Question 1

What is the correct equilibrium constant expression for this reaction?
2HI(g)  H2(g)+ I2(g)

Accepted Answer

Question 2

Consider the following equilibrium,
4NH3(g)+ 3O2(g)  2N2(g)+ 6H2O(g)+ 1531 kJ
State whether the concentrations of the reactants would increase, decrease, or remain constant after nitrogen gas was removed from the system.

Accepted Answer

Question 3

Consider the chemical reaction 2NH3(g)  N2(g)+ 3H2(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where Kc = 4.0 * 10-2. Initially, 1,220 moles of NH3(g)are present. Estimate the equilibrium concentration of H2(g).

Accepted Answer

The answer of Consider the chemical reaction 2NH3(g)  N2(g)+...

Question 4

At 400ºC, Kc = 64 for the equilibrium H2(g) + I2(g)  c = 64 for the equilibrium H2(g) + I2(g)    2HI(g) . If 3.00 mol H2 and 3.00 mol I2 are introduced into an empty 4.0 L vessel, find the equilibrium concentration of HI at 400ºC. A) 0.15 M B) 1.2 M C) 2.4 M D) 4.8 M E) 5.8 M" class="answers-bank-image d-inline" rel="preload" > 2HI(g) . If 3.00 mol H2 and 3.00 mol I2 are introduced into an empty 4.0 L vessel, find the equilibrium concentration of HI at 400ºC.

Accepted Answer

A)  0.15 M
B)  1.2 M
C)  2.4 M
D)  4.8 M
E)  5.8 MF) B) and D)
G) D) and E)

Question 5

The reaction 2NO(g)  2(g) + O2(g) is exothermic,  \Delta Hºrxn = -180 kJ/mol. Which one of these statements is true? A) Kp at 1,000 K is less than Kp at 2,000 K. B) Kp at 1,000 K is larger than Kp at 2,000 K. C) The Kp's at 1000 K and 2000 K are the same. D) Kp depends on total pressure as well as temperature. " class="answers-bank-image d-inline" rel="preload" > N2(g) + O2(g) is exothermic,  Δ\DeltaΔ Hºrxn = -180 kJ/mol. Which one of these statements is true?

Accepted Answer

A)  Kp at 1,000 K is less than Kp at 2,000 K.
B)  Kp at 1,000 K is larger than Kp at 2,000 K.
C)  The Kp's at 1000 K and 2000 K are the same.
D)  Kp depends on total pressure as well as temperature. E) A) and B)
F) C) and D)

Question 6

In which of these gas-phase equilibria is the yield of products increased by increasing the total pressure on the reaction mixture?

Accepted Answer

A)  CO(g) + H2O(g)  2O(g)    CO2(g) + H2(g)  
B)  2NO(g) + Cl2(g)    2NOCl(g)  
C)  2SO3(g)    2SO2(g) + O2(g)  
D)  PCl5(g)    PCl3(g) + Cl2(g) " class="answers-bank-image d-inline" rel="preload" > CO2(g) + H2(g) 
B)  2NO(g) + Cl2(g)   2NOCl(g) 
C)  2SO3(g)   2SO2(g) + O2(g) 
D)  PCl5(g)   PCl3(g) + Cl2(g) E) B) and D)
F) B) and C)

Question 7

Hydrogen iodide decomposes according to the equation:
2HI(g)  H2(g)+ I2(g), Kc = 0.0156 at 400ºC
A 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC.
Calculate the concentration of H2 equilibrium.

Accepted Answer

Question 8

Consider the two gaseous equilibria: SO2(g) + 1/2O2(g)  2(g) + 1/2O2(g)     SO3(g) K1  2SO3(g)      SO2(g) + O2(g) K2 The values of the equilibrium constants K1 and K2 are related by A) K2 = K12 B) K22 = K1 C) K2 = 1/K   D) K2 = 1/K1 E) none of these." class="answers-bank-image d-inline" rel="preload" >  SO3(g) K1
 2SO3(g)  2(g) + 1/2O2(g)     SO3(g) K1  2SO3(g)      SO2(g) + O2(g) K2 The values of the equilibrium constants K1 and K2 are related by A) K2 = K12 B) K22 = K1 C) K2 = 1/K   D) K2 = 1/K1 E) none of these." class="answers-bank-image d-inline" rel="preload" >   SO2(g) + O2(g) K2
The values of the equilibrium constants K1 and K2 are related by

