Question 1

For the following reaction,what is △n required in the conversion of Kc to Kp? P4(s)+ 5O2(g)⇌ P4O10(s)

Accepted Answer

A) 3 
B) 4 
C) -4 
D) 5 
E) -5 
A) 3 
B) 4 
C) -4 
D) 5 
E) -5

Question 2

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. 
$\quad$N2O4(g)⇌ 2NO2$\quad$ (g)K = 1.46
$\quad$2N2O4(g)⇌ 4NO2$\quad$(g)K = ?

Accepted Answer

A) 2.13 
B) 0.685 
C) 3.11 
D) 1.46 
E) 1.13 
A) 2.13 
B) 0.685 
C) 3.11 
D) 1.46 
E) 1.13

Question 3

In a reaction mixture containing only reactants,what is the value of Q?

Accepted Answer

A) -1 
B) 1 
C) ∞ 
D) 0 
E) Q = K 
A) -1 
B) 1 
C) ∞ 
D) 0 
E) Q = K

Question 4

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO2(g). 
$\quad$N2O4(g)⇌ 2NO2(g)$\quad$$\quad$Kc = 0.21 M
$\quad$[N2O4]eq = 0.068 mol L-1

Accepted Answer

A) 1.9 mol L-1 
B) 0.12 mol L-1 
C) 0.60 mol L-1 
D) 0.028 mol L-1 
E) 0.036 mol L-1 
A) 1.9 mol L-1 
B) 0.12 mol L-1 
C) 0.60 mol L-1 
D) 0.028 mol L-1 
E) 0.036 mol L-1

Question 5

For the following reaction,what is Δn required in the conversion of Kc to Kp? 
$\quad$2SO2(g)+ O2(g)⇌ 2SO3(g)

Accepted Answer

A) 3 
B) -1 
C) -2 
D) 2 
E) 1 
A) 3 
B) -1 
C) -2 
D) 2 
E) 1

Question 6

Phosphorus trichloride and phosphorus pentachloride equilibrate in the presence of molecular chlorine according to the following reaction: $\mathrm { PCl } _ { 3 }$ (g)+ $\mathrm { Cl } _ { 2 }$ (g)? $\mathrm { PCl } _ { 5 }$ (g) An equilibrium mixture at 450 K contains $\mathrm { P } _ { \mathrm { PCl } _ { 3 } }$ = 0.124 bar, $\mathrm { P } _ { \mathrm { Cl } _ { 2 } }$ = 0.157 bar,and $\mathrm { P } _ { \mathrm { PCl } _ { 5 } }$ = 1.30 bar.What is the value of Kp at this temperature?

Accepted Answer

A) 66.8 bar-1 
B) 4.63 bar-1 
C) 2.53 × 10-2 bar-1 
D) 1.50 × 10-2 bar-1 
E) 1.03 bar-1 
A) 66.8 bar-1 
B) 4.63 bar-1 
C) 2.53 × 10-2 bar-1 
D) 1.50 × 10-2 bar-1 
E) 1.03 bar-1

Question 7

Express the equilibrium constant for the following reaction: 
CH3Cl(g)+ 1/2 Cl2(g)? CH2Cl2(g)+ 1/2 H2(g)

Accepted Answer

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

Question 8

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

Accepted Answer

A) 0.46 bar 
B) 0.037 bar 
C) 0.19 bar 
D) 0.14 bar 
E) 0.68 bar 
A) 0.46 bar 
B) 0.037 bar 
C) 0.19 bar 
D) 0.14 bar 
E) 0.68 bar

Question 9

Calculate the value of [N2]eq if [H2]eq = 2.0 mol L-1,[NH3]eq = 0.50 mol L-1,and Kc = 2.0. 
$\quad$$\quad$N2(g)+ 3H2(g)⇌ 2NH3(g)

Accepted Answer

A) 0.016 mol L-1 
B) 0.031 mol L-1 
C) 0.062 mol L-1 
D) 0.40 mol L-1 
E) 62.5 mol L-1 
A) 0.016 mol L-1 
B) 0.031 mol L-1 
C) 0.062 mol L-1 
D) 0.40 mol L-1 
E) 62.5 mol L-1

Question 10

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. 
$\quad$2SO2(g)+ O2(g)⇌ 2SO3$\quad$ (g)K = 1.7 × 106
$\quad$SO3(g)⇌ 1/2 O2(g)+ SO2$\quad$(g)K = ?

