Question 1

Kc is 1.67 × 1020 at 25 °C for the formation of iron(III) oxalate complex ion:
Fe3+(aq) + 3C2O42-(aq) ⇌ [Fe(C2O4) 3]3-(aq) 
If 0.0200 mol L-1 Fe3+ is initially mixed with 1.00 mol L-1 oxalate ion,what is the concentration of Fe3+ ion at equilibrium?

Accepted Answer

A)  1.44 × 10-22 mol L-1
B)  0.0100 mol L-1
C)  8.35 × 1019 mol L-1
D)  6.94 × 1021 mol L-1

Question 2

Equilibrium reactions are noted by a single straight arrow for a yield sign.

Accepted Answer

A) True 
 B)False

Question 3

Which of the following equilibrium constants-reaction types is INCORRECT?

Accepted Answer

A)  1.4 × 1083 equilibrium reaction-goes to completion.
B)  1.6 × 10-23 equilibrium reaction-does not occur.
C)  1.8 × 10-5 equilibrium reaction-more reactants than products at equilibrium.
D)  1.0 equilibrium reaction-equal amounts of products and reactants.
E)  3.2 × 103 equilibrium reaction-more reactants than products at equilibrium.

Question 4

The equilibrium constant,Kp,equals 3.40 for the isomerization reaction:
Cis-2-butene ⇌ trans-2-butene
If a flask initially contains 0.250 bar of cis-2-butene and 0.165 bar of trans-2-butene,what is the equilibrium pressure of each gas?

Accepted Answer

A)  P(cis-2-butene) = 0.0485 bar and P(trans-2-butene) = 0.165 bar
B)  P(cis-2-butene) = 0.0458 bar and P(trans-2-butene) = 0.156 bar
C)  P(cis-2-butene) = 0.0735 bar and P(trans-2-butene) = 0.250 bar
D)  P(cis-2-butene) = 0.0943 bar and P(trans-2-butene) = 0.321 bar

Question 5

Consider the following reaction occurring at 960 K:
CO2(g) + H2(g) ⇌ CO(g) + H2O(g) 
At equilibrium,the concentrations of reactants and products are: [CO2] = 0.0400 M,[H2] = 0.0220 M,[CO] = 0.0240 M,and [H2O] = 0.0190 M.This equilibrium is perturbed by adding CO2(g) to the system such that when a new equilibrium is reached,the concentration of CO2 is 0.050 M.What is the concentration of H2(g) at this equilibrium?

Accepted Answer

A)  0.050 M
B)  0.482 M
C)  0.462 M
D)  0.300 M
E)  0.0504 M

Question 6

For the reaction:
3 Fe(s) + 4 H2O(g) ⇌ Fe3O4(s) + 4 H2(g) 
Write the expression for Kp.

Accepted Answer

A)   2O(g) ⇌ Fe3O4(s) + 4 H2(g)  Write the expression for Kp. 
A)     
B)     
C)     
D)     
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B)   2O(g) ⇌ Fe3O4(s) + 4 H2(g)  Write the expression for Kp. 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2O(g) ⇌ Fe3O4(s) + 4 H2(g)  Write the expression for Kp. 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2O(g) ⇌ Fe3O4(s) + 4 H2(g)  Write the expression for Kp. 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2O(g) ⇌ Fe3O4(s) + 4 H2(g)  Write the expression for Kp. 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 7

Consider the reaction:
2 SO2(g) + O2(g) ⇌ 2 SO3(g) ,ΔrH° = -196.6 kJ/mol
The equilibrium is displaced to the left if:

Accepted Answer

A)  some sulfur trioxide is removed
B)  the temperature is raised
C)  some sulfur dioxide is added
D)  the pressure is raised
E)  the temperature is lowered

Question 8

Write the equilibrium constant expression for the reaction:
3 Sn(s) + 4 HNO3(aq) + H2O(l) ⇌ 3 H2SnO3(s) + 4 NO(g)

Accepted Answer

A)  Kc = 3(aq) + H2O(l) ⇌ 3 H2SnO3(s) + 4 NO(g)  
A)  Kc =   
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >
B)  Kc = 3(aq) + H2O(l) ⇌ 3 H2SnO3(s) + 4 NO(g)  
A)  Kc =   
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >
C)  Kc = 3(aq) + H2O(l) ⇌ 3 H2SnO3(s) + 4 NO(g)  
A)  Kc =   
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >
D)  Kc = 3(aq) + H2O(l) ⇌ 3 H2SnO3(s) + 4 NO(g)  
A)  Kc =   
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >
E)  Kc = 3(aq) + H2O(l) ⇌ 3 H2SnO3(s) + 4 NO(g)  
A)  Kc =   
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" > B

Question 9

At a certain temperature the equilibrium constant,Kc,equals 0.11 for the reaction:
2 ICl(g) ⇌ I2(g) + Cl2(g) 
What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0 L flask?

