Question 1

For the reaction PCl3(g) + Cl2(g)  3(g) + Cl2(g)    PCl5(g) at a particular temperature,Kc = 32.4.Suppose a system at that temperature is prepared with [PCl5] = 0.50 M,[Cl2] = 0.4 M,and [PCl3] = 0.10M.Which of the following is correct? A) The system will proceed in the direction of forming more PCl5 and Cl2 until equilibrium is reached. B) The system is at equilibrium. C) The system will proceed in the direction of forming more PCl5 until equilibrium is reached. D) The system will proceed in the direction of forming more PCl3 and Cl2 until equilibrium is reached. E) The system will proceed in the direction of forming more PCl3 and PCl5 until equilibrium is reached." class="answers-bank-image d-inline" rel="preload" > PCl5(g) at a particular temperature,Kc = 32.4.Suppose a system at that temperature is prepared with [PCl5] = 0.50 M,[Cl2] = 0.4 M,and [PCl3] = 0.10M.Which of the following is correct?

Accepted Answer

A)  The system will proceed in the direction of forming more PCl5 and Cl2 until equilibrium is reached.
B)  The system is at equilibrium.
C)  The system will proceed in the direction of forming more PCl5 until equilibrium is reached.
D)  The system will proceed in the direction of forming more PCl3 and Cl2 until equilibrium is reached.
E)  The system will proceed in the direction of forming more PCl3 and PCl5 until equilibrium is reached.F) A) and E)
G) A) and C)

Question 2

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)  
E)  2H2O2 (g)    2H2O(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > CO2(g) + H2(g) 
B)  2NO(g) + Cl2(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)  
E)  2H2O2 (g)    2H2O(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > 2NOCl(g) 
C)  2SO3(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)  
E)  2H2O2 (g)    2H2O(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > 2SO2(g) + O2(g) 
D)  PCl5(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)  
E)  2H2O2 (g)    2H2O(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > PCl3(g) + Cl2(g) 
E)  2H2O2 (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)  
E)  2H2O2 (g)    2H2O(g) + O2(g) " class="answers-bank-image d-inline" rel="preload" > 2H2O(g) + O2(g) F) A) and B)
G) D) and E)

Question 3

Hydrogen peroxide (H2O2) decomposes according to the following equation. H2O2(l) → H2O(l) + ½O2(g) .
What is KP for this reaction at 25°C? (ΔH° = -98.2 kJ/mol,ΔS° = 70.1 J/K • mol,R = 8.314 J/K• mol)

Accepted Answer

A)  1.3 × 10-21
B)  20.9
C)  3.46 × 1017
D)  7.4 × 1020
E)  8.6 × 104F) A) and B)
G) A) and E)

Question 4

What is defined as a fraction with product concentrations in the numerator and reactant concentrations in the denominator and with 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)  Reaction quotient
E)  Mass actionF) A) and C)
G) A) and B)

Question 5

The following reactions occur at 500 K.Arrange them in order of increasing tendency to proceed to completion (least completion → greatest completion) . 1 2NOCl 2 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 2 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  2NO2 KP = 1.5 × 103
3 2SO3 2 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  2SO2 + O2 KP = 1.3 × 10 -5
4 2NO2 2 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 + O2 KP = 5.9 × 10 -5

Accepted Answer

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

Question 6

Hydrogen iodide decomposes according to the equation 2HI(g)  2(g) + I2(g) ,for which Kc = 0.0156 at 400ºC.Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of H2 at equilibrium? A) 0.275 M B) 0.138 M C) 0.0275 M D) 0.0550 M E) 0.220 M" class="answers-bank-image d-inline" rel="preload" > H2(g) + I2(g) ,for which Kc = 0.0156 at 400ºC.Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of H2 at equilibrium?

Accepted Answer

A)  0.275 M
B)  0.138 M
C)  0.0275 M
D)  0.0550 M
E)  0.220 MF) A) and D)
G) B) and C)

Question 7

When a reaction reaches _________,the concentration of the reactants and products will no longer change.

Accepted Answer

The answer of When a reaction reaches _________,the concentration of...

