Question 1

How will equilibrium be affected for a reaction having the same number of moles of gaseous reactants and products if the pressure is increased?

Accepted Answer

There will

Question 2

An equilibrium mixture of CO,O2,and CO2 at a certain temperature contains 0.0010 mol L-1 CO2 and 0.0015 mol L-1 O2.At this temperature,Kc equals 1.4 × 102 L mol-1 for the reaction: 2CO(g)+ O2(g)⇌ 2CO2(g)
What is the equilibrium concentration of CO?

Accepted Answer

A) 4.8 × 10-6 mol L-1 
B) 8.5 × 10-3 mol L-1 
C) 9.3 × 10-2 mol L-1 
D) 3.1 × 10-1 mol L-1 
A) 4.8 × 10-6 mol L-1 
B) 8.5 × 10-3 mol L-1 
C) 9.3 × 10-2 mol L-1 
D) 3.1 × 10-1 mol L-1

Question 3

At a certain temperature the equilibrium constant,Kc,equals 0.11 for the reaction: 
$\quad$$\quad$$\quad$2ICl(g)⇌ I2(g)+ Cl2(g)
What is the equilibrium concentration of ICl if 0.75 mol of I2 and 0.75 mol of Cl2 are initially mixed in a 2.0 L flask?

Accepted Answer

A) 0.23 mol L-1 
B) 0.28 mol L-1 
C) 0.225 mol L-1 
D) 0.56 mol L-1 
A) 0.23 mol L-1 
B) 0.28 mol L-1 
C) 0.225 mol L-1 
D) 0.56 mol L-1

Question 4

Express the equilibrium constant for the following reaction: 
P(g)+ 3/2 Cl2(g)? PCl3(g)

Accepted Answer

A) $K P = \frac { \mathrm { P } ^ { 2 } \left( \mathrm { PCl } _ { 3 } \right) } { \mathrm { P } ^ { 2 } ( \mathrm { P } ) \times \mathrm { P } ^ { 3 } \left( \mathrm { Cl } _ { 2 } \right) }$ 
B) $K P = \frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { PCl } _ { 3 } \right) } { \mathrm { P } ^ { 1 / 2 } ( \mathrm { P } ) \times \mathrm { P } ^ { 1 / 3 } \left( \mathrm { Cl } _ { 2 } \right) }$ 
C) $K P = \frac { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) } { \mathrm { P } ( \mathrm { P } ) \times \mathrm { P } ^ { 3 / 2 } \left( \mathrm { Cl } _ { 2 } \right) }$ 
D) $K P = \frac { \mathrm { P } ^ { 2 } ( \mathrm { P } ) \times \mathrm { P } ^ { 3 } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { PCl } _ { 3 } \right) }$ 
E) $K p = \frac { \mathrm { P } ( \mathrm { P } ) \times \mathrm { P } ^ { 3 / 2}  \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) }$ 
A) $K P = \frac { \mathrm { P } ^ { 2 } \left( \mathrm { PCl } _ { 3 } \right) } { \mathrm { P } ^ { 2 } ( \mathrm { P } ) \times \mathrm { P } ^ { 3 } \left( \mathrm { Cl } _ { 2 } \right) }$ 
B) $K P = \frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { PCl } _ { 3 } \right) } { \mathrm { P } ^ { 1 / 2 } ( \mathrm { P } ) \times \mathrm { P } ^ { 1 / 3 } \left( \mathrm { Cl } _ { 2 } \right) }$ 
C) $K P = \frac { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) } { \mathrm { P } ( \mathrm { P } ) \times \mathrm { P } ^ { 3 / 2 } \left( \mathrm { Cl } _ { 2 } \right) }$ 
D) $K P = \frac { \mathrm { P } ^ { 2 } ( \mathrm { P } ) \times \mathrm { P } ^ { 3 } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { PCl } _ { 3 } \right) }$ 
E) $K p = \frac { \mathrm { P } ( \mathrm { P } ) \times \mathrm { P } ^ { 3 / 2}  \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) }$

Question 5

Consider the following reaction: 
Xe(g)+ 2F2(g)⇌ XeF4(g)
A reaction mixture initially contains 2.24 bar Xe and 4.27 bar F2.If the equilibrium pressure of Xe is 0.34 bar,find the equilibrium constant (Kp)for the reaction.