Accepted Answer

A)  0.14 mol L-1
B)  0.17 mol L-1
C)  0.27 mol L-1
D)  0.34 mol L-1

Question 10

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25 °C and ΔrH° = 58.03 kJ/mol.Assume that 1 mole of N2O4 and 2 moles of NO2 are introduced into a 5.0 liter container.What will be the equilibrium value of [N2O]?

Accepted Answer

A)  0.928 M
B)  0.0822 M
C)  0.358 M
D)  0.379 M
E)  0.042 M

Question 11

Consider the following reaction:
POCl3(g) ⇌ POCl(g) + Cl2(g) with Kc = 0.450
A sample of pure POCl3(g) was placed in a reaction vessel and allowed to decompose according to the above reaction.At equilibrium,the concentrations of POCl(g) and Cl2(g) were each 0.150 M.What was the initial concentration of POCl3(g) ?

Accepted Answer

A)  0.225 M
B)  0.200 M
C)  0.633 M
D)  0.483 M
E)  0.350 M B

Question 12

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25 °C and ΔrH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N2O4 was present inside the container,compute 2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25 °C and ΔrH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N2O4 was present inside the container,compute   At equilibrium. A) 0.398 atm B) 0.113 atm C) 0.602 atm D) 0.285 atm E) 0.715 atm" class="answers-bank-image d-inline" rel="preload" >
At equilibrium.

Accepted Answer

A)  0.398 atm
B)  0.113 atm
C)  0.602 atm
D)  0.285 atm
E)  0.715 atm

Question 13

Consider the following hypothetical equilibrium reaction:
A2(g) + B2(g) ⇌ 2 AB(g)  where Kc = 2(g) + B2(g) ⇌ 2 AB(g)  where Kc =   The equilibrium constant for the reaction: 2 A2(g) + 2 B2(g) ⇌ 4 AB(g) is ________. A)    B) Kc4  C)      D)    E) Kc2 " class="answers-bank-image d-inline" rel="preload" >
The equilibrium constant for the reaction: 2 A2(g) + 2 B2(g) ⇌ 4 AB(g) is ________.

Accepted Answer

A)   2(g) + B2(g) ⇌ 2 AB(g)  where Kc =   The equilibrium constant for the reaction: 2 A2(g) + 2 B2(g) ⇌ 4 AB(g) is ________. 
A)     
B)  Kc4  
C)       
D)     
E)  Kc2 " class="answers-bank-image d-inline" rel="preload" >
B)  Kc4 
C)   2(g) + B2(g) ⇌ 2 AB(g)  where Kc =   The equilibrium constant for the reaction: 2 A2(g) + 2 B2(g) ⇌ 4 AB(g) is ________. 
A)     
B)  Kc4  
C)       
D)     
E)  Kc2 " class="answers-bank-image d-inline" rel="preload" >  
D)   2(g) + B2(g) ⇌ 2 AB(g)  where Kc =   The equilibrium constant for the reaction: 2 A2(g) + 2 B2(g) ⇌ 4 AB(g) is ________. 
A)     
B)  Kc4  
C)       
D)     
E)  Kc2 " class="answers-bank-image d-inline" rel="preload" >
E)  Kc2  E

Question 14

In a system in equilibrium,two opposing reactions occur at equal rates.

Accepted Answer

A) True 
 B)False

Question 15

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25 °C and ΔrH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N2O4 was present inside the container,compute 2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25 °C and ΔrH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N2O4 was present inside the container,compute   At equilibrium.  A) 7.98 atm B) 8.88 atm C) 1.12 atm D) 1.01 atm E) 8.99 atm" class="answers-bank-image d-inline" rel="preload" >
At equilibrium.