Question 8

At 500°C the equilibrium constant,KP ,is 4.00 ×10-4 for the equilibrium: 2HCN(g)  P ,is 4.00 ×10-4 for the equilibrium: 2HCN(g)    H2(g) + C2N2(g)  What is Kp for the following reaction? H2(g) + C2 N2(g)    2HCN(g)  A) 2.00 × 10-4 B) -4.00 × 10-4 C) 1.25 × 103 D) 2.50 × 103 E) 4.00 × 104" class="answers-bank-image d-inline" rel="preload" > H2(g) + C2N2(g) 
What is Kp for the following reaction?
H2(g) + C2 N2(g)  P ,is 4.00 ×10-4 for the equilibrium: 2HCN(g)    H2(g) + C2N2(g)  What is Kp for the following reaction? H2(g) + C2 N2(g)    2HCN(g)  A) 2.00 × 10-4 B) -4.00 × 10-4 C) 1.25 × 103 D) 2.50 × 103 E) 4.00 × 104" class="answers-bank-image d-inline" rel="preload" > 2HCN(g)

Accepted Answer

A)  2.00 × 10-4
B)  -4.00 × 10-4
C)  1.25 × 103
D)  2.50 × 103
E)  4.00 × 104F) B) and E)
G) B) and C)

Question 9

Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position,regardless of the physical state of the substance involved.

Accepted Answer

A) True 
 B)False

Question 10

Hydrogen iodide decomposes according to the equation 2HI(g)  2(g) + I2(g) ,for which Kc = 0.0156 at 400ºC.Suppose 0.550 mol HI is injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of HI at equilibrium? A) 0.138 M B) 0.220 M C) 0.550 M D) 0.275 M E) 0.0275 M" class="answers-bank-image d-inline" rel="preload" > H2(g) + I2(g) ,for which Kc = 0.0156 at 400ºC.Suppose 0.550 mol HI is injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of HI at equilibrium?

Accepted Answer

A)  0.138 M
B)  0.220 M
C)  0.550 M
D)  0.275 M
E)  0.0275 MF) D) and E)
G) C) and E)

Question 11

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g)  2(g) .What is KP for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol.(R = 8.314 J/K • mol)  A) 1.60 × 10-2 B) 2.10 × 10-7 C) 62.8 D) 4.90 × 106 E) 3.20 × 109" class="answers-bank-image d-inline" rel="preload" > 2NO(g) + Cl2(g) .What is KP for this reaction at 227°C?
For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol.(R = 8.314 J/K • mol)

Accepted Answer

A)  1.60 × 10-2
B)  2.10 × 10-7
C)  62.8
D)  4.90 × 106
E)  3.20 × 109F) None of the above
G) A) and B)

Question 12

There are guidelines to help write equilibrium constants.

Accepted Answer

A) True 
 B)False

Question 13

The reaction system POBr3(g)  3(g)    POBr(g) + Br2(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container? A) POBr will be consumed in order to establish a new equilibrium. B) The partial pressures of POBr3 and POBr will remain steady while the partial pressure of bromine increases. C) The partial pressure of bromine will increase while the partial pressure of POBr decreases. D) The partial pressure of bromine remains steady while the partial pressures of POBr3 and POBr increase. E) The forward reaction will proceed to establish equilibrium." class="answers-bank-image d-inline" rel="preload" > POBr(g) + Br2(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?

Accepted Answer

A)  POBr will be consumed in order to establish a new equilibrium.
B)  The partial pressures of POBr3 and POBr will remain steady while the partial pressure of bromine increases.
C)  The partial pressure of bromine will increase while the partial pressure of POBr decreases.
D)  The partial pressure of bromine remains steady while the partial pressures of POBr3 and POBr increase.
E)  The forward reaction will proceed to establish equilibrium.F) A) and E)
G) C) and E)

Question 14

When the following reaction is at equilibrium,which relationship is always true? 2NOCl(g)  2(g)  A) [NO] [Cl2] = [NOCl] B) [NO]2 [Cl2] = [NOCl]2 C) [NOCl] = [NO] D) 2[NO] = [Cl2] E) [NO]2 [Cl2] = Kc [NOCl]2" class="answers-bank-image d-inline" rel="preload" > 2NO(g) + Cl2(g)

