Question 1

Which of the following statements is TRUE?

Accepted Answer

A) Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction. 
B) The equilibrium constant for the forward reaction is equal to the equilibrium constant for the reverse reaction. 
C) A reaction quotient (Q)larger than the equilibrium constant (K)means that the reaction will favour the production of more products. 
D) Dynamic equilibrium indicates that the amount of reactants and products are equal. 
E) Dynamic equilibrium is established when K = 0. 
A) Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction. 
B) The equilibrium constant for the forward reaction is equal to the equilibrium constant for the reverse reaction. 
C) A reaction quotient (Q)larger than the equilibrium constant (K)means that the reaction will favour the production of more products. 
D) Dynamic equilibrium indicates that the amount of reactants and products are equal. 
E) Dynamic equilibrium is established when K = 0.

Question 2

Express the equilibrium constant for the following reaction: 
$\quad$$\quad$2Na(s)+ 2H2O(l)? 2NaOH(aq)+ H2(g)

Accepted Answer

A) 
Kc = $\frac { [ \mathrm { NaOH } ] ^ { 2 } \left[ \mathrm { H } _ { 2 } \right] } { [ \mathrm { Na } ] ^ { 2 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 2 } }$ 
B) 
Kc = [H2][NaOH]-2 
C) 
Kc = $\frac { [ \mathrm { Na } ] ^ { 2 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 2 } } { [ \mathrm { NaOH } ] ^ { 2 } \left[ \mathrm { H } _ { 2 } \right] }$ 
D) Kc = [H2][NaOH]2 
E) 
Kc = $\frac { [ \mathrm { NaOH } ] ^ { 1 / 2 } \left[ \mathrm { H } _ { 2 } \right] } { [ \mathrm { Na } ] ^ { 1 / 2 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 1 / 2 } }$ 
A) 
Kc = $\frac { [ \mathrm { NaOH } ] ^ { 2 } \left[ \mathrm { H } _ { 2 } \right] } { [ \mathrm { Na } ] ^ { 2 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 2 } }$ 
B) 
Kc = [H2][NaOH]-2 
C) 
Kc = $\frac { [ \mathrm { Na } ] ^ { 2 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 2 } } { [ \mathrm { NaOH } ] ^ { 2 } \left[ \mathrm { H } _ { 2 } \right] }$ 
D) Kc = [H2][NaOH]2 
E) 
Kc = $\frac { [ \mathrm { NaOH } ] ^ { 1 / 2 } \left[ \mathrm { H } _ { 2 } \right] } { [ \mathrm { Na } ] ^ { 1 / 2 } \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] ^ { 1 / 2 } }$

Question 3

The following reaction is exothermic.Which change will shift the equilibrium to the left? 
2SO2(g)+ O2(g)⇌ 2SO3(g)

Accepted Answer

A) lowering the temperature 
B) increasing the pressure 
C) increasing the volume 
D) none of the above 
A) lowering the temperature 
B) increasing the pressure 
C) increasing the volume 
D) none of the above

Question 4

At a certain temperature,nitogen and hydrogen react to form ammonia: 
$\quad$N2(g)+ 3H2(g)⇌ 2NH3(g)
When initial amounts of N2,H2,and NH3 are mixed,the concentration of NH3 increases.Which statement below is TRUE?

Accepted Answer

A) Kc c > Q 
C) Kc = Q 
D) Kc = Q = 0 
A) Kc c > Q 
C) Kc = Q 
D) Kc = Q = 0

Question 5

Consider the following reaction,equilibrium pressures,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of CO. 
$\quad$$\quad$CO(g)+ 2H2(g)⇌ CH3OH(l)$\quad$$\quad$Kp = 2.25 × 104 bar-3
$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ P(H2)eq = 0.52 bar

Accepted Answer

A) 8.3 × 104 bar 
B) 1.2 × 10-5 bar 
C) 6.25 × 10-3 bar 
D) 8.5 × 10-5 bar 
E) 1.6 × 10-4 bar 
A) 8.3 × 104 bar 
B) 1.2 × 10-5 bar 
C) 6.25 × 10-3 bar 
D) 8.5 × 10-5 bar 
E) 1.6 × 10-4 bar

Question 6

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

Accepted Answer

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

Question 7

Consider the following reaction: 
NO(g)+ SO3(g)⇌ NO2(g)+ SO2(g)
A reaction mixture initially contains 2.0 bar NO2 and 1.0 bar SO2.Determine the equilibrium pressure of SO2 if Kp for the reaction at this temperature is 0.0118.

