Question 1

If a reaction is endothermic, __________ the reaction temperature results in an increase in K.

Accepted Answer

The answer of If a reaction is endothermic, __________ the...

Question 2

Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)  2 (g)  A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.36 mol of NOBr. How many moles of NO and Br2, respectively, are in the flask at equilibrium? A) .28,.28 B) .36,.18 C) .28,.14 D) .14,.23 E) .36,.36" class="answers-bank-image d-inline" rel="preload" > 2NO (g) + Br2 (g) 
A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.36 mol of NOBr. How many moles of NO and Br2, respectively, are in the flask at equilibrium?

Accepted Answer

A)  .28,.28
B)  .36,.18
C)  .28,.14
D)  .14,.23
E)  .36,.36

Question 3

Given the following reaction at equilibrium at 450.0°C: CaCO3 (s)  3 (s)    CaO (s) + CO2 (g)  If pCO2 = 0.0135 atm, Kc = __________. A) 135 B) 0.0821 C) 0.801 D) 2.27 × 10-4 E) 8.01" class="answers-bank-image d-inline" rel="preload" > CaO (s) + CO2 (g) 
If pCO2 = 0.0135 atm, Kc = __________.

Accepted Answer

A)  135
B)  0.0821
C)  0.801
D)  2.27 × 10-4
E)  8.01

Question 4

In an exothermic equilibrium reaction, increasing the reaction temperature favors the formation of reactants.

Accepted Answer

A) True 
 B)False

Question 5

The reaction below is exothermic: 2SO2 (g) + O2 (g)  2 (g) + O2 (g)    2SO3 (g)  Le Châtelier's Principle predicts that __________ will result in an increase in the number of moles of SO3 (g) in the reaction container. A) increasing the pressure B) decreasing the pressure C) increasing the temperature D) removing some oxygen E) increasing the volume of the container" class="answers-bank-image d-inline" rel="preload" > 2SO3 (g) 
Le Châtelier's Principle predicts that __________ will result in an increase in the number of moles of SO3 (g) in the reaction container.

Accepted Answer

A)  increasing the pressure
B)  decreasing the pressure
C)  increasing the temperature
D)  removing some oxygen
E)  increasing the volume of the container

Question 6

The equilibrium constant for the gas phase reaction 2NH3 (g)  3 (g)    N2 (g) + 3H2 (g)  Is Keq = 230 at 300°C. At equilibrium, __________. A) products predominate B) reactants predominate C) roughly equal amounts of products and reactants are present D) only products are present E) only reactants are present" class="answers-bank-image d-inline" rel="preload" > N2 (g) + 3H2 (g) 
Is Keq = 230 at 300°C. At equilibrium, __________.

Accepted Answer

A)  products predominate
B)  reactants predominate
C)  roughly equal amounts of products and reactants are present
D)  only products are present
E)  only reactants are present

Question 7

The Keq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) + eq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? SO3 (g)    SO2 (g) +   O2 (g)  A) 0.224 B) 0.0125 C) 0.112 D) 8.93 E) -0.112" class="answers-bank-image d-inline" rel="preload" > O2 (g)  eq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? SO3 (g)    SO2 (g) +   O2 (g)  A) 0.224 B) 0.0125 C) 0.112 D) 8.93 E) -0.112" class="answers-bank-image d-inline" rel="preload" > SO3 (g) 
What is the value of Keq at this temperature for the following reaction?
SO3 (g)  eq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? SO3 (g)    SO2 (g) +   O2 (g)  A) 0.224 B) 0.0125 C) 0.112 D) 8.93 E) -0.112" class="answers-bank-image d-inline" rel="preload" > SO2 (g) + eq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? SO3 (g)    SO2 (g) +   O2 (g)  A) 0.224 B) 0.0125 C) 0.112 D) 8.93 E) -0.112" class="answers-bank-image d-inline" rel="preload" > O2 (g)