Accepted Answer

A)  [NO] [Cl2] = [NOCl]
B)  [NO]2 [Cl2] = [NOCl]2
C)  [NOCl] = [NO]
D)  2[NO] = [Cl2]
E)  [NO]2 [Cl2] = Kc [NOCl]2F) All of the above
G) C) and D)

Question 15

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g) + O2(g)  2(g) + O2(g)    2NO(g)  The equilibrium constant KP for the reaction is 0.0025 at 2127°C.If a container is charged with 8) 00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, What will be the equilibrium partial pressure of nitrogen? A) 0.15 atm B) 0.31 atm C) 3.08 atm D) 7.69 atm E) 7.85 atm" class="answers-bank-image d-inline" rel="preload" > 2NO(g) 
The equilibrium constant KP for the reaction is 0.0025 at 2127°C.If a container is charged with
8) 00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium,
What will be the equilibrium partial pressure of nitrogen?

Accepted Answer

A)  0.15 atm
B)  0.31 atm
C)  3.08 atm
D)  7.69 atm
E)  7.85 atmF) All of the above
G) A) and B)

Question 16

For _______-________ reactions KP = Kc (RT)Δn gas.

Accepted Answer

Question 17

Which equation is correct?

Accepted Answer

A)  ΔG = ΔG° - RT logKeq
B)  ΔG = ΔG° + RT lnQ
C)  ΔG = RT lnQ
D)  ΔG = -RT logQ
E)  ΔG = -RT logKeqF) D) and E)
G) A) and C)

Question 18

For the reaction H2(g) + Br2(g)  2(g) + Br2(g)    2HBr(g) ,Kc = 81.4 at 385ºC.If [H2] = [Br2] = [HBr] = 2.4 × 10-4M at 385ºC,which one of the following is correct? A) [H2] and [HBr] decrease as the system moves toward equilibrium. B) The system is at equilibrium. C) [H2] and [Br2] increase as the system approaches equilibrium. D) [HBr] increases as the system approaches equilibrium. E) [HBr] and [Br2] increases as the system approaches equilibrium." class="answers-bank-image d-inline" rel="preload" > 2HBr(g) ,Kc = 81.4 at 385ºC.If [H2] = [Br2] = [HBr] = 2.4 × 10-4M at 385ºC,which one of the following is correct?

Accepted Answer

A)  [H2] and [HBr] decrease as the system moves toward equilibrium.
B)  The system is at equilibrium.
C)  [H2] and [Br2] increase as the system approaches equilibrium.
D)  [HBr] increases as the system approaches equilibrium.
E)  [HBr] and [Br2] increases as the system approaches equilibrium.F) A) and E)
G) C) and D)

Question 19

At elevated temperatures,hydrogen iodide may decompose to form hydrogen gas and iodine gas,as follows. 2HI(g)  2(g) + I2(g)  In a particular experiment,the concentrations at equilibrium were measured to be [HI] = 0.85 Mol/L,[I2] = 0.60 mol/L,and [H2] = 0.27 mol/L.What is Kc for the above reaction? A) 5.3 B) 0.22 C) 4.5 D) 0.19 E) 1.6 × 102" class="answers-bank-image d-inline" rel="preload" > H2(g) + I2(g) 
In a particular experiment,the concentrations at equilibrium were measured to be [HI] = 0.85
Mol/L,[I2] = 0.60 mol/L,and [H2] = 0.27 mol/L.What is Kc for the above reaction?

Accepted Answer

A)  5.3
B)  0.22
C)  4.5
D)  0.19
E)  1.6 × 102F) None of the above
G) A) and D)

Question 20

In the gas phase,methyl isonitrile (CH3NC) isomerizes to acetonitrile (CH3CN) , H3C-N≡C(g)  3NC) isomerizes to acetonitrile (CH3CN) , H3C-N≡C(g)    H3C-C≡N(g) with ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C.Find the equilibrium constant for this reaction at 100°C. A) 1.68 × 10-10 B) 5.96 × 109 C) 2.16 × 1010 D) 4.63 × 10-11 E) 8.64 × 1012" class="answers-bank-image d-inline" rel="preload" > H3C-C≡N(g) with ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C.Find the equilibrium constant for this reaction at 100°C.