Accepted Answer

A) 0.011 bar 
B) 0.037 bar 
C) 0.10 bar 
D) 0.0038 bar 
E) 0.067 bar 
A) 0.011 bar 
B) 0.037 bar 
C) 0.10 bar 
D) 0.0038 bar 
E) 0.067 bar

Question 8

Consider the following reaction: 
COCl2(g)⇌ CO(g)+ Cl2(g)
A reaction mixture initially contains 1.6 mol L-1 COCl2.Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is 8.33 × 10-4 M.Calculate this based on the assumption that the answer is negligible compared to 1.6.

Accepted Answer

A) 4.2 × 10-4 mol L-1 
B) 1.5 × 10-3 mol L-1 
C) 3.7 × 10-2 mol L-1 
D) 2.1 × 10-2 mol L-1 
E) 1.3 × 10-3 mol L-1 
A) 4.2 × 10-4 mol L-1 
B) 1.5 × 10-3 mol L-1 
C) 3.7 × 10-2 mol L-1 
D) 2.1 × 10-2 mol L-1 
E) 1.3 × 10-3 mol L-1

Question 9

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 mol L-1,[I2]eq = 0.39 mol L-1,[HI]eq = 1.6 mol L-1. 
$\quad$$\quad$H2(g)+ I2(g)⇌ 2HI(g)

Accepted Answer

A) 2.1 × 10-2 
B) 29 
C) 47 
D) 3.4 × 10-2 
E) 8.7 × 10-2 
A) 2.1 × 10-2 
B) 29 
C) 47 
D) 3.4 × 10-2 
E) 8.7 × 10-2

Question 10

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 mol L-1,[HI]eq = 5.6 × 10-16 mol L-1,[Cl2]eq = 0.0019 mol L-1. 
$\quad$$\quad$2HCl(g)+ I2(s)⇌ 2HI(g)+ Cl2(g)

Accepted Answer

A) 8.2 × 10-18 M 
B) 2.9 × 1031 M 
C) 1.2 × 1017 M 
D) 1.4 × 10-19 M 
E) 3.5 × 10-32 M 
A) 8.2 × 10-18 M 
B) 2.9 × 1031 M 
C) 1.2 × 1017 M 
D) 1.4 × 10-19 M 
E) 3.5 × 10-32 M

Question 11

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H2O(g). 
$\quad$$\quad$C2H4(g)+ H2O(g)⇌ C2H5OH(g)Kc = 9.0 × 103 M-1
$\quad$$\quad$[C2H4]eq = 0.015 mol L-1 $\quad$$\quad$[C2H5OH]eq = 1.69 mol L-1

Accepted Answer

A) 9.9 × 10-7 mol L-1 
B) 80.mol L-1 
C) 1.0 mol L-1 
D) 1.68 mol L-1 
E) 0.013 mol L-1 
A) 9.9 × 10-7 mol L-1 
B) 80.mol L-1 
C) 1.0 mol L-1 
D) 1.68 mol L-1 
E) 0.013 mol L-1

Question 12

The equilibrium constant is equal to 5.00 L mol-1 at 1300 K for the reaction: 2SO2(g)+ O2(g)⇌ 2SO3(g)
If initial concentrations are [SO2] = 6.00 mol L-1,[O2] = 0.45 mol L-1,and [SO3] = 9.00 mol L-1,the system is

Accepted Answer

A) at equilibrium. 
B) not at equilibrium and will remain in an unequilibrated state. 
C) not at equilibrium and will shift to the left to achieve an equilibrium state. 
D) not at equilibrium and will shift to the right to achieve an equilibrium state. 
A) at equilibrium. 
B) not at equilibrium and will remain in an unequilibrated state. 
C) not at equilibrium and will shift to the left to achieve an equilibrium state. 
D) not at equilibrium and will shift to the right to achieve an equilibrium state.