Accepted Answer

A) 25 bar-2 
B) 0.12 bar-2 
C) 0.99 bar-2 
D) 8.3 bar-2 
E) 0.040 bar-2 
A) 25 bar-2 
B) 0.12 bar-2 
C) 0.99 bar-2 
D) 8.3 bar-2 
E) 0.040 bar-2

Question 6

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 
2H2S(g)+ 3O2(g)⇌ 2H2O(g)+ 2SO2(g)

Accepted Answer

A) The reaction will shift in the direction of products. 
B) No effect will be observed. 
C) The reaction will shift in the direction of reactants. 
D) The equilibrium constant will decrease. 
E) The equilibrium constant will increase. 
A) The reaction will shift in the direction of products. 
B) No effect will be observed. 
C) The reaction will shift in the direction of reactants. 
D) The equilibrium constant will decrease. 
E) The equilibrium constant will increase.

Question 7

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.5 mol L-1,[H2]eq = 1.1 mol L-1,[NH3]eq = 0.47 mol L-1. 
$\quad$$\quad$N2(g)+ 3H2(g)⇌ 2NH3(g)

Accepted Answer

A) 3.5 M-2 
B) 0.28 M-2 
C) 9.1 M-2 
D) 0.11 M-2 
E) 0.78 M-2 
A) 3.5 M-2 
B) 0.28 M-2 
C) 9.1 M-2 
D) 0.11 M-2 
E) 0.78 M-2

Question 8

Consider the following reaction at equilibrium.What effect will adding 1 mole of Ar to the reaction mixture have on the system? 
2H2S(g)+ 3O2(g)⇌ 2H2O(g)+ 2SO2(g)

Accepted Answer

A) The reaction will shift in the direction of products. 
B) No effect will be observed. 
C) The reaction will shift in the direction of reactants. 
D) The equilibrium constant will decrease. 
E) The equilibrium constant will increase. 
A) The reaction will shift in the direction of products. 
B) No effect will be observed. 
C) The reaction will shift in the direction of reactants. 
D) The equilibrium constant will decrease. 
E) The equilibrium constant will increase.

Question 9

Can the Kp and Kc for a reaction ever have the same value? Why or why not?

Accepted Answer

Yes,they can have the same value.Since K

Question 10

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. 
$\quad$A(g)+ 2B(g)⇌ AB2$\quad$ (g)Kc = 59
$\quad$AB2(g)+ B(g)⇌ AB3$\quad$(g)Kc = ?
$\quad$A(g)+ 3B(g)⇌ AB3$\quad$ (g)Kc = 478

Accepted Answer

A) 3.5 × 10-5 
B) 2.8 × 104 
C) 8.1 
D) 0.12 
E) 89 
A) 3.5 × 10-5 
B) 2.8 × 104 
C) 8.1 
D) 0.12 
E) 89

Question 11

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. 
$\quad$2HD(g)⇌ H2(g)+ D2$\quad$ (g)K = 0.28
$\quad$2H2(g)+ 2D2(g)⇌ 4HD$\quad$(g)K = ?

Accepted Answer

A) 7.8 × 10-2 
B) 3.6 
C) 0.53 
D) 13 
E) 1.9 
A) 7.8 × 10-2 
B) 3.6 
C) 0.53 
D) 13 
E) 1.9

Question 12

Consider the following reaction at equilibrium.What effect will removing H2O have on the system? 
2H2S(g)+ 3O2(g)⇌ 2H2O(g)+ 2SO2(g)

Accepted Answer

A) The reaction will shift to the left. 
B) No change will be observed. 
C) The equilibrium constant will decrease. 
D) The equilibrium constant will increase. 
E) The reaction will shift in the direction of products. 
A) The reaction will shift to the left. 
B) No change will be observed. 
C) The equilibrium constant will decrease. 
D) The equilibrium constant will increase. 
E) The reaction will shift in the direction of products.