Accepted Answer

A) 3.4 × 102 
B) 8.5 
C) 1.3 × 103 
D) 1.2 × 10-6 
E) 7.7 × 10-4 
A) 3.4 × 102 
B) 8.5 
C) 1.3 × 103 
D) 1.2 × 10-6 
E) 7.7 × 10-4

Question 11

The equilibrium constant,Kp,equals 3.40 at 25 °C for the isomerization reaction: 
$\quad$$\quad$cis-2-butene ⇌ trans-2-butene
If a flask initially contains 5.00 bar of each gas,in what direction will the system shift to reach equilibrium?

Accepted Answer

A) It will shift left. 
B) It will shift right. 
C) The system is already at equilibrium. 
D) The system is not at equilibrium and will remain in an unequilibrated state. 
A) It will shift left. 
B) It will shift right. 
C) The system is already at equilibrium. 
D) The system is not at equilibrium and will remain in an unequilibrated state.

Question 12

For which of the following reactions will Kc = Kp?

Accepted Answer

A) 4NH3(g)+ 3O2(g)⇌ 2N2(g)+ 6H2O(g) 
B) SO3(g)+ NO(g)⇌ SO2(g)+ NO2(g) 
C) 2N2(g)+ O2(g)⇌ 2N2O(g) 
D) 2SO2(g)+ O2(g)⇌ 2SO3(g) 
E) PCl3(g) + 1/2 O2(g) ⇌ PCl3O(g) 
A) 4NH3(g)+ 3O2(g)⇌ 2N2(g)+ 6H2O(g) 
B) SO3(g)+ NO(g)⇌ SO2(g)+ NO2(g) 
C) 2N2(g)+ O2(g)⇌ 2N2O(g) 
D) 2SO2(g)+ O2(g)⇌ 2SO3(g) 
E) PCl3(g) + 1/2 O2(g) ⇌ PCl3O(g)

Question 13

For the following reaction,what is △n required in the conversion of Kc to Kp? 2Na(s)+ 2H2O(l)⇌ 2NaOH(aq)+ H2(g)

Accepted Answer

A) 3 
B) -1 
C) -2 
D) 2 
E) 1 
A) 3 
B) -1 
C) -2 
D) 2 
E) 1

Question 14

Express the equilibrium constant for the following reaction: 
H2(g)+ Br2(g)? 2HBr(g)

Accepted Answer

A) KP = $\frac {P(HBr) } { (\mathrm { P } ^ { 1 / 2 } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } ^ { 1 / 2 } \left( \mathrm { Br } _ { 2 } \right) }$ 
B) KP = $\frac { \mathrm { P } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { Br } _ { 2 } \right) } { \mathrm { P } ^ { 2 } ( \mathrm { HBr } ) }$ 
C) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } ^ { 2 } \left( \mathrm { Br } _ { 2 } \right) } { \mathrm { P } ^ { 4 } ( \mathrm { HBr } ) }$ 
D) KP= $\frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } ^{1 / 2} \left( \mathrm { Br } _ { 2 } \right) } { \mathrm { P } ( \mathrm { HBr } ) }$ 
E) KP = $\frac { \mathrm { P } ^ { 2 } ( \mathrm { HBr } ) } { \mathrm { P } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { Br } _ { 2 } \right) }$ 
A) KP = $\frac {P(HBr) } { (\mathrm { P } ^ { 1 / 2 } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } ^ { 1 / 2 } \left( \mathrm { Br } _ { 2 } \right) }$ 
B) KP = $\frac { \mathrm { P } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { Br } _ { 2 } \right) } { \mathrm { P } ^ { 2 } ( \mathrm { HBr } ) }$ 
C) KP = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } ^ { 2 } \left( \mathrm { Br } _ { 2 } \right) } { \mathrm { P } ^ { 4 } ( \mathrm { HBr } ) }$ 
D) KP= $\frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } ^{1 / 2} \left( \mathrm { Br } _ { 2 } \right) } { \mathrm { P } ( \mathrm { HBr } ) }$ 
E) KP = $\frac { \mathrm { P } ^ { 2 } ( \mathrm { HBr } ) } { \mathrm { P } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } \left( \mathrm { Br } _ { 2 } \right) }$