Question 13

Consider the following reaction and its equilibrium constant: 
I2(g)⇌ 2I(g)$\quad$$\quad$Kp = 0.209 atm
A reaction mixture contains 0.89 atm I2 and 1.77 atm I.Which of the following statements is TRUE concerning this system?

Accepted Answer

A) The reaction will shift in the direction of reactants. 
B) The reaction quotient will increase. 
C) The reaction will shift in the direction of products. 
D) The equilibrium constant will decrease. 
E) The system is at equilibrium. 
A) The reaction will shift in the direction of reactants. 
B) The reaction quotient will increase. 
C) The reaction will shift in the direction of products. 
D) The equilibrium constant will decrease. 
E) The system is at equilibrium.

Question 14

Consider the following reaction and its equilibrium constant: 
4CuO(s)+ CH4(g)⇌ CO2(g)+ 4Cu(s)+ 2H2O(g)Kc = 1.10
A reaction mixture contains 0.22 mol L-1 CH4,0.67 mol L-1 CO2 and 1.3 mol L-1 H2O.Which of the following statements is TRUE concerning this system?

Accepted Answer

A) The reaction will shift in the direction of products. 
B) The equilibrium constant will increase. 
C) The reaction quotient will increase. 
D) The reaction will shift in the direction of reactants. 
E) The system is at equilibrium. 
A) The reaction will shift in the direction of products. 
B) The equilibrium constant will increase. 
C) The reaction quotient will increase. 
D) The reaction will shift in the direction of reactants. 
E) The system is at equilibrium.

Question 15

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. 
$\quad$A(g)+ B(g)⇌ AB$\quad$$\quad$(g)K = 0.24
$\quad$AB(g)+ A(g)⇌ A2B$\quad$(g)K = 3.8
$\quad$2A(g)+ B(g)⇌ A2B$\quad$ (g)K = ?

Accepted Answer

A) 4.0 
B) 0.91 
C) 3.6 
D) 16 
E) 0.63 
A) 4.0 
B) 0.91 
C) 3.6 
D) 16 
E) 0.63

Question 16

Consider the following reaction at equilibrium.What effect will increasing the temperature have on the system? 
C3H8(g)+ 5O2(g)⇌ 3CO2(g)+ 4H2O(l)ΔrH° = -2220 kJ

Accepted Answer

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

Question 17

Express the equilibrium constant for the following reaction: 
$\quad$$\quad$B(OH)3(aq) + 2H2O(l)? B(OH)3(OH)-(aq)+ H3O+(aq)

Accepted Answer

A) Kc = $\frac { \left[ \mathrm { H } _ { 3 } \mathrm { O } ^ { + } \right] \times \left[ \mathrm { B } ( \mathrm { OH } ) _ { 3 } ( \mathrm { OH } ) ^ { - } \right] } { \left[ \mathrm { B } ( \mathrm { OH } ) _ { 3 } \right] \times \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] }$ 
B) Kc = $\left[ \mathrm { B } ( \mathrm { OH } ) _ { 3 } \right]$
$\left[ \mathrm { H } _ { 3 } \mathrm { O } ^ { + } \right] \times \left[ \mathrm { B } ( \mathrm { OH } ) _ { 3 } ( \mathrm { OH } ) ^ { - } \right]$

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

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

Question 18

For the reaction: N2(g)+ 2O2(g)⇌ 2NO2(g),Kc = 8.3 × 10-10 M-1 at 25 °C.What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?

Accepted Answer

A) 3.3 × 10-11 mol L-1 
B) 1.7 × 10-10 mol L-1 
C) 6.0 × 109 mol L-1 
D) 3.0 × 1010 mol L-1 
A) 3.3 × 10-11 mol L-1 
B) 1.7 × 10-10 mol L-1 
C) 6.0 × 109 mol L-1 
D) 3.0 × 1010 mol L-1

Question 19

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO2(g). 
$\quad$$\quad$NH2COONH4(s)⇌ 2NH3(g)+ CO2(g)$\quad$Kc = 1.58 × 10-8 M3
$\quad$$\quad$[NH3]eq = 2.9 × 10-3 mol L-1