Accepted Answer

A)  0.224
B)  0.0125
C)  0.112
D)  8.93
E)  -0.112

Question 8

The Keq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) + eq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? 2SO3 (g)    2SO2 (g) + O2 (g)  A) 79.7 B) 2.99 C) 17.86 D) 4.46 E) 8.93" class="answers-bank-image d-inline" rel="preload" > O2 (g)  eq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? 2SO3 (g)    2SO2 (g) + O2 (g)  A) 79.7 B) 2.99 C) 17.86 D) 4.46 E) 8.93" class="answers-bank-image d-inline" rel="preload" > SO3 (g) 
What is the value of Keq at this temperature for the following reaction?
2SO3 (g)  eq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) +   O2 (g)    SO3 (g)  What is the value of Keq at this temperature for the following reaction? 2SO3 (g)    2SO2 (g) + O2 (g)  A) 79.7 B) 2.99 C) 17.86 D) 4.46 E) 8.93" class="answers-bank-image d-inline" rel="preload" > 2SO2 (g) + O2 (g)

Accepted Answer

A)  79.7
B)  2.99
C)  17.86
D)  4.46
E)  8.93

Question 9

The equilibrium-constant expression for the reaction Ti (s) + 2Cl2 (g)  2 (g)    TiCl4 (l)  Is given by A)    B)    C)    D) [Cl2 (g) ]-2  E)   " class="answers-bank-image d-inline" rel="preload" > TiCl4 (l) 
Is given by

Accepted Answer

A)   2 (g)    TiCl4 (l)  Is given by 
A)     
B)     
C)     
D)  [Cl2 (g) ]-2  
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2 (g)    TiCl4 (l)  Is given by 
A)     
B)     
C)     
D)  [Cl2 (g) ]-2  
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2 (g)    TiCl4 (l)  Is given by 
A)     
B)     
C)     
D)  [Cl2 (g) ]-2  
E)    " class="answers-bank-image d-inline" rel="preload" >
D)  [Cl2 (g) ]-2 
E)   2 (g)    TiCl4 (l)  Is given by 
A)     
B)     
C)     
D)  [Cl2 (g) ]-2  
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 10

Given the following reaction at equilibrium, if Kc = 1.90 × 1019 at 25.0°C, Kp = __________. H2 (g) + Br2 (g)  c = 1.90 × 1019 at 25.0°C, Kp = __________. H2 (g) + Br2 (g)    2 HBr (g)  A) 5.26 × 10-20 B) 1.56 × 104 C) 6.44 × 105 D) 1.90 × 1019 E) none of the above" class="answers-bank-image d-inline" rel="preload" > 2 HBr (g)

Accepted Answer

A)  5.26 × 10-20
B)  1.56 × 104
C)  6.44 × 105
D)  1.90 × 1019
E)  none of the above

Question 11

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N2O4 (g)  2O4 (g)    2NO2 (g)  A 1.000-L flask is charged with 3.00 × 10-2 mol of N2O4. At equilibrium, 2.36 × 10-2 mol of N2O4 remains. Keq for this reaction is __________. A) 0.723 B) 0.391 C) 0.212 D) 6.94 × 10-3 E) 1.92 × 10-4" class="answers-bank-image d-inline" rel="preload" > 2NO2 (g) 
A 1.000-L flask is charged with 3.00 × 10-2 mol of N2O4. At equilibrium, 2.36 × 10-2 mol of N2O4 remains. Keq for this reaction is __________.

Accepted Answer

A)  0.723
B)  0.391
C)  0.212
D)  6.94 × 10-3
E)  1.92 × 10-4 D

Question 12

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (aq) + H2O (l)  2O (l)    H3O+ (aq) + F- (aq)  A) [HF][H2O] / [H3O+][F-] B) 1 / [HF] C) [H3O+][F-] / [HF][H2O] D) [H3O+][F-] / [HF] E) [F-] / [HF]" class="answers-bank-image d-inline" rel="preload" > H3O+ (aq) + F- (aq)

Accepted Answer

A)  [HF][H2O] / [H3O+][F-]
B)  1 / [HF]
C)  [H3O+][F-] / [HF][H2O]
D)  [H3O+][F-] / [HF]
E)  [F-] / [HF]

Question 13

Which one of the following is true concerning the Haber process?

Accepted Answer

A)  It is a process used for shifting equilibrium positions to the right for more economical chemical synthesis of a variety of substances.
B)  It is a process used for the synthesis of ammonia.
C)  It is another way of stating Le Châtelier's principle.
D)  It is an industrial synthesis of sodium chloride that was discovered by Karl Haber.
E)  It is a process for the synthesis of elemental chlorine. B

Question 14

If Reaction A + Reaction B = Reaction C, then Kc Reaction C = __________.

Accepted Answer

K_cReaction ...

Question 15

For an exothermic reaction, increasing the reaction temperature results in a(an)__________ in K.