Accepted Answer

A)  7.98 atm
B)  8.88 atm
C)  1.12 atm
D)  1.01 atm
E)  8.99 atm

Question 16

For the following chemical equilibrium,Kp = 4.6 × 10-14 at 25 °C,find the value of Kc for this reaction at 25 °C.
2 Cl2(g) + 2 H2O(g) ⇌ 4 HCl(g) + O2(g)

Accepted Answer

A)  Kc = 1.9 × 10-15 
B)  Kc = 2.2 × 10-14 
C)  Kc = 1.1 × 10-12 
D)  Kc = 9.4 × 10-14 
E)  Kc = 4.6 × 10-14

Question 17

For the reaction CO(g) + 3 H2(g) ⇌ H2O(g) + CH4(g) ,Kc = 190 at 1000 K.If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025 M,[H2] = 0.045 M,[H2O] = 0.025,M and [CH4] = 0.046 M,in which direction will a reaction occur and why?

Accepted Answer

A)  toward products because Qc = 0.17
B)  toward reactants because Qc = 0.0029
C)  toward products because Qc = 0.35
D)  toward reactants because Qc = 505
E)  it is at equilibrium because Qc = 1

Question 18

Choose the INCORRECT statement.

Accepted Answer

A)  A certain amount of energy,called the activation energy,must be available if a reaction is to take place.
B)  A reversible chemical reaction is one in which equilibrium is never established due to the constant decomposition of the products.
C)  When the rate of the reverse reaction equals the rate of the forward reaction,equilibrium has been established.
D)  Changes in temperature will change the value of an equilibrium constant.
E)  Chemical equilibrium is a dynamic equilibrium.

Question 19

For the reaction CO(g) + 3 H2(g) ⇌ H2O(g) + CH4(g) ,Kc = 190 at 1000 K.If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M,[H2] = 0.045 M,[H2O] = 0.020,M and [CH4] = 0.031 M,in which direction will a reaction occur and why?

Accepted Answer

A)  toward products because Qc = 0.38
B)  toward reactants because Qc = 0.24
C)  toward products because Qc = 4.1
D)  toward reactants because Qc = 61
E)  it is at equilibrium because Qc = 190

Question 20

Write the equilibrium constant expression for the following reaction:
2 KI(aq) + H2O2(aq) ⇌ 2 KOH(aq) + I2(aq)

Accepted Answer

A)  Kc = 2O2(aq) ⇌ 2 KOH(aq) + I2(aq)  
A)  Kc =   
B)  Kc = [I2] 
C)  Kc = [I2]2  
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >
B)  Kc = [I2]
C)  Kc = [I2]2 
D)  Kc = 2O2(aq) ⇌ 2 KOH(aq) + I2(aq)  
A)  Kc =   
B)  Kc = [I2] 
C)  Kc = [I2]2  
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >
E)  Kc = 2O2(aq) ⇌ 2 KOH(aq) + I2(aq)  
A)  Kc =   
B)  Kc = [I2] 
C)  Kc = [I2]2  
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >

Exam 15: Principles of Chemical Equilibrium

K_c is 1.67 × 10²⁰ at 25 °C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3C₂O₄^2-(aq) ⇌ [Fe(C₂O₄) ₃]^3-(aq) If 0.0200 mol L^-1 Fe³⁺ is initially mixed with 1.00 mol L^-1 oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

Correct Answer
verified

Equilibrium reactions are noted by a single straight arrow for a yield sign.

Correct Answer
verified

Which of the following equilibrium constants-reaction types is INCORRECT?

Correct Answer
verified

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene If a flask initially contains 0.250 bar of cis-2-butene and 0.165 bar of trans-2-butene,what is the equilibrium pressure of each gas?

Correct Answer
verified

Correct Answer
verified

For the reaction: 3 Fe(s) + 4 H₂O(g) ⇌ Fe₃O₄(s) + 4 H₂(g) Write the expression for Kp.

Correct Answer
verified

Consider the reaction: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) ,Δ_rH° = -196.6 kJ/mol The equilibrium is displaced to the left if:

Correct Answer
verified

Write the equilibrium constant expression for the reaction: 3 Sn(s) + 4 HNO₃(aq) + H₂O(l) ⇌ 3 H₂SnO₃(s) + 4 NO(g)

Correct Answer
verified
B

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: 2 ICl(g) ⇌ I₂(g) + Cl₂(g) What is the equilibrium concentration of ICl if 0.45 mol of I₂ and 0.45 mol of Cl₂ are initially mixed in a 2.0 L flask?

Correct Answer
verified

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which K_p = 0.1134 at 25 °C and Δ_rH° = 58.03 kJ/mol.Assume that 1 mole of N₂O₄ and 2 moles of NO₂ are introduced into a 5.0 liter container.What will be the equilibrium value of [N₂O]?