Accepted Answer

A) 0.053 mol L-1 
B) 4.6 × 10-11 mol L-1 
C) 1.9 × 10-3 mol L-1 
D) 5.4 × 10-6 mol L-1 
E) 0.022 mol L-1 
A) 0.053 mol L-1 
B) 4.6 × 10-11 mol L-1 
C) 1.9 × 10-3 mol L-1 
D) 5.4 × 10-6 mol L-1 
E) 0.022 mol L-1

Question 20

Calculate P (NO)eq,if P(NOCl)eq = 0.33 bar,P(Cl2)eq = 0.50 bar,and Kp = 1.9 × 10-2 bar . 
$\quad$$\quad$2NOCl(g)⇌ 2NO(g)+ Cl2(g)

Accepted Answer

A) 1.7 bar 
B) 0.0042 bar 
C) 0.30 bar 
D) 0.064 bar 
E) 0.087 bar 
A) 1.7 bar 
B) 0.0042 bar 
C) 0.30 bar 
D) 0.064 bar 
E) 0.087 bar

Exam 14: Chemical Equilibrium

Which of the following statements is TRUE?

Express the equilibrium constant for the following reaction: \quad\quad 2Na(s)+ 2H2O(l)? 2NaOH(aq)+ H2(g)

The following reaction is exothermic.Which change will shift the equilibrium to the left? 2SO2(g)+ O2(g)⇌ 2SO3(g)

At a certain temperature,nitogen and hydrogen react to form ammonia: \quad N2(g)+ 3H2(g)⇌ 2NH3(g) When initial amounts of N2,H2,and NH3 are mixed,the concentration of NH3 increases.Which statement below is TRUE?

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

Consider the following reaction: NO(g)+ SO3(g)⇌ NO2(g)+ SO2(g) A reaction mixture initially contains 2.0 bar NO2 and 1.0 bar SO2.Determine the equilibrium pressure of SO2 if Kp for the reaction at this temperature is 0.0118.

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 mol L-1,[I2]eq = 0.39 mol L-1,[HI]eq = 1.6 mol L-1. \quad\quad H2(g)+ I2(g)⇌ 2HI(g)

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [HCl]eq = 0.13 mol L-1,[HI]eq = 5.6 × 10-16 mol L-1,[Cl2]eq = 0.0019 mol L-1. \quad\quad 2HCl(g)+ I2(s)⇌ 2HI(g)+ Cl2(g)

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H2O(g). \quad\quad C2H4(g)+ H2O(g)⇌ C2H5OH(g)Kc = 9.0 × 103 M-1 \quad\quad [C2H4]eq = 0.015 mol L-1 \quad\quad [C2H5OH]eq = 1.69 mol L-1

The equilibrium constant is equal to 5.00 L mol-1 at 1300 K for the reaction: 2SO2(g)+ O2(g)⇌ 2SO3(g) If initial concentrations are [SO2] = 6.00 mol L-1,[O2] = 0.45 mol L-1,and [SO3] = 9.00 mol L-1,the system is

Consider the following reaction and its equilibrium constant: I2(g)⇌ 2I(g) \quad\quad Kp = 0.209 atm A reaction mixture contains 0.89 atm I2 and 1.77 atm I.Which of the following statements is TRUE concerning this system?

Consider the following reaction and its equilibrium constant: 4CuO(s)+ CH4(g)⇌ CO2(g)+ 4Cu(s)+ 2H2O(g)Kc = 1.10 A reaction mixture contains 0.22 mol L-1 CH4,0.67 mol L-1 CO2 and 1.3 mol L-1 H2O.Which of the following statements is TRUE concerning this system?

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. \quad A(g)+ B(g)⇌ AB \quad\quad (g)K = 0.24 \quad AB(g)+ A(g)⇌ A2B \quad (g)K = 3.8 \quad 2A(g)+ B(g)⇌ A2B \quad (g)K = ?