Question 15

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. 
$\quad$N2O4(g)⇌ 2NO2(g)$\quad$ K = 1.46
$\quad$3N2O4(g)⇌ 6NO2(g)$\quad$K = ?

Accepted Answer

A) 2.13 
B) 0.685 
C) 3.11 
D) 1.46 
E) 1.13 
A) 2.13 
B) 0.685 
C) 3.11 
D) 1.46 
E) 1.13

Question 16

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(CO)eq = 6.8 × 10-11 atm,P(O2)eq = 1.3 × 10-3 atm,P(CO2)eq = 0.041 atm. 
$\quad$$\quad$2 CO(g)+ O2(g)⇌ 2 CO2(g)

Accepted Answer

A) 3.6 × 10-21 atm-1 
B) 2.8 × 1020 atm-1 
C) 4.6 × 1011 atm-1 
D) 2.2 × 10-12 atm-1 
E) 3.6 × 10-15 atm-1 
A) 3.6 × 10-21 atm-1 
B) 2.8 × 1020 atm-1 
C) 4.6 × 1011 atm-1 
D) 2.2 × 10-12 atm-1 
E) 3.6 × 10-15 atm-1

Question 17

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

Accepted Answer

A) raising the temperature 
B) removing SO3 
C) adding O2 
D) increasing the pressure 
E) adding SO2 
A) raising the temperature 
B) removing SO3 
C) adding O2 
D) increasing the pressure 
E) adding SO2

Question 18

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

Accepted Answer

A) raising the temperature 
B) adding a solid 
C) adding argon 
D) none of the above 
A) raising the temperature 
B) adding a solid 
C) adding argon 
D) none of the above

Question 19

Consider the following reaction at equilibrium.What effect will adding CO2 have on the system? 
$\quad$$\quad$CO2(g)+ C(graphite)⇌ 2CO(g)

Accepted Answer

A) No effect will be observed since CO2 is not included in the equilibrium expression. 
B) The equilibrium constant will decrease. 
C) The reaction will shift in the direction of reactants. 
D) The equilibrium constant will increase. 
E) The reaction will shift in the direction of products. 
A) No effect will be observed since CO2 is not included in the equilibrium expression. 
B) The equilibrium constant will decrease. 
C) The reaction will shift in the direction of reactants. 
D) The equilibrium constant will increase. 
E) The reaction will shift in the direction of products.

Question 20

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

Accepted Answer

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

Exam 14: Chemical Equilibrium

For the following reaction,what is △n required in the conversion of Kc to Kp? P4(s)+ 5O2(g)⇌ P4O10(s)

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. \quad N2O4(g)⇌ 2NO2 \quad (g)K = 1.46 \quad 2N2O4(g)⇌ 4NO2 \quad (g)K = ?

In a reaction mixture containing only reactants,what is the value of Q?

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO2(g). \quad N2O4(g)⇌ 2NO2(g) \quad\quad Kc = 0.21 M \quad [N2O4]eq = 0.068 mol L-1

For the following reaction,what is Δn required in the conversion of Kc to Kp? \quad 2SO2(g)+ O2(g)⇌ 2SO3(g)

Express the equilibrium constant for the following reaction: CH3Cl(g)+ 1/2 Cl2(g)? CH2Cl2(g)+ 1/2 H2(g)

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

Calculate the value of [N2]eq if [H2]eq = 2.0 mol L-1,[NH3]eq = 0.50 mol L-1,and Kc = 2.0. \quad\quad N2(g)+ 3H2(g)⇌ 2NH3(g)

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. \quad 2SO2(g)+ O2(g)⇌ 2SO3 \quad (g)K = 1.7 × 106 \quad SO3(g)⇌ 1/2 O2(g)+ SO2 \quad (g)K = ?

