Question 1

The following reaction occurred when a 1.0-liter reaction vessel was initially charged with 2.0 moles of N2(g) and 4.0 moles of H2(g) : 3H2(g) + N2(g)  2(g) and 4.0 moles of H2(g) : 3H2(g) + N2(g)    2NH3(g)  Once equilibrium was established,the concentration of NH3(g) was determined to be 0.57 M at 700.°C.The value for Kc at 700.°C for the formation of ammonia is: A)  3.2 × 10-1 B)  6.1 × 10-3 C)  1.1 × 10-1 D)  6.0 × 10-2 E)  none of these" class="answers-bank-image d-inline" rel="preload" > 2NH3(g) 
Once equilibrium was established,the concentration of NH3(g) was determined to be 0.57 M at 700.°C.The value for Kc at 700.°C for the formation of ammonia is:

Accepted Answer

A)   3.2 × 10-1
B)   6.1 × 10-3
C)   1.1 × 10-1
D)   6.0 × 10-2
E)   none of these

Question 2

A sample of solid NH4NO3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: NH4NO3(s)  4NO3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: NH4NO3(s)    N2O(g) + 2H2O(g)  At equilibrium the total pressure in the container was found to be 2.72 atm at a temperature of 500.°C.Calculate Kp. A)  1.64 B)  0.822 C)  2.98 D)  80.5 E)  0.745" class="answers-bank-image d-inline" rel="preload" > N2O(g) + 2H2O(g) 
At equilibrium the total pressure in the container was found to be 2.72 atm at a temperature of 500.°C.Calculate Kp.

Accepted Answer

A)   1.64
B)   0.822
C)   2.98
D)   80.5
E)   0.745

Question 3

For the equilibrium N2O4(g)  2O4(g)    2NO2(g) ,at 298 K,Kp = 0.15.For this reaction system,it is found that the partial pressure of N2O4 is 3.7 × 10-2 atm at equilibrium.What is the partial pressure of NO2 at equilibrium? A)  4.9 atm B)  24 atm C)  0.0016 atm D)  0.0055 atm E)  0.074 atm" class="answers-bank-image d-inline" rel="preload" > 2NO2(g) ,at 298 K,Kp = 0.15.For this reaction system,it is found that the partial pressure of N2O4 is 3.7 × 10-2 atm at equilibrium.What is the partial pressure of NO2 at equilibrium?

Accepted Answer

A)   4.9 atm
B)   24 atm
C)   0.0016 atm
D)   0.0055 atm
E)   0.074 atm

Question 4

Which of the following statements is true if reaction quotient (Q) is greater than equilibrium constant (K) ?

Accepted Answer

A)   Reactant concentrations will increase.
B)   Product concentrations will increase.
C)   Reactants will convert to products.
D)   Standard enthalpy of formation of products decreases.
E)   Standard enthalpy of formation of reactants increases.

Question 5

The standard enthalpy of formation of ammonia is -46.1 kJ/mol.
1/2 N2(g)+ 3/2 H2(g)  NH3(g)
Commercially,the reaction is carried out at high temperatures.Using your knowledge of kinetics and equilibrium,explain an advantage and a disadvantage of synthesizing ammonia at high temperatures.

Accepted Answer

The rate of formation of ammonia is negl...

Question 6

Consider the following equilibrium. PCl3(g) + Cl2(g)  3(g) + Cl2(g)    PCl5(g)  ΔH = -92 kJ The concentration of PCl3 at equilibrium can be increased by: A)  decreasing the temperature. B)  adding Cl2 to the system. C)  adding PCl5 to the system. D)  increasing the pressure. E)  adding a catalyst." class="answers-bank-image d-inline" rel="preload" > PCl5(g)  ΔH = -92 kJ
The concentration of PCl3 at equilibrium can be increased by:

Accepted Answer

A)   decreasing the temperature.
B)   adding Cl2 to the system.
C)   adding PCl5 to the system.
D)   increasing the pressure.
E)   adding a catalyst.