Accepted Answer

A)  1.68 × 10-10
B)  5.96 × 109
C)  2.16 × 1010
D)  4.63 × 10-11
E)  8.64 × 1012F) C) and D)
G) All of the above

Exam 15: Chemical Equilibrium

Correct Answer
verified

When a reaction reaches _________,the concentration of the reactants and products will no longer change.

Correct Answer
verified

Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position,regardless of the physical state of the substance involved.

Correct Answer
verified

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g) + Cl₂(g) .What is K_P for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol.(R = 8.314 J/K • mol)

Correct Answer
verified

For _-__ reactions K_P = K_c (RT)^Δⁿ gas.

Correct Answer
verified

Correct Answer
verified

For the reaction H₂(g) + Br₂(g) 2HBr(g) ,K_c = 81.4 at 385ºC.If [H₂] = [Br₂] = [HBr] = 2.4 × 10^-4M at 385ºC,which one of the following is correct?

Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + I₂(g) ,for which K_c = 0.0156 at 400ºC.Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of H₂ at equilibrium?

Correct Answer
verified

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

Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + I₂(g) ,for which K_c = 0.0156 at 400ºC.Suppose 0.550 mol HI is injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of HI at equilibrium?

Correct Answer
verified

Which equation is correct?

Correct Answer
verified

There are guidelines to help write equilibrium constants.

Correct Answer
verified

For the reaction PCl₃(g) + Cl₂(g) PCl₅(g) at a particular temperature,K_c = 32.4.Suppose a system at that temperature is prepared with [PCl₅] = 0.50 M,[Cl₂] = 0.4 M,and [PCl₃] = 0.10M.Which of the following is correct?

Correct Answer
verified

Correct Answer
verified

At 500°C the equilibrium constant,K_P ,is 4.00 ×10^-4 for the equilibrium: 2HCN(g) H₂(g) + C₂N₂(g) What is K_p for the following reaction? H₂(g) + C₂ N₂(g) 2HCN(g)

Correct Answer
verified

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

Correct Answer
verified

The reaction system POBr₃(g) POBr(g) + Br₂(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?

Correct Answer
verified

When the following reaction is at equilibrium,which relationship is always true? 2NOCl(g) 2NO(g) + Cl₂(g)

Correct Answer
verified

Hydrogen peroxide (H2O2) decomposes according to the following equation. H₂O₂(l) → H₂O(l) + ½O₂(g) . What is K_P for this reaction at 25°C? (ΔH° = -98.2 kJ/mol,ΔS° = 70.1 J/K • mol,R = 8.314 J/K• mol)

Correct Answer
verified

In the gas phase,methyl isonitrile (CH₃NC) isomerizes to acetonitrile (CH₃CN) , H₃C-N≡C(g) H₃C-C≡N(g) with ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C.Find the equilibrium constant for this reaction at 100°C.

Correct Answer
verified

Exam 15: Chemical Equilibrium

At elevated temperatures,hydrogen iodide may decompose to form hydrogen gas and iodine gas,as follows. 2HI(g) H2(g) + I2(g) In a particular experiment,the concentrations at equilibrium were measured to be [HI] = 0.85 Mol/L,[I2] = 0.60 mol/L,and [H2] = 0.27 mol/L.What is Kc for the above reaction?

Correct AnswerverifiedShow Answer

When a reaction reaches _________,the concentration of the reactants and products will no longer change.

Correct AnswerverifiedShow Answer

Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position,regardless of the physical state of the substance involved.

Correct AnswerverifiedShow Answer

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g) + Cl2(g) .What is KP for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol.(R = 8.314 J/K • mol)

Correct AnswerverifiedShow Answer

For _______-________ reactions KP = Kc (RT)Δn gas.

Correct AnswerverifiedShow Answer

The following reactions occur at 500 K.Arrange them in order of increasing tendency to proceed to completion (least completion → 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

Correct AnswerverifiedShow Answer

For the reaction H2(g) + Br2(g) 2HBr(g) ,Kc = 81.4 at 385ºC.If [H2] = [Br2] = [HBr] = 2.4 × 10-4M at 385ºC,which one of the following is correct?

