂]  0.100 M and [NH₃]  0.352 M

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

If the reaction quotient Q has a smaller value than the related equilibrium constant, K, ________

Correct Answer
verified

For the following reaction, K_p = 137 at 3.50 10²K. What is the value of K_c? 2C₄H₁₀(l)  3O₂(g) 8CO₂(g)  10H₂O(g)

Correct Answer
verified

Exam 14: Chemical Equilibrium: How Much Product Does a Reaction Really Make

The forward rate constant, kf, and reverse rate constant, kr, for a chemical reaction are not equal. Which of the following must be true?

Correct AnswerverifiedShow Answer

Hydrofluoric acid, HF, dissociates in water according to the following reaction. HF(aq) H(aq)  F(aq) Kc  3.5  104 What is the concentration of H in a 0.0100 M solution of HF?

Correct AnswerverifiedUse the quadratic fo...View AnswerShow Answer

The sulfide ion, S2, reacts with water as a weak base: S2  H2O SH  OH K  1.0 If sodium sulfide were dissolved in water to make a solution of 0.50 M, what would be the resulting concentration of OH?

Correct AnswerverifiedShow Answer

Equilibrium constants can be expressed in terms of molar concentration, Kc, or partial pressure, KP. To relate these two equilibrium constants to each other, ________

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

If the reaction quotient Q has a larger value than the related equilibrium constant, K, ________

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Given the following reactions and associated equilibrium constants K1  3.1 K2  4.5 what is the equilibrium constant for the following reaction? SO3(g)  NO(g) SO2(g)  NO2(g) Knew  ?

Correct AnswerverifiedShow Answer

Which of the listed perturbations will change the position of equilibrium for the following reaction? List those that do as a sequence of letters (e.g., ACE) . NH4CO2NH2(s) 2NH3(g)  CO2(g)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

How would an increase in temperature affect the following equilibrium? N2(g)  3H2(g) 2NH3(g) H°  92.0 kJ/mol

Correct AnswerverifiedShow Answer

Under what conditions are the values of Kc and Kp for a given gas-phase equilibrium the same?

Correct AnswerverifiedShow Answer

Which of the following is true for a chemical reaction at equilibrium?

Correct AnswerverifiedShow Answer

For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH3), the value of Kp is 4.5  1012. What is the value of Kc for the same reaction?

Correct Answerverified2.8 F1F1F1...View AnswerShow Answer

A series of four equilibrium steps can be defined for the following overall reaction: Cu2  4NH3 [Cu(NH3) 4]2Koverall Cu2  NH3 [Cu(NH3) ]2K1 [Cu(NH3) ]2  NH3 [Cu(NH3) 2]2K2 Etc) What is true about K4?

Correct AnswerverifiedShow Answer

In the following reaction, which of the statements is true, given the concentrations of each species? N2(g)  3 H2(g) 2 NH3(g) K  9.60 [N2]  [H2]  0.100 M and [NH3]  0.352 M

Correct AnswerverifiedShow Answer

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If the reaction quotient Q has a smaller value than the related equilibrium constant, K, ________

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For the following reaction, Kp = 137 at 3.50 102K. What is the value of Kc? 2C4H10(l)  3O2(g) 8CO2(g)  10H2O(g)

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The forward rate constant, k_f, and reverse rate constant, k_r, for a chemical reaction are not equal. Which of the following must be true?

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Hydrofluoric acid, HF, dissociates in water according to the following reaction. HF(aq) H^(aq)  F^(aq) K_c  3.5  10^⁴ What is the concentration of H^ in a 0.0100 M solution of HF?

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Use the quadratic fo...
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The sulfide ion, S²^, reacts with water as a weak base: S²^  H₂O SH^  OH^K  1.0 If sodium sulfide were dissolved in water to make a solution of 0.50 M, what would be the resulting concentration of OH^?

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Equilibrium constants can be expressed in terms of molar concentration, K_c, or partial pressure, K_P. To relate these two equilibrium constants to each other, ________

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Given the following reactions and associated equilibrium constants K₁ 3.1 K₂ 4.5 what is the equilibrium constant for the following reaction? SO₃(g)  NO(g) SO₂(g)  NO₂(g) K_new ?

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Which of the listed perturbations will change the position of equilibrium for the following reaction? List those that do as a sequence of letters (e.g., ACE) . NH₄CO₂NH₂(s) 2NH₃(g)  CO₂(g)

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How would an increase in temperature affect the following equilibrium? N₂(g)  3H₂(g) 2NH₃(g) H^°  92.0 kJ/mol

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Under what conditions are the values of K_c and K_p for a given gas-phase equilibrium the same?

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For the reaction of hydrogen and nitrogen gases at 30°C to form two moles of ammonia gas (NH₃), the value of K_p is 4.5  10^¹². What is the value of K_c for the same reaction?

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2.8 F1F1F1...
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A series of four equilibrium steps can be defined for the following overall reaction: Cu²^  4NH₃ [Cu(NH₃) ₄]²^K_overall Cu²^  NH₃ [Cu(NH₃) ]²^K₁ [Cu(NH₃) ]²^  NH₃ [Cu(NH₃) ₂]²^K₂ Etc) What is true about K₄?

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In the following reaction, which of the statements is true, given the concentrations of each species? N₂(g)  3 H₂(g) 2 NH₃(g) K  9.60 [N₂]  [H₂]  0.100 M and [NH₃]  0.352 M

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For the following reaction, K_p = 137 at 3.50 10²K. What is the value of K_c? 2C₄H₁₀(l)  3O₂(g) 8CO₂(g)  10H₂O(g)

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