Question 7

Excess Ag2SO4(s) is placed in water at 25 °C.At equilibrium,the solution contains 0.029 M Ag+(aq) .What is the equilibrium constant for the reaction below? Ag2SO4(s)  2SO4(s) is placed in water at 25 °C.At equilibrium,the solution contains 0.029 M Ag+(aq) .What is the equilibrium constant for the reaction below? Ag2SO4(s)    2 Ag+(aq) + SO42-(aq)  A)  1.8 × 10-7 B)  6.1 × 10-6 C)  1.2 × 10-5 D)  2.4 × 10-5 E)  8.4 × 10-4" class="answers-bank-image d-inline" rel="preload" > 2 Ag+(aq) + SO42-(aq)

Accepted Answer

A)   1.8 × 10-7
B)   6.1 × 10-6
C)   1.2 × 10-5
D)   2.4 × 10-5
E)   8.4 × 10-4

Question 8

When gaseous carbon monoxide and hydrogen are combined in a sealed vessel and heated they will eventually form an equilibrium mixture of reactants and products according to the balanced chemical equilibrium below. CO(g) + 3H2(g)  2(g)    CH4(g) + H2O(g)  In one such reaction 3 moles of one reactant were combined with 1 mole of the other reactant in a fixed volume vessel and heated to 1200 K.Analysis of the reaction mixture at various times gave the results below.Which component of the reaction mixture is represented by curve B?   A)  hydrogen B)  carbon monoxide C)  either methane or water D)  either hydrogen or carbon monoxide E)  not enough information to decide" class="answers-bank-image d-inline" rel="preload" > CH4(g) + H2O(g) 
In one such reaction 3 moles of one reactant were combined with 1 mole of the other reactant in a fixed volume vessel and heated to 1200 K.Analysis of the reaction mixture at various times gave the results below.Which component of the reaction mixture is represented by curve B? 2(g)    CH4(g) + H2O(g)  In one such reaction 3 moles of one reactant were combined with 1 mole of the other reactant in a fixed volume vessel and heated to 1200 K.Analysis of the reaction mixture at various times gave the results below.Which component of the reaction mixture is represented by curve B?   A)  hydrogen B)  carbon monoxide C)  either methane or water D)  either hydrogen or carbon monoxide E)  not enough information to decide" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   hydrogen
B)   carbon monoxide
C)   either methane or water
D)   either hydrogen or carbon monoxide
E)   not enough information to decide

Question 9

At 25 °C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? AgBr(s)  +(aq) + Br-(aq)  A)  5.40 × 10-13 B)  5.40 × 10-11 C)  1.90 × 10-8 D)  7.35 × 10-7 E)  1.90 × 10-6" class="answers-bank-image d-inline" rel="preload" > Ag+(aq) + Br-(aq)

Accepted Answer

A)   5.40 × 10-13
B)   5.40 × 10-11
C)   1.90 × 10-8
D)   7.35 × 10-7
E)   1.90 × 10-6

Question 10

What is the Kc expression for the equilibrium given below? CuI(s)  c expression for the equilibrium given below? CuI(s)    Cu+(aq) + I−(aq)  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > Cu+(aq) + I−(aq)

Accepted Answer

A)   c expression for the equilibrium given below? CuI(s)    Cu+(aq) + I−(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   c expression for the equilibrium given below? CuI(s)    Cu+(aq) + I−(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   c expression for the equilibrium given below? CuI(s)    Cu+(aq) + I−(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   c expression for the equilibrium given below? CuI(s)    Cu+(aq) + I−(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   c expression for the equilibrium given below? CuI(s)    Cu+(aq) + I−(aq)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 11

