Deck 14: Chemical Equilibrium

Question 1

Give the direction of the reaction if K >> 1.

A)The forward reaction is favoured.
B)The reverse reaction is favoured.
C)Neither direction is favoured.
D)If the temperature is raised,then the forward reaction is favoured.
E)If the temperature is raised,then the reverse reaction is favoured.

Answer 1

The forward reaction is favoured.

Question 2

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

A)7.8 × 10^-2
B)3.6
C)0.53
D)13
E)1.9

Answer 2

13

Question 3

Express the equilibrium constant for the following reaction:
PCl₅(g)? PCl₃(g)+ Cl₂(g)

A)K_P = $\frac { \mathrm { P } \left( \mathrm { PCl } _ { 5 } \right) } { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) }$
B)K_P = $\frac { \mathrm { P } ^ { 2 } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } ^ { 2 } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } ^ { 2 } \left( \mathrm { PCl } _ { 5 } \right) }$
C)K_P = $\frac { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } ^ { 2 } ( \mathrm { Cl } ) } { \mathrm { P } \left( \mathrm { PCl } _ { 5 } \right) }$
D)K_P = $\frac { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { PCl } _ { 5 } \right) }$
E)K_P = $\frac { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { PCl } _ { 5 } \right) } { \mathrm { P } ^ { 1 / 2 } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } ^ { 1 / 2 } \left( \mathrm { Cl } _ { 2 } \right) }$

Answer 3

K_P = $\frac { \mathrm { P } \left( \mathrm { PCl } _ { 3 } \right) \times \mathrm { P } \left( \mathrm { Cl } _ { 2 } \right) } { \mathrm { P } \left( \mathrm { PCl } _ { 5 } \right) }$

Question 4

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

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

Question 5

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

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

Question 6

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. H₂(g)+ Br₂(g)⇌ 2HBr(g)K = 3.8 × 10⁴
4HBr(g)⇌ 2H₂(g)+ 2Br₂(g)K = ?

A)1.9 × 10⁴
B)5.1 × 10^-3
C)2.6 × 10^-5
D)6.9 × 10^-10
E)1.6 × 10³

Question 7

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

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

Question 8

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

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

Question 9

Give the direction of the reaction if K << 1.

A)The forward reaction is favoured.
B)The reverse reaction is favoured.
C)Neither direction is favoured.
D)If the temperature is raised,then the forward reaction is favoured.
E)If the temperature is raised,then the reverse reaction is favoured.

Question 10

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

A)K_P = $\frac {P(HBr) } { (\mathrm { P } ^ { 1 / 2 } \left( \mathrm { H } _ { 2 } \right) \times \mathrm { P } ^ { 1 / 2 } \left( \mathrm { Br } _ { 2 } \right) }$


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

Question 11

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

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 12

Which of the following statements is correct?

A)When K >> 1,the reverse reaction is favoured and essentially goes to completion.
B)When K << 1,the forward reaction is favoured and the reverse reaction does not proceed to a great extent.
C)When K ≈ 1,neither the forward nor reverse reaction is strongly favoured,and about the same amount of reactants and products exist at equilibrium.
D)K >> 1 implies that the reaction is very fast at producing products.
E)When K = 0 the reaction is in equilibrium.

Question 13

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

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

Question 14

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

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 15

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

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

Question 16

The equilibrium constant is given for one of two reactions below.Determine the value of the missing equilibrium constant. H₂(g)+ Br₂(g)⇌ 2HBr(g)K = 3.8 × 10⁴
2HBr(g)⇌ H₂(g)+ Br₂(g)K = ?

A)1.9 × 10⁴
B)5.3 × 10^-5
C)2.6 × 10^-5
D)6.4 × 10^-4
E)1.6 × 10³

Question 17

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

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

Question 18

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

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

Question 19

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

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

Question 20

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

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

Question 21

The reaction below has a K_p value of 3.3 × 10^-5 bar.What is the value of K_c for this reaction at 700 K? 2SO₃(g)⇌ 2SO₂(g)+ O₂(g)

A)5.7 × 10^-7 M
B)1.7 × 10⁶ M
C)3.3 × 10^-5 M
D)3.0 × 10⁴ M
E)1.9 × 10^-3 M

Question 22

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

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

Question 23

Express the equilibrium constant for the following reaction:
$\quad$$\quad$$\quad$ SO_2(g) + H₂O(l)? H₂SO₃(aq)

A)K = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { SO } _ { 3 } \right] \times \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \mathrm { P } \left( \mathrm { SO } _ { 2 } \right) }$
B)K = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { SO } _ { 3 } \right] } { \mathrm { P } \left( \mathrm { SO } _ { 2 } \right) }$
C)K = $\frac { \mathrm { P } _ { \left[ \mathrm { SO } _ { 2 } \right) } } { \left. \mathrm { H } _ { 2 } \mathrm { SO } _ { 3 } \right] }$
D)K = $\frac { \left[ \mathrm { H } _ { 2 } \mathrm { SO } _ { 3 } \right] } { \mathrm { P } \left( \mathrm { SO } _ { 2 } \right) \times \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] }$
E)K = $\frac { \mathrm { P } \left( \mathrm { SO } _ { 2 } \right) \times \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \left[ \mathrm { H } _ { 2 } \mathrm { SO } _ { 3 } \right] }$