The equilibrium constant,Kp,equals 3.40 at 25 °C for the isomerization reaction: \quad\quad cis-2-butene ⇌ trans-2-butene If a flask initially contains 5.00 bar of each gas,in what direction will the system shift to reach equilibrium?

For which of the following reactions will Kc = Kp?

For the following reaction,what is △n required in the conversion of Kc to Kp? 2Na(s)+ 2H2O(l)⇌ 2NaOH(aq)+ H2(g)

Express the equilibrium constant for the following reaction: H2(g)+ Br2(g)? 2HBr(g)

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. \quad N2O4(g)⇌ 2NO2(g) \quad K = 1.46 \quad 3N2O4(g)⇌ 6NO2(g) \quad K = ?

Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(CO)eq = 6.8 × 10-11 atm,P(O2)eq = 1.3 × 10-3 atm,P(CO2)eq = 0.041 atm. \quad\quad 2 CO(g)+ O2(g)⇌ 2 CO2(g)

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

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

Consider the following reaction at equilibrium.What effect will adding CO2 have on the system? \quad\quad CO2(g)+ C(graphite)⇌ 2CO(g)

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

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Filters

For the following reaction,what is △n required in the conversion of K_c to K_p? P₄(s)+ 5O₂(g)⇌ P₄O₁₀(s)

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. $\quad$ N₂O₄(g)⇌ 2NO₂ $\quad$ (g)K = 1.46 $\quad$ 2N₂O₄(g)⇌ 4NO₂ $\quad$ (g)K = ?

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO₂(g). $\quad$ N₂O₄(g)⇌ 2NO₂(g) $\quad$ $\quad$ K_c = 0.21 M $\quad$ [N₂O₄]_eq = 0.068 mol L^-1

For the following reaction,what is Δn required in the conversion of K_c to K_p? $\quad$ 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)

Express the equilibrium constant for the following reaction: CH₃Cl(g)+ 1/2 Cl₂(g)? CH₂Cl₂(g)+ 1/2 H₂(g)

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

Calculate the value of [N₂]_eq if [H₂]_eq = 2.0 mol L^-1,[NH₃]_eq= 0.50 mol L^-1,and K_c = 2.0. $\quad$ $\quad$ N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. $\quad$ 2SO₂(g)+ O₂(g)⇌ 2SO₃ $\quad$ (g)K = 1.7 × 10⁶ $\quad$ SO₃(g)⇌ 1/2 O₂(g)+ SO₂ $\quad$ (g)K = ?

The equilibrium constant,K_p,equals 3.40 at 25 °C for the isomerization reaction: $\quad$ $\quad$ cis-2-butene ⇌ trans-2-butene If a flask initially contains 5.00 bar of each gas,in what direction will the system shift to reach equilibrium?

For which of the following reactions will K_c = K_p?

For the following reaction,what is △n required in the conversion of K_c to K_p? 2Na(s)+ 2H₂O(l)⇌ 2NaOH(aq)+ H₂(g)

Express the equilibrium constant for the following reaction: H₂(g)+ Br₂(g)? 2HBr(g)

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. $\quad$ N₂O₄(g)⇌ 2NO₂(g) $\quad$ K = 1.46 $\quad$ 3N₂O₄(g)⇌ 6NO₂(g) $\quad$ K = ?

Determine the value of K_p for the following reaction if the equilibrium concentrations are as follows: P(CO)_eq = 6.8 × 10^-11 atm,P(O₂)_eq = 1.3 × 10^-3 atm,P(CO₂)_eq = 0.041 atm. $\quad$ $\quad$ 2 CO(g)+ O₂(g)⇌ 2 CO₂(g)

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

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

Consider the following reaction at equilibrium.What effect will adding CO₂ have on the system? $\quad$ $\quad$ CO₂(g)+ C(graphite)⇌ 2CO(g)

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