Which of the following is the correct balanced equation for the equilibrium constant expression given below? 2(aq)    Pb(s) + F2(aq)  B)  PbF2(s)    Pb2+(aq) + 2 F-(aq)  C)  Pb2+(aq) + 2 F-(aq)    PbF2(s)  D)  Pb(s) + F2(aq)    PbF2(aq)  E)  PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   PbF2(aq)  2(aq)    Pb(s) + F2(aq)  
B)   PbF2(s)    Pb2+(aq) + 2 F-(aq)  
C)   Pb2+(aq) + 2 F-(aq)    PbF2(s)  
D)   Pb(s) + F2(aq)    PbF2(aq)  
E)   PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" > Pb(s) + F2(aq) 
B)   PbF2(s)  2(aq)    Pb(s) + F2(aq)  
B)   PbF2(s)    Pb2+(aq) + 2 F-(aq)  
C)   Pb2+(aq) + 2 F-(aq)    PbF2(s)  
D)   Pb(s) + F2(aq)    PbF2(aq)  
E)   PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" > Pb2+(aq) + 2 F-(aq) 
C)   Pb2+(aq) + 2 F-(aq)  2(aq)    Pb(s) + F2(aq)  
B)   PbF2(s)    Pb2+(aq) + 2 F-(aq)  
C)   Pb2+(aq) + 2 F-(aq)    PbF2(s)  
D)   Pb(s) + F2(aq)    PbF2(aq)  
E)   PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" > PbF2(s) 
D)   Pb(s) + F2(aq)  2(aq)    Pb(s) + F2(aq)  
B)   PbF2(s)    Pb2+(aq) + 2 F-(aq)  
C)   Pb2+(aq) + 2 F-(aq)    PbF2(s)  
D)   Pb(s) + F2(aq)    PbF2(aq)  
E)   PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" > PbF2(aq) 
E)   PbF+(aq) + F-(aq)  2(aq)    Pb(s) + F2(aq)  
B)   PbF2(s)    Pb2+(aq) + 2 F-(aq)  
C)   Pb2+(aq) + 2 F-(aq)    PbF2(s)  
D)   Pb(s) + F2(aq)    PbF2(aq)  
E)   PbF+(aq) + F-(aq)    PbF2(aq) " class="answers-bank-image d-inline" rel="preload" > PbF2(aq)

Question 12

For the reaction 2NO(g) + O2(g)  2(g)    2NO2(g) at 750°C,what is the relationship between Kc and Kp? A)  Kc = Kp B)  Kc = Kp × (RT) -1 C)  Kc = Kp = 1.0 D)  Kc = Kp × (RT) ¾ E)  Kc = Kp × (RT) 1" class="answers-bank-image d-inline" rel="preload" > 2NO2(g) at 750°C,what is the relationship between Kc and Kp?

Accepted Answer

A)   Kc = Kp
B)   Kc = Kp × (RT) -1
C)   Kc = Kp = 1.0
D)   Kc = Kp × (RT) ¾
E)   Kc = Kp × (RT) 1

Question 13

Assume that the following chemical reaction is at equilibrium. 2 ICl(g)  2(g) + Cl2(g)  ΔH° = +26.9 kJ At 25 °C,Kp = 2.0 × 105.If the temperature is increase to 45 °C,which statement applies? A)  Kp will decrease and the reaction will proceed in the backward direction. B)  Kp will decrease and the reaction will proceed in the forward direction. C)  Kp will remain unchanged and the reaction will proceed in the forward direction. D)  Kp will increase and the reaction will proceed in the backward direction. E)  Kp will increase and the reaction will proceed in the forward direction." class="answers-bank-image d-inline" rel="preload" > I2(g) + Cl2(g) 
ΔH° = +26.9 kJ
At 25 °C,Kp = 2.0 × 105.If the temperature is increase to 45 °C,which statement applies?

Accepted Answer

A)   Kp will decrease and the reaction will proceed in the backward direction.
B)   Kp will decrease and the reaction will proceed in the forward direction.
C)   Kp will remain unchanged and the reaction will proceed in the forward direction.
D)   Kp will increase and the reaction will proceed in the backward direction.
E)   Kp will increase and the reaction will proceed in the forward direction.