Correct Answer
verified

Correct Answer
verified
B

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which K_p = 0.1134 at 25 °C and Δ_rH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N₂O₄ was present inside the container,compute At equilibrium.

Correct Answer
verified

Consider the following hypothetical equilibrium reaction: A₂(g) + B₂(g) ⇌ 2 AB(g) where K_c = The equilibrium constant for the reaction: 2 A₂(g) + 2 B₂(g) ⇌ 4 AB(g) is ________.

Correct Answer
verified
E

In a system in equilibrium,two opposing reactions occur at equal rates.

Correct Answer
verified

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which K_p = 0.1134 at 25 °C and Δ_rH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N₂O₄ was present inside the container,compute At equilibrium.

Correct Answer
verified

For the following chemical equilibrium,K_p = 4.6 × 10^-14 at 25 °C,find the value of K_c for this reaction at 25 °C. 2 Cl₂(g) + 2 H₂O(g) ⇌ 4 HCl(g) + O₂(g)

Correct Answer
verified

For the reaction CO(g) + 3 H₂(g) ⇌ H₂O(g) + CH₄(g) ,K_c = 190 at 1000 K.If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025 M,[H₂] = 0.045 M,[H₂O] = 0.025,M and [CH₄] = 0.046 M,in which direction will a reaction occur and why?

Correct Answer
verified

Choose the INCORRECT statement.

Correct Answer
verified

For the reaction CO(g) + 3 H₂(g) ⇌ H₂O(g) + CH₄(g) ,K_c = 190 at 1000 K.If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M,[H₂] = 0.045 M,[H₂O] = 0.020,M and [CH₄] = 0.031 M,in which direction will a reaction occur and why?

Correct Answer
verified

Write the equilibrium constant expression for the following reaction: 2 KI(aq) + H₂O₂(aq) ⇌ 2 KOH(aq) + I₂(aq)

Correct Answer
verified

Exam 15: Principles of Chemical Equilibrium

Kc is 1.67 × 1020 at 25 °C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3C2O42-(aq) ⇌ [Fe(C2O4) 3]3-(aq) If 0.0200 mol L-1 Fe3+ is initially mixed with 1.00 mol L-1 oxalate ion,what is the concentration of Fe3+ ion at equilibrium?

Correct AnswerverifiedShow Answer

Equilibrium reactions are noted by a single straight arrow for a yield sign.

Correct AnswerverifiedShow Answer

Which of the following equilibrium constants-reaction types is INCORRECT?

Correct AnswerverifiedShow Answer

The equilibrium constant,Kp,equals 3.40 for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene If a flask initially contains 0.250 bar of cis-2-butene and 0.165 bar of trans-2-butene,what is the equilibrium pressure of each gas?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

For the reaction: 3 Fe(s) + 4 H2O(g) ⇌ Fe3O4(s) + 4 H2(g) Write the expression for Kp.

Correct AnswerverifiedShow Answer

Consider the reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) ,ΔrH° = -196.6 kJ/mol The equilibrium is displaced to the left if:

Correct AnswerverifiedShow Answer

Write the equilibrium constant expression for the reaction: 3 Sn(s) + 4 HNO3(aq) + H2O(l) ⇌ 3 H2SnO3(s) + 4 NO(g)

Correct AnswerverifiedB

At a certain temperature the equilibrium constant,Kc,equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g) What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0 L flask?

Correct AnswerverifiedShow Answer

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25 °C and ΔrH° = 58.03 kJ/mol.Assume that 1 mole of N2O4 and 2 moles of NO2 are introduced into a 5.0 liter container.What will be the equilibrium value of [N2O]?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedB

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25 °C and ΔrH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N2O4 was present inside the container,compute At equilibrium.

Correct AnswerverifiedShow Answer

Consider the following hypothetical equilibrium reaction: A2(g) + B2(g) ⇌ 2 AB(g) where Kc = The equilibrium constant for the reaction: 2 A2(g) + 2 B2(g) ⇌ 4 AB(g) is ________.

Correct AnswerverifiedE

In a system in equilibrium,two opposing reactions occur at equal rates.

Correct AnswerverifiedShow Answer

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25 °C and ΔrH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N2O4 was present inside the container,compute At equilibrium.