Accepted Answer

A)  K2 = K12
B)  K22 = K1
C)  K2 = 1/K 2(g) + 1/2O2(g)     SO3(g) K1  2SO3(g)      SO2(g) + O2(g) K2 The values of the equilibrium constants K1 and K2 are related by 
A)  K2 = K12 
B)  K22 = K1 
C)  K2 = 1/K   
D)  K2 = 1/K1 
E)  none of these." class="answers-bank-image d-inline" rel="preload" >
D)  K2 = 1/K1
E)  none of these.F) B) and C)
G) D) and E)

Question 9

Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J  CO(g)+ H2(g). What will happen to the mass of carbon if we add gaseous water to the system?

Accepted Answer

The mass o...

Question 10

Kc for the reaction CO2(g)+ H2(g)  H2O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon monoxide in the final equilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

Accepted Answer

Question 11

A solution was prepared such that the initial concentrations of Cu2+(aq)and CN-(aq)were 0.0120 M and 0.0400 M, respectively. These ions react according to the following chemical equation
Cu2+(aq)+ 4CN-(aq)  Cu(CN)42-(aq)Kc = 1.0 * 1025
 What will be the concentration of Cu2+(aq)at equilibrium?

Accepted Answer

The answer of A solution was prepared such that the...

Question 12

On analysis, an equilibrium mixture for the reaction 2H2S(g)  2S(g)     2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction. A) 1.6 B) 3.2 C) 12.8 D) 0.64 E) 0.8" class="answers-bank-image d-inline" rel="preload" >  2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction.

Accepted Answer

A)  1.6
B)  3.2
C)  12.8
D)  0.64
E)  0.8F) A) and E)
G) A) and B)

Question 13

For the equilibrium reaction 2SO2(g) + O2(g)  2(g) + O2(g)    2SO3(g) ,  \Delta Hºrxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase? A) Decrease the temperature. B) Add SO2 gas. C) Remove O2 gas. D) Add a catalyst. E) None of these. " class="answers-bank-image d-inline" rel="preload" > 2SO3(g) ,  Δ\DeltaΔ Hºrxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase?

Accepted Answer

A)  Decrease the temperature.
B)  Add SO2 gas.
C)  Remove O2 gas.
D)  Add a catalyst.
E)  None of these. F) D) and E)
G) C) and E)

Question 14

Consider the chemical reaction 2NH3(g)  N2(g)+ 3H2(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where Kc = 4.0 * 10-2. Initially, 1,220 moles of NH3(g)are present. Estimate the equilibrium concentration of N2(g).

Accepted Answer

The answer of Consider the chemical reaction 2NH3(g)  N2(g)+...

Question 15

Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J CO(g)+ H2(g). If additional gaseous water is added to this reaction mixture, what will happen to the temperature of the mixture?

Accepted Answer

The temper...

Question 16

Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.

Accepted Answer

A catalyst affects both the fo...

Question 17

The following reactions occur at 500 K. Arrange them in order of increasing tendency to proceed to completion (least completion →\rarr→  greatest completion) . 
1) 2NOCl  2NO + Cl2 Kp = 1.7 * 10- 2   2) N2O4    2NO2 Kp = 1.5 * 103   3) 2SO3    2SO2 + O2 Kp = 1.3 * 10 -5   4) 2NO2    2NO + O2 Kp = 5.9 * 10 -5 A) 2   2NO + Cl2 Kp = 1.7 * 10- 2
 
2) N2O4   2NO2 Kp = 1.5 * 103
 
3) 2SO3   2SO2 + O2 Kp = 1.3 * 10 -5
 
4) 2NO2   2NO + O2 Kp = 5.9 * 10 -5

Accepted Answer

A)  2 
B)  3 
C)  3 
D)  4 
E)  4 < 3 < 1 < 2 F) C) and D)
G) A) and D)

Question 18

The data below refer to the following reaction:
2NO(g)+ Br2(g)  2NOBr(g)  Calculate Kc.