Question 13

Consider the following reaction: 
2H2O(g)+ 2SO2(g)⇌ 2H2S(g)+ 3O2(g)
A reaction mixture initially contains 2.8 mol L-1 H2O and 2.6 mol L-1 SO2.Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6 mol L-1.

Accepted Answer

A) 0.045 mol L-1 
B) 0.058 mol L-1 
C) 0.028 mol L-1 
D) 3.1 × 10-3 mol L-1 
E) 0.12 mol L-1 
A) 0.045 mol L-1 
B) 0.058 mol L-1 
C) 0.028 mol L-1 
D) 3.1 × 10-3 mol L-1 
E) 0.12 mol L-1

Question 14

Express the equilibrium constant for the following reaction: 
$\mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) _ { 6 } ^ { 3 + } \underset { ( a q ) } { 3 + } + 6 \mathrm { CN } - ( a q ) = \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \underset { ( a q ) } { 3 - } + 6 \mathrm { H } _ { 2 } \mathrm { O } ( l )$

Accepted Answer

A) Kc = $\frac { \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \right] } { \left[ \mathrm { CN } ^ { - } \right] ^ { 6 } \times \left[ \mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) 6 ^ { 3 + } \right] }$ 
B) Kc = $\frac { \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \right] \times \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 6 } } { \left[ \mathrm { CN } ^ { - } \right] ^ { 6 } \times \left[ \mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) _ { 6 } ^ { 3 + } \right] }$ 
C) Kc = $\frac { \left[ \mathrm { CN } ^ { - } \right] ^ { 6 } \times \left[ \mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) 6 ^ { 3 + } \right] } { \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \right] }$ 
D) Kc = $\frac { \left[ \mathrm { CN } ^ { - } \right] ^ { 6 } \times \left[ \mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) 6 ^ { 3 + } \right] } { \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \right] \times \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 6 } }$ 
E) Kc = $\frac { \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \right] ^ { 3 } } { \left[ \mathrm { CN } ^ { - } \right] ^ { 6 } \times \left[ \mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) _ { 6 } ^ { 3 + } \right] ^ { 3 } }$ 
A) Kc = $\frac { \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \right] } { \left[ \mathrm { CN } ^ { - } \right] ^ { 6 } \times \left[ \mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) 6 ^ { 3 + } \right] }$ 
B) Kc = $\frac { \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \right] \times \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 6 } } { \left[ \mathrm { CN } ^ { - } \right] ^ { 6 } \times \left[ \mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) _ { 6 } ^ { 3 + } \right] }$ 
C) Kc = $\frac { \left[ \mathrm { CN } ^ { - } \right] ^ { 6 } \times \left[ \mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) 6 ^ { 3 + } \right] } { \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \right] }$ 
D) Kc = $\frac { \left[ \mathrm { CN } ^ { - } \right] ^ { 6 } \times \left[ \mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) 6 ^ { 3 + } \right] } { \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \right] \times \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 6 } }$ 
E) Kc = $\frac { \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } ^ { 3 - } \right] ^ { 3 } } { \left[ \mathrm { CN } ^ { - } \right] ^ { 6 } \times \left[ \mathrm { Fe } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) _ { 6 } ^ { 3 + } \right] ^ { 3 } }$

Question 15

Consider the following reaction: 
CO2(g)+ C(graphite)⇌ 2CO(g)
A reaction mixture initially contains 0.56 bar CO2 and 0.32 bar CO.Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is 2.25 bar.