Question 14

Consider the following equilibrium: CO2(g) + H2(g)  2(g) + H2(g)    CO(g) + H2O(g) ; Kc = 1.6 at 1260 K Suppose 0.019 mol CO2 and 0.030 mol H2 are placed in a 3.00-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g) ? (R = 0.0821 L · atm/K·mol)  A)  4 atm B)  0.35 atm C)  1.6 atm D)  0.66 atm E)  1 atm" class="answers-bank-image d-inline" rel="preload" > CO(g) + H2O(g) ; Kc = 1.6 at 1260 K
Suppose 0.019 mol CO2 and 0.030 mol H2 are placed in a 3.00-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g) ? (R = 0.0821 L · atm/K·mol)

Accepted Answer

A)   4 atm
B)   0.35 atm
C)   1.6 atm
D)   0.66 atm
E)   1 atm

Question 15

Consider the formation of ozone by the following reaction. 3 O2(g)  2(g)    2 O3(g)  Calculate the value of Kp,given that Kc = 2.5 × 10-29 at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)  A)  1.0 × 10-30 B)  2.1 × 10-30 C)  2.5 × 10-29 D)  3.3 × 10-28 E)  6.1 ×10-28" class="answers-bank-image d-inline" rel="preload" > 2 O3(g) 
Calculate the value of Kp,given that Kc = 2.5 × 10-29 at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)

Accepted Answer

A)   1.0 × 10-30
B)   2.1 × 10-30
C)   2.5 × 10-29
D)   3.3 × 10-28
E)   6.1 ×10-28

Question 16

Consider the reaction below. 2 HF(g)  2(g) + F2(g) (Kc = 1.00 × 10-2)  Given that 1.00 mol of HF(g) ,0.241 mol of H2(g) ,and 0.750 mol of F2(g) are mixed in a 5.00 L flask,determine the reaction quotient,Q. A)  Q = 0.0452 B)  Q = 0.181 C)  Q = 0.0362 D)  Q = 1.99 E)  None of these" class="answers-bank-image d-inline" rel="preload" > H2(g) + F2(g) (Kc = 1.00 × 10-2) 
Given that 1.00 mol of HF(g) ,0.241 mol of H2(g) ,and 0.750 mol of F2(g) are mixed in a 5.00 L flask,determine the reaction quotient,Q.

Accepted Answer

A)   Q = 0.0452
B)   Q = 0.181
C)   Q = 0.0362
D)   Q = 1.99
E)   None of these

Question 17

Write the expression for Kp for the reaction below. 2 NOBr(g)  p for the reaction below. 2 NOBr(g)    2 NO(g) + Br2(   )  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > 2 NO(g) + Br2( p for the reaction below. 2 NOBr(g)    2 NO(g) + Br2(   )  A)    B)    C)    D)    E)   " class="answers-bank-image d-inline" rel="preload" > )

Accepted Answer

A)   p for the reaction below. 2 NOBr(g)    2 NO(g) + Br2(   )  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   p for the reaction below. 2 NOBr(g)    2 NO(g) + Br2(   )  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   p for the reaction below. 2 NOBr(g)    2 NO(g) + Br2(   )  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   p for the reaction below. 2 NOBr(g)    2 NO(g) + Br2(   )  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   p for the reaction below. 2 NOBr(g)    2 NO(g) + Br2(   )  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Exam 16: Principles of Chemical Reactivity: Equilibria

Correct Answer
verified

Consider the formation of ozone by the following reaction. 3 O₂(g) 2 O₃(g) Calculate the value of K_p,given that K_c = 2.5 × 10^-29 at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)

Correct Answer
verified

What is the K_c expression for the equilibrium given below? CuI(s) Cu⁺(aq) + I−(aq)

Correct Answer
verified

At 25 °C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? AgBr(s) Ag⁺(aq) + Br^-(aq)

Correct Answer
verified

Write the expression for K_p for the reaction below. 2 NOBr(g) 2 NO(g) + Br₂( )

Correct Answer
verified

For the equilibrium N₂O₄(g) 2NO₂(g) ,at 298 K,K_p = 0.15.For this reaction system,it is found that the partial pressure of N₂O₄ is 3.7 × 10^-2 atm at equilibrium.What is the partial pressure of NO₂ at equilibrium?

Correct Answer
verified

Correct Answer
verified

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I₂(g) + Cl₂(g) ΔH° = +26.9 kJ At 25 °C,K_p = 2.0 × 10⁵.If the temperature is increase to 45 °C,which statement applies?