Correct AnswerverifiedShow Answer

For the following chemical equilibrium,Kp = 4.6 × 10-14 at 25 °C,find the value of Kc for this reaction at 25 °C. 2 Cl2(g) + 2 H2O(g) ⇌ 4 HCl(g) + O2(g)

Correct AnswerverifiedShow Answer

For the reaction CO(g) + 3 H2(g) ⇌ H2O(g) + CH4(g) ,Kc = 190 at 1000 K.If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025 M,[H2] = 0.045 M,[H2O] = 0.025,M and [CH4] = 0.046 M,in which direction will a reaction occur and why?

Correct AnswerverifiedShow Answer

Choose the INCORRECT statement.

Correct AnswerverifiedShow Answer

For the reaction CO(g) + 3 H2(g) ⇌ H2O(g) + CH4(g) ,Kc = 190 at 1000 K.If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M,[H2] = 0.045 M,[H2O] = 0.020,M and [CH4] = 0.031 M,in which direction will a reaction occur and why?

Correct AnswerverifiedShow Answer

Write the equilibrium constant expression for the following reaction: 2 KI(aq) + H2O2(aq) ⇌ 2 KOH(aq) + I2(aq)

Correct AnswerverifiedShow Answer

K_c is 1.67 × 10²⁰ at 25 °C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3C₂O₄^2-(aq) ⇌ [Fe(C₂O₄) ₃]^3-(aq) If 0.0200 mol L^-1 Fe³⁺ is initially mixed with 1.00 mol L^-1 oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: Cis-2-butene ⇌ trans-2-butene If a flask initially contains 0.250 bar of cis-2-butene and 0.165 bar of trans-2-butene,what is the equilibrium pressure of each gas?

Correct Answer
verified

Correct Answer
verified

For the reaction: 3 Fe(s) + 4 H₂O(g) ⇌ Fe₃O₄(s) + 4 H₂(g) Write the expression for Kp.

Correct Answer
verified

Consider the reaction: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) ,Δ_rH° = -196.6 kJ/mol The equilibrium is displaced to the left if:

Correct Answer
verified

Write the equilibrium constant expression for the reaction: 3 Sn(s) + 4 HNO₃(aq) + H₂O(l) ⇌ 3 H₂SnO₃(s) + 4 NO(g)

Correct Answer
verified
B

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: 2 ICl(g) ⇌ I₂(g) + Cl₂(g) What is the equilibrium concentration of ICl if 0.45 mol of I₂ and 0.45 mol of Cl₂ are initially mixed in a 2.0 L flask?

Correct Answer
verified

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which K_p = 0.1134 at 25 °C and Δ_rH° = 58.03 kJ/mol.Assume that 1 mole of N₂O₄ and 2 moles of NO₂ are introduced into a 5.0 liter container.What will be the equilibrium value of [N₂O]?

Correct Answer
verified

Correct Answer
verified
B

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which K_p = 0.1134 at 25 °C and Δ_rH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N₂O₄ was present inside the container,compute At equilibrium.

Correct Answer
verified

Consider the following hypothetical equilibrium reaction: A₂(g) + B₂(g) ⇌ 2 AB(g) where K_c = The equilibrium constant for the reaction: 2 A₂(g) + 2 B₂(g) ⇌ 4 AB(g) is ________.

Correct Answer
verified
E

Correct Answer
verified

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which K_p = 0.1134 at 25 °C and Δ_rH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N₂O₄ was present inside the container,compute At equilibrium.

Correct Answer
verified

For the following chemical equilibrium,K_p = 4.6 × 10^-14 at 25 °C,find the value of K_c for this reaction at 25 °C. 2 Cl₂(g) + 2 H₂O(g) ⇌ 4 HCl(g) + O₂(g)

Correct Answer
verified

For the reaction CO(g) + 3 H₂(g) ⇌ H₂O(g) + CH₄(g) ,K_c = 190 at 1000 K.If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025 M,[H₂] = 0.045 M,[H₂O] = 0.025,M and [CH₄] = 0.046 M,in which direction will a reaction occur and why?

Correct Answer
verified

Correct Answer
verified

For the reaction CO(g) + 3 H₂(g) ⇌ H₂O(g) + CH₄(g) ,K_c = 190 at 1000 K.If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M,[H₂] = 0.045 M,[H₂O] = 0.020,M and [CH₄] = 0.031 M,in which direction will a reaction occur and why?

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Write the equilibrium constant expression for the following reaction: 2 KI(aq) + H₂O₂(aq) ⇌ 2 KOH(aq) + I₂(aq)

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