Accepted Answer

A) 0.83 bar 
B) 0.31 bar 
C) 0.26 bar 
D) 0.58 bar 
E) 0.42 bar 
A) 0.83 bar 
B) 0.31 bar 
C) 0.26 bar 
D) 0.58 bar 
E) 0.42 bar

Question 16

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl)eq = 0.22 atm,P(NO)eq = 0.10 atm,P(Cl2)eq = 0.081 atm. 
$\quad$$\quad$2NOCl(g)⇌ 2NO(g)+ Cl2(g)

Accepted Answer

A) 3.7 × 10-2 atm 
B) 60 atm 
C) 27 atm 
D) 1.7 × 10-2 atm 
E) 1.8 × 10-3 atm 
A) 3.7 × 10-2 atm 
B) 60 atm 
C) 27 atm 
D) 1.7 × 10-2 atm 
E) 1.8 × 10-3 atm

Question 17

Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? 
Xe(g)+ 2F2(g)⇌ XeF4(g)

Accepted Answer

A) The reaction will shift to the left in the direction of reactants. 
B) The equilibrium constant will increase. 
C) No effect will be observed. 
D) The reaction will shift to the right in the direction of products. 
E) The equilibrium constant will decrease. 
A) The reaction will shift to the left in the direction of reactants. 
B) The equilibrium constant will increase. 
C) No effect will be observed. 
D) The reaction will shift to the right in the direction of products. 
E) The equilibrium constant will decrease.

Question 18

The reaction below has a Kc value of 1.0 × 1012 M-1.What is the value of Kp for this reaction at 500 K? 
$\quad$2SO2(g)+ O2(g)⇌ 2SO3(g)

Accepted Answer

A) 4.2 × 10-11 bar-1 
B) 1.0 × 1012 bar-1 
C) 2.4 × 10-12 bar-1 
D) 4.1 × 1013 bar-1 
E) 2.4 × 1010 bar-1 
A) 4.2 × 10-11 bar-1 
B) 1.0 × 1012 bar-1 
C) 2.4 × 10-12 bar-1 
D) 4.1 × 1013 bar-1 
E) 2.4 × 1010 bar-1

Question 19

Express the equilibrium constant for the following reaction: 
N2(g)+ 3H2(g)? 2NH3(g)

Accepted Answer

A) KP = $\frac { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P }^{ 1 / 3 }\left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^{1 / 2 }\left( \mathrm { NH } _ { 3 } \right) }$ 
B) KP = $\frac { \mathrm { P } ^ { 6 } \left( \mathrm { NH } _ { 3 } \right) } { \mathrm { P } ^ { 3 } \left( \mathrm {~N} _ { 2 } \right) \times \mathrm { P } ^ { 9 } \left( \mathrm { H } _ { 2 } \right) }$ 
C) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { NH } _ { 3 } \right) } { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 3 } \left( \mathrm { H } _ { 2 } \right) }$ 
D) KP= $\frac { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 3 } \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { NH } _ { 3 } \right) }$ 
E) KP = $\frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { NH } _ { 3 } \right) } { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 1 / 3 } \left( \mathrm { H } _ { 2 } \right) }$ 
A) KP = $\frac { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P }^{ 1 / 3 }\left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^{1 / 2 }\left( \mathrm { NH } _ { 3 } \right) }$ 
B) KP = $\frac { \mathrm { P } ^ { 6 } \left( \mathrm { NH } _ { 3 } \right) } { \mathrm { P } ^ { 3 } \left( \mathrm {~N} _ { 2 } \right) \times \mathrm { P } ^ { 9 } \left( \mathrm { H } _ { 2 } \right) }$ 
C) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { NH } _ { 3 } \right) } { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 3 } \left( \mathrm { H } _ { 2 } \right) }$ 
D) KP= $\frac { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 3 } \left( \mathrm { H } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { NH } _ { 3 } \right) }$ 
E) KP = $\frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { NH } _ { 3 } \right) } { \mathrm { P } \left( \mathrm { N } _ { 2 } \right) \times \mathrm { P } ^ { 1 / 3 } \left( \mathrm { H } _ { 2 } \right) }$

Question 20

For the following reaction,what is Δn required in the conversion of Kc to Kp? 
$\quad$$\quad$N2(g)+ 3H2(g)⇌ 2NH3(g)

Accepted Answer

A) 4 
B) -4 
C) -2 
D) 2 
E) 1 
A) 4 
B) -4 
C) -2 
D) 2 
E) 1

Exam 14: Chemical Equilibrium

How will equilibrium be affected for a reaction having the same number of moles of gaseous reactants and products if the pressure is increased?