Accepted Answer

Question 19

Two moles of PCl5 are placed in a 5.0 L container. Dissociation takes place according to the equation PCl5 (g)  PCl3(g)+ Cl2(g). At equilibrium, 0.40 mol of Cl2 are present. Calculate the equilibrium constant (Kc)for this reaction under the conditions of this experiment.

Accepted Answer

Exam 15: Chemical Equilibrium

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Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g). If additional gaseous water is added to this reaction mixture, what will happen to the temperature of the mixture?

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The temper...
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Two moles of PCl₅ are placed in a 5.0 L container. Dissociation takes place according to the equation PCl₅ (g) PCl₃(g)+ Cl₂(g). At equilibrium, 0.40 mol of Cl₂ are present. Calculate the equilibrium constant (K_c)for this reaction under the conditions of this experiment.

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The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Calculate K_c.

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Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g). What will happen to the mass of carbon if we add gaseous water to the system?

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The mass o...
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What is the correct equilibrium constant expression for this reaction? 2HI(g) H₂(g)+ I₂(g)

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In which of these gas-phase equilibria is the yield of products increased by increasing the total pressure on the reaction mixture?

Correct Answer
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At 400ºC, K_c = 64 for the equilibrium H₂(g) + I₂(g) 2HI(g) . If 3.00 mol H₂ and 3.00 mol I₂ are introduced into an empty 4.0 L vessel, find the equilibrium concentration of HI at 400ºC.

Correct Answer
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Correct Answer
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K_c for the reaction CO₂(g)+ H₂(g) H₂O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon monoxide in the final equilibrium system obtained by initially adding 1.00 mol of H₂, 2.00 mol of CO₂, 0.750 mol of H₂O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

Correct Answer
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Correct Answer
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Consider the two gaseous equilibria: SO₂(g) + ¹/₂O₂(g) SO₃(g) K₁ 2SO₃(g) SO₂(g) + O₂(g) K₂ The values of the equilibrium constants K₁ and K₂are related by

Correct Answer
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Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.

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A catalyst affects both the fo...
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Hydrogen iodide decomposes according to the equation: 2HI(g) H₂(g)+ I₂(g), K_c = 0.0156 at 400ºC A 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC. Calculate the concentration of H₂ equilibrium.

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Consider the chemical reaction 2NH₃(g) N₂(g)+ 3H₂(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g)are present. Estimate the equilibrium concentration of N₂(g).

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Consider the chemical reaction 2NH₃(g) N₂(g)+ 3H₂(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g)are present. Estimate the equilibrium concentration of H₂(g).

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On analysis, an equilibrium mixture for the reaction 2H₂S(g) 2H₂(g) + S₂(g) was found to contain 1.0 mol H₂S, 4.0 mol H₂, and 0.80 mol S₂ in a 4.0 L vessel. Calculate the equilibrium constant, K_c, for this reaction.

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Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after nitrogen gas was removed from the system.

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Exam 15: Chemical Equilibrium

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A solution was prepared such that the initial concentrations of Cu2+(aq)and CN-(aq)were 0.0120 M and 0.0400 M, respectively. These ions react according to the following chemical equation Cu2+(aq)+ 4CN-(aq) Cu(CN)42-(aq)Kc = 1.0 * 1025 What will be the concentration of Cu2+(aq)at equilibrium?

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Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J CO(g)+ H2(g). If additional gaseous water is added to this reaction mixture, what will happen to the temperature of the mixture?

Correct AnswerverifiedThe temper...View AnswerShow Answer

Two moles of PCl5 are placed in a 5.0 L container. Dissociation takes place according to the equation PCl5 (g) PCl3(g)+ Cl2(g). At equilibrium, 0.40 mol of Cl2 are present. Calculate the equilibrium constant (Kc)for this reaction under the conditions of this experiment.

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The data below refer to the following reaction: 2NO(g)+ Br2(g) 2NOBr(g) Calculate Kc.

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Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J CO(g)+ H2(g). What will happen to the mass of carbon if we add gaseous water to the system?

Correct AnswerverifiedThe mass o...View AnswerShow Answer

What is the correct equilibrium constant expression for this reaction? 2HI(g) H2(g)+ I2(g)

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In which of these gas-phase equilibria is the yield of products increased by increasing the total pressure on the reaction mixture?