Accepted Answer

The answer of For an exothermic reaction, increasing the reaction...

Question 16

Le Châtelier's principle states that if a system at equilibrium is disturbed, the equilibrium will shift to minimize the disturbance.

Accepted Answer

A) True 
 B)False  True

Question 17

At 27°C, Kp = 0.095 for the equilibrium: NH4HS (s)  p = 0.095 for the equilibrium: NH4HS (s)    NH3 (g) + H2S (g)  A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4HS remains. A) 0.31 B) 0.095 C) 0.052 D) 0.0049 E) 3.8" class="answers-bank-image d-inline" rel="preload" > NH3 (g) + H2S (g) 
A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4HS remains.

Accepted Answer

A)  0.31
B)  0.095
C)  0.052
D)  0.0049
E)  3.8

Question 18

Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g)  2 (g) + O2 (g)    2SO3 (g) ΔH° = -99 kJ Le Châtelier's principle predicts that an increase in temperature will result in __________. A) a decrease in the partial pressure of SO3 B) a decrease in the partial pressure of SO2 C) an increase in Keq D) no changes in equilibrium partial pressures E) the partial pressure of O2 will decrease" class="answers-bank-image d-inline" rel="preload" > 2SO3 (g) ΔH° = -99 kJ
Le Châtelier's principle predicts that an increase in temperature will result in __________.

Accepted Answer

A)  a decrease in the partial pressure of SO3
B)  a decrease in the partial pressure of SO2
C)  an increase in Keq
D)  no changes in equilibrium partial pressures
E)  the partial pressure of O2 will decrease

Question 19

Consider the following reaction at equilibrium: 2CO2 (g)  2 (g)    2CO (g) + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that adding O2 (g) to the reaction container will __________. A) increase the partial pressure of CO (g) at equilibrium B) decrease the partial pressure of CO2 (g) at equilibrium C) increase the value of the equilibrium constant D) increase the partial pressure of CO2 (g) at equilibrium E) decrease the value of the equilibrium constant" class="answers-bank-image d-inline" rel="preload" > 2CO (g) + O2 (g) ΔH° = -514 kJ
Le Châtelier's principle predicts that adding O2 (g) to the reaction container will __________.

Accepted Answer

A)  increase the partial pressure of CO (g) at equilibrium
B)  decrease the partial pressure of CO2 (g) at equilibrium
C)  increase the value of the equilibrium constant
D)  increase the partial pressure of CO2 (g) at equilibrium
E)  decrease the value of the equilibrium constant

Question 20

The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g)  p) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g)    PCl3 (g) + Cl2 (g)  A vessel is charged with PCl5, giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl3 is __________ atm. A) 0.0782 B) 0.0455 C) 0.0908 D) 0.0330 E) 0.123" class="answers-bank-image d-inline" rel="preload" > PCl3 (g) + Cl2 (g) 
A vessel is charged with PCl5, giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl3 is __________ atm.

Accepted Answer

A)  0.0782
B)  0.0455
C)  0.0908
D)  0.0330
E)  0.123

Exam 15: Chemical Equilibrium

If a reaction is endothermic, __________ the reaction temperature results in an increase in K.

Correct Answer
verified

Correct Answer
verified

Given the following reaction at equilibrium at 450.0°C: CaCO₃ (s) CaO (s) + CO₂ (g) If pCO₂ = 0.0135 atm, K_c = __________.

Correct Answer
verified

In an exothermic equilibrium reaction, increasing the reaction temperature favors the formation of reactants.

Correct Answer
verified

The reaction below is exothermic: 2SO₂ (g) + O₂ (g) 2SO₃ (g) Le Châtelier's Principle predicts that __________ will result in an increase in the number of moles of SO₃ (g) in the reaction container.

Correct Answer
verified

The equilibrium constant for the gas phase reaction 2NH₃ (g) N₂ (g) + 3H₂ (g) Is K_eq = 230 at 300°C. At equilibrium, __________.