Correct Answer
verified

Consider the reaction below. 2 HF(g) H₂(g) + F₂(g) (K_c = 1.00 × 10^-2) Given that 1.00 mol of HF(g) ,0.241 mol of H₂(g) ,and 0.750 mol of F₂(g) are mixed in a 5.00 L flask,determine the reaction quotient,Q.

Correct Answer
verified

Consider the following equilibrium: CO₂(g) + H₂(g) CO(g) + H₂O(g) ; K_c = 1.6 at 1260 K Suppose 0.019 mol CO₂ and 0.030 mol H₂ are placed in a 3.00-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g) ? (R = 0.0821 L · atm/K·mol)

Correct Answer
verified

Consider the following equilibrium. PCl₃(g) + Cl₂(g) PCl₅(g) ΔH = -92 kJ The concentration of PCl₃ at equilibrium can be increased by:

Correct Answer
verified

Correct Answer
verified

Which of the following is the correct balanced equation for the equilibrium constant expression given below?

Correct Answer
verified

Excess Ag₂SO₄(s) is placed in water at 25 °C.At equilibrium,the solution contains 0.029 M Ag⁺(aq) .What is the equilibrium constant for the reaction below? Ag₂SO₄(s) 2 Ag⁺(aq) + SO₄^2-(aq)

Correct Answer
verified

Which of the following statements is true if reaction quotient (Q) is greater than equilibrium constant (K) ?

Correct Answer
verified

The standard enthalpy of formation of ammonia is -46.1 kJ/mol. 1/2 N₂(g)+ 3/2 H₂(g) NH₃(g) Commercially,the reaction is carried out at high temperatures.Using your knowledge of kinetics and equilibrium,explain an advantage and a disadvantage of synthesizing ammonia at high temperatures.

Correct Answer
verified
The rate of formation of ammonia is negl...
View Answer

For the reaction 2NO(g) + O₂(g) 2NO₂(g) at 750°C,what is the relationship between K_c and K_p?

Correct Answer
verified

Exam 16: Principles of Chemical Reactivity: Equilibria

Correct AnswerverifiedShow Answer

Consider the formation of ozone by the following reaction. 3 O2(g) 2 O3(g) Calculate the value of Kp,given that Kc = 2.5 × 10-29 at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)

Correct AnswerverifiedShow Answer

What is the Kc expression for the equilibrium given below? CuI(s) Cu+(aq) + I−(aq)

Correct AnswerverifiedShow Answer

At 25 °C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? AgBr(s) Ag+(aq) + Br-(aq)

Correct AnswerverifiedShow Answer

Write the expression for Kp for the reaction below. 2 NOBr(g) 2 NO(g) + Br2( )

Correct AnswerverifiedShow Answer

For the equilibrium N2O4(g) 2NO2(g) ,at 298 K,Kp = 0.15.For this reaction system,it is found that the partial pressure of N2O4 is 3.7 × 10-2 atm at equilibrium.What is the partial pressure of NO2 at equilibrium?

Correct AnswerverifiedShow Answer

A sample of solid NH4NO3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: NH4NO3(s) N2O(g) + 2H2O(g) At equilibrium the total pressure in the container was found to be 2.72 atm at a temperature of 500.°C.Calculate Kp.

Correct AnswerverifiedShow Answer

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I2(g) + Cl2(g) ΔH° = +26.9 kJ At 25 °C,Kp = 2.0 × 105.If the temperature is increase to 45 °C,which statement applies?

Correct AnswerverifiedShow Answer

Consider the reaction below. 2 HF(g) H2(g) + F2(g) (Kc = 1.00 × 10-2) Given that 1.00 mol of HF(g) ,0.241 mol of H2(g) ,and 0.750 mol of F2(g) are mixed in a 5.00 L flask,determine the reaction quotient,Q.

Correct AnswerverifiedShow Answer

Consider the following equilibrium: CO2(g) + H2(g) CO(g) + H2O(g) ; Kc = 1.6 at 1260 K Suppose 0.019 mol CO2 and 0.030 mol H2 are placed in a 3.00-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g) ? (R = 0.0821 L · atm/K·mol)

Correct AnswerverifiedShow Answer

Consider the following equilibrium. PCl3(g) + Cl2(g) PCl5(g) ΔH = -92 kJ The concentration of PCl3 at equilibrium can be increased by:

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which of the following is the correct balanced equation for the equilibrium constant expression given below?