Correct AnswerverifiedShow Answer

Hydrogen iodide decomposes according to the equation 2HI(g) H2(g) + I2(g) ,for which Kc = 0.0156 at 400ºC.Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of H2 at equilibrium?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Hydrogen iodide decomposes according to the equation 2HI(g) H2(g) + I2(g) ,for which Kc = 0.0156 at 400ºC.Suppose 0.550 mol HI is injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of HI at equilibrium?

Correct AnswerverifiedShow Answer

Which equation is correct?

Correct AnswerverifiedShow Answer

There are guidelines to help write equilibrium constants.

Correct AnswerverifiedShow Answer

For the reaction PCl3(g) + Cl2(g) PCl5(g) at a particular temperature,Kc = 32.4.Suppose a system at that temperature is prepared with [PCl5] = 0.50 M,[Cl2] = 0.4 M,and [PCl3] = 0.10M.Which of the following is correct?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

At 500°C the equilibrium constant,KP ,is 4.00 ×10-4 for the equilibrium: 2HCN(g) H2(g) + C2N2(g) What is Kp for the following reaction? H2(g) + C2 N2(g) 2HCN(g)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

The reaction system POBr3(g) POBr(g) + Br2(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?

Correct AnswerverifiedShow Answer

When the following reaction is at equilibrium,which relationship is always true? 2NOCl(g) 2NO(g) + Cl2(g)

Correct AnswerverifiedShow Answer

Hydrogen peroxide (H2O2) decomposes according to the following equation. H2O2(l) → H2O(l) + ½O2(g) . What is KP for this reaction at 25°C? (ΔH° = -98.2 kJ/mol,ΔS° = 70.1 J/K • mol,R = 8.314 J/K• mol)

Correct AnswerverifiedShow Answer

In the gas phase,methyl isonitrile (CH3NC) isomerizes to acetonitrile (CH3CN) , H3C-N≡C(g) H3C-C≡N(g) with ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C.Find the equilibrium constant for this reaction at 100°C.

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Nitrosyl chloride (NOCl) decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g) + Cl₂(g) .What is K_P for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol.(R = 8.314 J/K • mol)

Correct Answer
verified

For _-__ reactions K_P = K_c (RT)^Δⁿ gas.

Correct Answer
verified

Correct Answer
verified

For the reaction H₂(g) + Br₂(g) 2HBr(g) ,K_c = 81.4 at 385ºC.If [H₂] = [Br₂] = [HBr] = 2.4 × 10^-4M at 385ºC,which one of the following is correct?

Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + I₂(g) ,for which K_c = 0.0156 at 400ºC.Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of H₂ at equilibrium?

Correct Answer
verified

Correct Answer
verified

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + I₂(g) ,for which K_c = 0.0156 at 400ºC.Suppose 0.550 mol HI is injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of HI at equilibrium?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

For the reaction PCl₃(g) + Cl₂(g) PCl₅(g) at a particular temperature,K_c = 32.4.Suppose a system at that temperature is prepared with [PCl₅] = 0.50 M,[Cl₂] = 0.4 M,and [PCl₃] = 0.10M.Which of the following is correct?

Correct Answer
verified

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At 500°C the equilibrium constant,K_P ,is 4.00 ×10^-4 for the equilibrium: 2HCN(g) H₂(g) + C₂N₂(g) What is K_p for the following reaction? H₂(g) + C₂ N₂(g) 2HCN(g)

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The reaction system POBr₃(g) POBr(g) + Br₂(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?

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When the following reaction is at equilibrium,which relationship is always true? 2NOCl(g) 2NO(g) + Cl₂(g)

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Hydrogen peroxide (H2O2) decomposes according to the following equation. H₂O₂(l) → H₂O(l) + ½O₂(g) . What is K_P for this reaction at 25°C? (ΔH° = -98.2 kJ/mol,ΔS° = 70.1 J/K • mol,R = 8.314 J/K• mol)

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In the gas phase,methyl isonitrile (CH₃NC) isomerizes to acetonitrile (CH₃CN) , H₃C-N≡C(g) H₃C-C≡N(g) with ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C.Find the equilibrium constant for this reaction at 100°C.

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