An equilibrium mixture of CO,O2,and CO2 at a certain temperature contains 0.0010 mol L-1 CO2 and 0.0015 mol L-1 O2.At this temperature,Kc equals 1.4 × 102 L mol-1 for the reaction: 2CO(g)+ O2(g)⇌ 2CO2(g) What is the equilibrium concentration of CO?

At a certain temperature the equilibrium constant,Kc,equals 0.11 for the reaction: \quad\quad\quad 2ICl(g)⇌ I2(g)+ Cl2(g) What is the equilibrium concentration of ICl if 0.75 mol of I2 and 0.75 mol of Cl2 are initially mixed in a 2.0 L flask?

Express the equilibrium constant for the following reaction: P(g)+ 3/2 Cl2(g)? PCl3(g)

Consider the following reaction: Xe(g)+ 2F2(g)⇌ XeF4(g) A reaction mixture initially contains 2.24 bar Xe and 4.27 bar F2.If the equilibrium pressure of Xe is 0.34 bar,find the equilibrium constant (Kp)for the reaction.

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 2H2S(g)+ 3O2(g)⇌ 2H2O(g)+ 2SO2(g)

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 1.5 mol L-1,[H2]eq = 1.1 mol L-1,[NH3]eq = 0.47 mol L-1. \quad\quad N2(g)+ 3H2(g)⇌ 2NH3(g)

Consider the following reaction at equilibrium.What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H2S(g)+ 3O2(g)⇌ 2H2O(g)+ 2SO2(g)

Can the Kp and Kc for a reaction ever have the same value? Why or why not?

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. \quad A(g)+ 2B(g)⇌ AB2 \quad (g)Kc = 59 \quad AB2(g)+ B(g)⇌ AB3 \quad (g)Kc = ? \quad A(g)+ 3B(g)⇌ AB3 \quad (g)Kc = 478

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. \quad 2HD(g)⇌ H2(g)+ D2 \quad (g)K = 0.28 \quad 2H2(g)+ 2D2(g)⇌ 4HD \quad (g)K = ?

Consider the following reaction at equilibrium.What effect will removing H2O have on the system? 2H2S(g)+ 3O2(g)⇌ 2H2O(g)+ 2SO2(g)

Consider the following reaction: 2H2O(g)+ 2SO2(g)⇌ 2H2S(g)+ 3O2(g) A reaction mixture initially contains 2.8 mol L-1 H2O and 2.6 mol L-1 SO2.Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6 mol L-1.

Consider the following reaction: CO2(g)+ C(graphite)⇌ 2CO(g) A reaction mixture initially contains 0.56 bar CO2 and 0.32 bar CO.Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is 2.25 bar.

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(NOCl)eq = 0.22 atm,P(NO)eq = 0.10 atm,P(Cl2)eq = 0.081 atm. \quad\quad 2NOCl(g)⇌ 2NO(g)+ Cl2(g)

Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? Xe(g)+ 2F2(g)⇌ XeF4(g)

The reaction below has a Kc value of 1.0 × 1012 M-1.What is the value of Kp for this reaction at 500 K? \quad 2SO2(g)+ O2(g)⇌ 2SO3(g)

Express the equilibrium constant for the following reaction: N2(g)+ 3H2(g)? 2NH3(g)

For the following reaction,what is Δn required in the conversion of Kc to Kp? \quad\quad N2(g)+ 3H2(g)⇌ 2NH3(g)

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Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Solutions

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Organic Chemistry I: Structures

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Filters

An equilibrium mixture of CO,O₂,and CO₂ at a certain temperature contains 0.0010 mol L^-1 CO₂ and 0.0015 mol L^-1 O₂.At this temperature,K_c equals 1.4 × 10² L mol^-1 for the reaction: 2CO(g)+ O₂(g)⇌ 2CO₂(g) What is the equilibrium concentration of CO?