Correct AnswerverifiedShow Answer

Excess Ag2SO4(s) is placed in water at 25 °C.At equilibrium,the solution contains 0.029 M Ag+(aq) .What is the equilibrium constant for the reaction below? Ag2SO4(s) 2 Ag+(aq) + SO42-(aq)

Correct AnswerverifiedShow Answer

Which of the following statements is true if reaction quotient (Q) is greater than equilibrium constant (K) ?

Correct AnswerverifiedShow Answer

The standard enthalpy of formation of ammonia is -46.1 kJ/mol. 1/2 N2(g)+ 3/2 H2(g) NH3(g) Commercially,the reaction is carried out at high temperatures.Using your knowledge of kinetics and equilibrium,explain an advantage and a disadvantage of synthesizing ammonia at high temperatures.

Correct AnswerverifiedThe rate of formation of ammonia is negl...View AnswerShow Answer

For the reaction 2NO(g) + O2(g) 2NO2(g) at 750°C,what is the relationship between Kc and Kp?

Correct AnswerverifiedShow Answer

Correct Answer
verified

Consider the formation of ozone by the following reaction. 3 O₂(g) 2 O₃(g) Calculate the value of K_p,given that K_c = 2.5 × 10^-29 at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)

Correct Answer
verified

What is the K_c expression for the equilibrium given below? CuI(s) Cu⁺(aq) + I−(aq)

Correct Answer
verified

At 25 °C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? AgBr(s) Ag⁺(aq) + Br^-(aq)

Correct Answer
verified

Write the expression for K_p for the reaction below. 2 NOBr(g) 2 NO(g) + Br₂( )

Correct Answer
verified

For the equilibrium N₂O₄(g) 2NO₂(g) ,at 298 K,K_p = 0.15.For this reaction system,it is found that the partial pressure of N₂O₄ is 3.7 × 10^-2 atm at equilibrium.What is the partial pressure of NO₂ at equilibrium?

Correct Answer
verified

Correct Answer
verified

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I₂(g) + Cl₂(g) ΔH° = +26.9 kJ At 25 °C,K_p = 2.0 × 10⁵.If the temperature is increase to 45 °C,which statement applies?

Correct Answer
verified

Consider the reaction below. 2 HF(g) H₂(g) + F₂(g) (K_c = 1.00 × 10^-2) Given that 1.00 mol of HF(g) ,0.241 mol of H₂(g) ,and 0.750 mol of F₂(g) are mixed in a 5.00 L flask,determine the reaction quotient,Q.

Correct Answer
verified

Consider the following equilibrium: CO₂(g) + H₂(g) CO(g) + H₂O(g) ; K_c = 1.6 at 1260 K Suppose 0.019 mol CO₂ and 0.030 mol H₂ are placed in a 3.00-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g) ? (R = 0.0821 L · atm/K·mol)

Correct Answer
verified

Consider the following equilibrium. PCl₃(g) + Cl₂(g) PCl₅(g) ΔH = -92 kJ The concentration of PCl₃ at equilibrium can be increased by:

Correct Answer
verified

Correct Answer
verified

Correct Answer
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Excess Ag₂SO₄(s) is placed in water at 25 °C.At equilibrium,the solution contains 0.029 M Ag⁺(aq) .What is the equilibrium constant for the reaction below? Ag₂SO₄(s) 2 Ag⁺(aq) + SO₄^2-(aq)

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The standard enthalpy of formation of ammonia is -46.1 kJ/mol. 1/2 N₂(g)+ 3/2 H₂(g) NH₃(g) Commercially,the reaction is carried out at high temperatures.Using your knowledge of kinetics and equilibrium,explain an advantage and a disadvantage of synthesizing ammonia at high temperatures.

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The rate of formation of ammonia is negl...
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For the reaction 2NO(g) + O₂(g) 2NO₂(g) at 750°C,what is the relationship between K_c and K_p?

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