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At 400ºC, Kc = 64 for the equilibrium H2(g) + I2(g) 2HI(g) . If 3.00 mol H2 and 3.00 mol I2 are introduced into an empty 4.0 L vessel, find the equilibrium concentration of HI at 400ºC.

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For the equilibrium reaction 2SO2(g) + O2(g) 2SO3(g) , Δ\DeltaΔ Hºrxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase?

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Kc for the reaction CO2(g)+ H2(g) H2O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon monoxide in the final equilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

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The reaction 2NO(g) N2(g) + O2(g) is exothermic, Δ\DeltaΔ Hºrxn = -180 kJ/mol. Which one of these statements is true?

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Consider the two gaseous equilibria: SO2(g) + 1/2O2(g) SO3(g) K1 2SO3(g) SO2(g) + O2(g) K2 The values of the equilibrium constants K1 and K2 are related by

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Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.

Correct AnswerverifiedA catalyst affects both the fo...View AnswerShow Answer

Hydrogen iodide decomposes according to the equation: 2HI(g) H2(g)+ I2(g), Kc = 0.0156 at 400ºC A 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC. Calculate the concentration of H2 equilibrium.

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Consider the chemical reaction 2NH3(g) N2(g)+ 3H2(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where Kc = 4.0 * 10-2. Initially, 1,220 moles of NH3(g)are present. Estimate the equilibrium concentration of N2(g).

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Consider the chemical reaction 2NH3(g) N2(g)+ 3H2(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where Kc = 4.0 * 10-2. Initially, 1,220 moles of NH3(g)are present. Estimate the equilibrium concentration of H2(g).

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On analysis, an equilibrium mixture for the reaction 2H2S(g) 2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction.

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Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after nitrogen gas was removed from the system.

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Correct Answer
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Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g). If additional gaseous water is added to this reaction mixture, what will happen to the temperature of the mixture?

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The temper...
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Two moles of PCl₅ are placed in a 5.0 L container. Dissociation takes place according to the equation PCl₅ (g) PCl₃(g)+ Cl₂(g). At equilibrium, 0.40 mol of Cl₂ are present. Calculate the equilibrium constant (K_c)for this reaction under the conditions of this experiment.

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The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Calculate K_c.

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Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g). What will happen to the mass of carbon if we add gaseous water to the system?

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The mass o...
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What is the correct equilibrium constant expression for this reaction? 2HI(g) H₂(g)+ I₂(g)

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Correct Answer
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At 400ºC, K_c = 64 for the equilibrium H₂(g) + I₂(g) 2HI(g) . If 3.00 mol H₂ and 3.00 mol I₂ are introduced into an empty 4.0 L vessel, find the equilibrium concentration of HI at 400ºC.

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Correct Answer
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K_c for the reaction CO₂(g)+ H₂(g) H₂O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon monoxide in the final equilibrium system obtained by initially adding 1.00 mol of H₂, 2.00 mol of CO₂, 0.750 mol of H₂O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

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Correct Answer
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Consider the two gaseous equilibria: SO₂(g) + ¹/₂O₂(g) SO₃(g) K₁ 2SO₃(g) SO₂(g) + O₂(g) K₂ The values of the equilibrium constants K₁ and K₂are related by

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Correct Answer
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A catalyst affects both the fo...
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Hydrogen iodide decomposes according to the equation: 2HI(g) H₂(g)+ I₂(g), K_c = 0.0156 at 400ºC A 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC. Calculate the concentration of H₂ equilibrium.

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Consider the chemical reaction 2NH₃(g) N₂(g)+ 3H₂(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g)are present. Estimate the equilibrium concentration of N₂(g).

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Consider the chemical reaction 2NH₃(g) N₂(g)+ 3H₂(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g)are present. Estimate the equilibrium concentration of H₂(g).

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On analysis, an equilibrium mixture for the reaction 2H₂S(g) 2H₂(g) + S₂(g) was found to contain 1.0 mol H₂S, 4.0 mol H₂, and 0.80 mol S₂ in a 4.0 L vessel. Calculate the equilibrium constant, K_c, for this reaction.

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Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the reactants would increase, decrease, or remain constant after nitrogen gas was removed from the system.

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