Consider the following reaction at equilibrium.What effect will increasing the temperature have on the system? C3H8(g)+ 5O2(g)⇌ 3CO2(g)+ 4H2O(l)ΔrH° = -2220 kJ

Express the equilibrium constant for the following reaction: \quad\quad B(OH)3(aq) + 2H2O(l)? B(OH)3(OH)-(aq)+ H3O+(aq)

For the reaction: N2(g)+ 2O2(g)⇌ 2NO2(g),Kc = 8.3 × 10-10 M-1 at 25 °C.What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO2(g). \quad\quad NH2COONH4(s)⇌ 2NH3(g)+ CO2(g) \quad Kc = 1.58 × 10-8 M3 \quad\quad [NH3]eq = 2.9 × 10-3 mol L-1

Calculate P (NO)eq,if P(NOCl)eq = 0.33 bar,P(Cl2)eq = 0.50 bar,and Kp = 1.9 × 10-2 bar . \quad\quad 2NOCl(g)⇌ 2NO(g)+ Cl2(g)

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

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

Liquids, solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Express the equilibrium constant for the following reaction: $\quad$ $\quad$ 2Na(s)+ 2H₂O(l)? 2NaOH(aq)+ H₂(g)

The following reaction is exothermic.Which change will shift the equilibrium to the left? 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)

At a certain temperature,nitogen and hydrogen react to form ammonia: $\quad$ N₂(g)+ 3H₂(g)⇌ 2NH₃(g) When initial amounts of N₂,H₂,and NH₃ are mixed,the concentration of NH₃ increases.Which statement below is TRUE?

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

Consider the following reaction: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g) A reaction mixture initially contains 2.0 bar NO₂ and 1.0 bar SO₂.Determine the equilibrium pressure of SO₂ if K_p for the reaction at this temperature is 0.0118.

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 mol L^-1,[I₂]_eq = 0.39 mol L^-1,[HI]_eq = 1.6 mol L^-1. $\quad$ $\quad$ H₂(g)+ I₂(g)⇌ 2HI(g)

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [HCl]_eq = 0.13 mol L^-1,[HI]_eq = 5.6 × 10^-16 mol L^-1,[Cl₂]_eq = 0.0019 mol L^-1. $\quad$ $\quad$ 2HCl(g)+ I₂(s)⇌ 2HI(g)+ Cl₂(g)

The equilibrium constant is equal to 5.00 L mol^-1 at 1300 K for the reaction: 2SO₂(g)+ O₂(g)⇌ 2SO₃(g) If initial concentrations are [SO₂] = 6.00 mol L^-1,[O₂] = 0.45 mol L^-1,and [SO₃] = 9.00 mol L^-1,the system is

Consider the following reaction and its equilibrium constant: I₂(g)⇌ 2I(g) $\quad$ $\quad$ K_p = 0.209 atm A reaction mixture contains 0.89 atm I₂ and 1.77 atm I.Which of the following statements is TRUE concerning this system?

Consider the following reaction and its equilibrium constant: 4CuO(s)+ CH₄(g)⇌ CO₂(g)+ 4Cu(s)+ 2H₂O(g)K_c = 1.10 A reaction mixture contains 0.22 mol L^-1 CH₄,0.67 mol L^-1 CO₂and 1.3 mol L^-1 H₂O.Which of the following statements is TRUE concerning this system?

The equilibrium constant is given for two of the reactions below.Determine the value of the missing equilibrium constant. $\quad$ A(g)+ B(g)⇌ AB $\quad$ $\quad$ (g)K = 0.24 $\quad$ AB(g)+ A(g)⇌ A₂B $\quad$ (g)K = 3.8 $\quad$ 2A(g)+ B(g)⇌ A₂B $\quad$ (g)K = ?

Consider the following reaction at equilibrium.What effect will increasing the temperature have on the system? C₃H₈(g)+ 5O₂(g)⇌ 3CO₂(g)+ 4H₂O(l)Δ_rH° = -2220 kJ

Express the equilibrium constant for the following reaction: $\quad$ $\quad$ B(OH)₃(aq)+ 2H₂O(l)? B(OH)₃(OH)^-(aq)+ H₃O⁺(aq)

For the reaction: N₂(g)+ 2O₂(g)⇌ 2NO₂(g),K_c = 8.3 × 10^-10 M^-1at 25 °C.What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

Calculate P (NO)_eq,if P(NOCl)_eq = 0.33 bar,P(Cl₂)_eq = 0.50 bar,and K_p = 1.9 × 10^-2 bar . $\quad$ $\quad$ 2NOCl(g)⇌ 2NO(g)+ Cl₂(g)