Correct Answer
verified

The K_eq for the equilibrium below is 0.112 at 700.0°C. SO₂ (g) + O₂ (g) SO₃ (g) What is the value of K_eq at this temperature for the following reaction? SO₃ (g) SO₂ (g) + O₂ (g)

Correct Answer
verified

The K_eq for the equilibrium below is 0.112 at 700.0°C. SO₂ (g) + O₂(g) SO₃ (g) What is the value of K_eq at this temperature for the following reaction? 2SO₃ (g) 2SO₂ (g) + O₂ (g)

Correct Answer
verified

The equilibrium-constant expression for the reaction Ti (s) + 2Cl₂(g) TiCl₄(l) Is given by

Correct Answer
verified

Given the following reaction at equilibrium, if K_c = 1.90 × 10¹⁹at 25.0°C, K_p = __________. H₂ (g) + Br₂ (g) 2 HBr (g)

Correct Answer
verified

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N₂O₄ (g) 2NO₂ (g) A 1.000-L flask is charged with 3.00 × 10^-2 mol of N₂O₄. At equilibrium, 2.36 × 10^-2 mol of N₂O₄ remains. K_eq for this reaction is __________.

Correct Answer
verified
D

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (aq) + H₂O (l) H₃O⁺ (aq) + F^- (aq)

Correct Answer
verified

Which one of the following is true concerning the Haber process?

Correct Answer
verified
B

If Reaction A + Reaction B = Reaction C, then K_cReaction C = __________.

Correct Answer
verified
K_cReaction ...
View Answer

For an exothermic reaction, increasing the reaction temperature results in a(an)__________ in K.

Correct Answer
verified

Le Châtelier's principle states that if a system at equilibrium is disturbed, the equilibrium will shift to minimize the disturbance.

Correct Answer
verified
True

At 27°C, K_p = 0.095 for the equilibrium: NH₄HS (s) NH₃(g) + H₂S (g) A sample of solid NH₄HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH₄HS remains.

Correct Answer
verified

Consider the following reaction at equilibrium: 2SO₂ (g) + O₂ (g) 2SO₃ (g) ΔH° = -99 kJ Le Châtelier's principle predicts that an increase in temperature will result in __________.

Correct Answer
verified

Consider the following reaction at equilibrium: 2CO₂ (g) 2CO (g) + O₂ (g) ΔH° = -514 kJ Le Châtelier's principle predicts that adding O₂ (g) to the reaction container will __________.

Correct Answer
verified

The equilibrium constant (K_p) for the interconversion of PCl₅ and PCl₃ is 0.0121: PCl₅ (g) PCl₃ (g) + Cl₂ (g) A vessel is charged with PCl₅, giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl₃ is __________ atm.

Correct Answer
verified

Exam 15: Chemical Equilibrium

If a reaction is endothermic, __________ the reaction temperature results in an increase in K.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Given the following reaction at equilibrium at 450.0°C: CaCO3 (s) CaO (s) + CO2 (g) If pCO2 = 0.0135 atm, Kc = __________.

Correct AnswerverifiedShow Answer

In an exothermic equilibrium reaction, increasing the reaction temperature favors the formation of reactants.

Correct AnswerverifiedShow Answer

The reaction below is exothermic: 2SO2 (g) + O2 (g) 2SO3 (g) Le Châtelier's Principle predicts that __________ will result in an increase in the number of moles of SO3 (g) in the reaction container.

Correct AnswerverifiedShow Answer

The equilibrium constant for the gas phase reaction 2NH3 (g) N2 (g) + 3H2 (g) Is Keq = 230 at 300°C. At equilibrium, __________.

Correct AnswerverifiedShow Answer

The Keq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) + O2 (g) SO3 (g) What is the value of Keq at this temperature for the following reaction? SO3 (g) SO2 (g) + O2 (g)

Correct AnswerverifiedShow Answer

The Keq for the equilibrium below is 0.112 at 700.0°C. SO2 (g) + O2 (g) SO3 (g) What is the value of Keq at this temperature for the following reaction? 2SO3 (g) 2SO2 (g) + O2 (g)

Correct AnswerverifiedShow Answer

The equilibrium-constant expression for the reaction Ti (s) + 2Cl2 (g) TiCl4 (l) Is given by

Correct AnswerverifiedShow Answer

Given the following reaction at equilibrium, if Kc = 1.90 × 1019 at 25.0°C, Kp = __________. H2 (g) + Br2 (g) 2 HBr (g)

Correct AnswerverifiedShow Answer

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N2O4 (g) 2NO2 (g) A 1.000-L flask is charged with 3.00 × 10-2 mol of N2O4. At equilibrium, 2.36 × 10-2 mol of N2O4 remains. Keq for this reaction is __________.