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: $\quad$ $\quad$ $\quad$ 2ICl(g)⇌ I₂(g)+ Cl₂(g) What is the equilibrium concentration of ICl if 0.75 mol of I₂ and 0.75 mol of Cl₂ are initially mixed in a 2.0 L flask?

Express the equilibrium constant for the following reaction: P(g)+ 3/2 Cl₂(g)? PCl₃(g)

Consider the following reaction: Xe(g)+ 2F₂(g)⇌ XeF₄(g) A reaction mixture initially contains 2.24 bar Xe and 4.27 bar F₂.If the equilibrium pressure of Xe is 0.34 bar,find the equilibrium constant (K_p)for the reaction.

Consider the following reaction at equilibrium.What effect will increasing the pressure of the reaction mixture have on the system? 2H₂S(g)+ 3O₂(g)⇌ 2H₂O(g)+ 2SO₂(g)

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [N₂]_eq = 1.5 mol L^-1,[H₂]_eq = 1.1 mol L^-1,[NH₃]_eq = 0.47 mol L^-1. $\quad$ $\quad$ N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

Consider the following reaction at equilibrium.What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H₂S(g)+ 3O₂(g)⇌ 2H₂O(g)+ 2SO₂(g)

Can the K_p and K_c for a reaction ever have the same value? Why or why not?

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. $\quad$ A(g)+ 2B(g)⇌ AB₂ $\quad$ (g)K_c = 59 $\quad$ AB₂(g)+ B(g)⇌ AB₃ $\quad$ (g)K_c = ? $\quad$ A(g)+ 3B(g)⇌ AB₃ $\quad$ (g)K_c = 478

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. $\quad$ 2HD(g)⇌ H₂(g)+ D₂ $\quad$ (g)K = 0.28 $\quad$ 2H₂(g)+ 2D₂(g)⇌ 4HD $\quad$ (g)K = ?

Consider the following reaction at equilibrium.What effect will removing H₂O have on the system? 2H₂S(g)+ 3O₂(g)⇌ 2H₂O(g)+ 2SO₂(g)

Consider the following reaction: 2H₂O(g)+ 2SO₂(g)⇌ 2H₂S(g)+ 3O₂(g) A reaction mixture initially contains 2.8 mol L^-1 H₂O and 2.6 mol L^-1 SO₂.Determine the equilibrium concentration of H₂S if K_c for the reaction at this temperature is 1.3 × 10^-6mol L^-1.

Consider the following reaction: CO₂(g)+ C(graphite)⇌ 2CO(g) A reaction mixture initially contains 0.56 bar CO₂ and 0.32 bar CO.Determine the equilibrium pressure of CO if K_p for the reaction at this temperature is 2.25 bar.

Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(NOCl)_eq = 0.22 atm,P(NO)_eq = 0.10 atm,P(Cl₂)_eq = 0.081 atm. $\quad$ $\quad$ 2NOCl(g)⇌ 2NO(g)+ Cl₂(g)

Consider the following reaction at equilibrium.What effect will reducing the volume of the reaction mixture have on the system? Xe(g)+ 2F₂(g)⇌ XeF₄(g)

The reaction below has a K_c value of 1.0 × 10¹²M^-1.What is the value of K_p for this reaction at 500 K? $\quad$ 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)

Express the equilibrium constant for the following reaction: N₂(g)+ 3H₂(g)? 2NH₃(g)

For the following reaction,what is Δn required in the conversion of K_c to K_p? $\quad$ $\quad$ N₂(g)+ 3H₂(g)⇌ 2NH₃(g)