Correct AnswerverifiedD

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (aq) + H2O (l) H3O+ (aq) + F- (aq)

Correct AnswerverifiedShow Answer

Which one of the following is true concerning the Haber process?

Correct AnswerverifiedB

If Reaction A + Reaction B = Reaction C, then Kc Reaction C = __________.

Correct AnswerverifiedKc Reaction ...View AnswerShow Answer

For an exothermic reaction, increasing the reaction temperature results in a(an)__________ in K.

Correct AnswerverifiedShow Answer

Le Châtelier's principle states that if a system at equilibrium is disturbed, the equilibrium will shift to minimize the disturbance.

Correct AnswerverifiedTrue

At 27°C, Kp = 0.095 for the equilibrium: NH4HS (s) NH3 (g) + H2S (g) A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4HS remains.

Correct AnswerverifiedShow Answer

Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) 2SO3 (g) ΔH° = -99 kJ Le Châtelier's principle predicts that an increase in temperature will result in __________.

Correct AnswerverifiedShow Answer

Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that adding O2 (g) to the reaction container will __________.

Correct AnswerverifiedShow Answer

The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g) PCl3 (g) + Cl2 (g) A vessel is charged with PCl5, giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl3 is __________ atm.

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified

Given the following reaction at equilibrium at 450.0°C: CaCO₃ (s) CaO (s) + CO₂ (g) If pCO₂ = 0.0135 atm, K_c = __________.

Correct Answer
verified

Correct Answer
verified

The reaction below is exothermic: 2SO₂ (g) + O₂ (g) 2SO₃ (g) Le Châtelier's Principle predicts that __________ will result in an increase in the number of moles of SO₃ (g) in the reaction container.

Correct Answer
verified

The equilibrium constant for the gas phase reaction 2NH₃ (g) N₂ (g) + 3H₂ (g) Is K_eq = 230 at 300°C. At equilibrium, __________.

Correct Answer
verified

The K_eq for the equilibrium below is 0.112 at 700.0°C. SO₂ (g) + O₂ (g) SO₃ (g) What is the value of K_eq at this temperature for the following reaction? SO₃ (g) SO₂ (g) + O₂ (g)

Correct Answer
verified

The K_eq for the equilibrium below is 0.112 at 700.0°C. SO₂ (g) + O₂(g) SO₃ (g) What is the value of K_eq at this temperature for the following reaction? 2SO₃ (g) 2SO₂ (g) + O₂ (g)

Correct Answer
verified

The equilibrium-constant expression for the reaction Ti (s) + 2Cl₂(g) TiCl₄(l) Is given by

Correct Answer
verified

Given the following reaction at equilibrium, if K_c = 1.90 × 10¹⁹at 25.0°C, K_p = __________. H₂ (g) + Br₂ (g) 2 HBr (g)

Correct Answer
verified

Dinitrogen tetroxide partially decomposes according to the following equilibrium: N₂O₄ (g) 2NO₂ (g) A 1.000-L flask is charged with 3.00 × 10^-2 mol of N₂O₄. At equilibrium, 2.36 × 10^-2 mol of N₂O₄ remains. K_eq for this reaction is __________.

Correct Answer
verified
D

Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (aq) + H₂O (l) H₃O⁺ (aq) + F^- (aq)

Correct Answer
verified

Correct Answer
verified
B

If Reaction A + Reaction B = Reaction C, then K_cReaction C = __________.

Correct Answer
verified
K_cReaction ...
View Answer

Correct Answer
verified

Correct Answer
verified
True

At 27°C, K_p = 0.095 for the equilibrium: NH₄HS (s) NH₃(g) + H₂S (g) A sample of solid NH₄HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH₄HS remains.

Correct Answer
verified

Consider the following reaction at equilibrium: 2SO₂ (g) + O₂ (g) 2SO₃ (g) ΔH° = -99 kJ Le Châtelier's principle predicts that an increase in temperature will result in __________.

Correct Answer
verified

Consider the following reaction at equilibrium: 2CO₂ (g) 2CO (g) + O₂ (g) ΔH° = -514 kJ Le Châtelier's principle predicts that adding O₂ (g) to the reaction container will __________.

Correct Answer
verified

The equilibrium constant (K_p) for the interconversion of PCl₅ and PCl₃ is 0.0121: PCl₅ (g) PCl₃ (g) + Cl₂ (g) A vessel is charged with PCl₅, giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl₃ is __________ atm.

Correct Answer
verified