Question 24

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [N₂]_eq = 3.6 mol L^-1,[O₂]_eq = 4.1 mol L^-1,[N₂O]_eq = 3.3 × 10^-18 mol L^-1. 2N₂(g)+ O₂(g)⇌ 2N₂O(g)

A)2.2 × 10^-19
B)4.5 × 10¹⁸
C)2.0 × 10^-37
D)5.0 × 10³⁶
E)4.9 × 10^-17

Question 25

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)

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

Question 26

For which reaction will K_p = K_c?

A)S(s)+ O₂(g)⇌ SO₂(g)
B)2HgO(s)⇌ Hg(l)+ O₂(g)
C)CaCO₃(s)⇌ CaO(s)+ CO₂(g)
D)H₂CO₃(s)⇌ H₂O(l)+ CO₂(g)
E)2H₂O(l)⇌ 2H₂(g)+ O₂(g)

Question 27

The reaction below has a K_p value of 41 bar^-2.What is the value of K_c for this reaction at 400 K? N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

A)2.4 × 10^-2 M^-2
B)4.4 × 10⁴ M^-2
C)41 M^-2
D)2.3 × 10^-5 M^-2
E)1.9 × 10⁴ M^-2

Question 28

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

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

Question 29

Express the equilibrium constant for the following reaction:
$\quad$$\quad$ P₄(s)+ 5O₂(g)? P₄O₁₀(s)

A)K_c = $\frac { \left[ \mathrm { P } _ { 4 } \right] \left[ \mathrm { O } _ { 2 } \right] ^ { 5 } } { \left[ \mathrm { P } _ { 4 } \mathrm { O } _ { 10 } \right] }$
B)K_c = $\frac { \left[ \mathrm { P } _ { 4 } \mathrm { O } _ { 10 } \right] } { \left[ \mathrm { P } _ { 4 } \right] \left[ \mathrm { O } _ { 2 } \right] ^ { 5 } }$
C)K_c = [O₂]^-5
D)K_c = [O₂]⁵
E)K_c = $\frac { \left[ \mathrm { P } _ { 4 } \mathrm { O } _ { 10 } \right] } { \left[ \mathrm { P } _ { 4 } \right] \left[ \mathrm { O } _ { 2 } \right] ^ { 1 / 5 } }$

Question 30

Express the equilibrium constant for the following reaction:
KClO₃(s)? KClO(s)+ O₂(g)

A)K_c = $\frac { [ \mathrm { KClO } ] \left[ \mathrm { O } _ { 2 } \right] } { \left[ \mathrm { KClO } _ { 3 } \right] }$
B)K_c = [O₂]^-1
C)K_c = $\frac { [ \mathrm { KClO } ] ^ { 2 } \left[ \mathrm { O } _ { 2 } \right] ^ { 2 } } { \left[ \mathrm { KClO } _ { 3 } \right] ^ { 2 } }$
D)K_c = $\left[ \mathrm { KClO } _ { 3 } \right]$
$[ \mathrm { KClO } ] \left[ \mathrm { O } _ { 2 } \right]$

$\frac {[{ KClO } _ { 3 }] } { \mathrm [{ KClO } ] \left[ \mathrm { O } _ { 2 } \right] }$








E)K_c = [O₂]

Question 31

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

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

Question 32

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

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

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



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

Question 33

For the following reaction,what is △n required in the conversion of K_c to K_p? KClO₃(s)⇌ KClO(s)+ O₂(g)

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

Question 34

The reaction below has a K_c value of 61 M^-2.What is the value of K_p for this reaction at 500 K? N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

A)15 bar^-2
B)61 bar^-2
C)28 bar^-2
D)3.6 × 10^-2 bar^-2
E)1.9 × 10^-2 bar^-2

Question 35

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

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

Question 36

For the following reaction,what is Δn required in the conversion of K_c to K_p? CH₄(g)+ H₂O(g)⇌ CO(g)+ 3H₂(g)

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

Question 37

For the following reaction,what is Δn required in the conversion of K_c to K_p? N₂O₄(g)⇌ 2NO₂(g)

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

Question 38

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

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 39

For which of the following reactions will K_c = K_p?

A)H₂(g)+ I₂(g)⇌ 2HI(g)
B)CH₄(g)+ H₂O(g)⇌ CO(g)+ 3H₂(g)
C)N₂O₄(g)⇌ 2NO₂(g)
D)CO(g)+ 2H₂(g)⇌ CH₃OH(g)
E)N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

Question 40

For which of the following reactions will K_c = K_p?

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)PCl_3(g) + 1/2 O_2(g) ⇌ PCl₃O_(g)

Question 41

In a reaction mixture containing reactants and products,each at a concentration of 1 mol L^-1,what is the value of Q?

A)-1
B)1
C)∞
D)0
E)Q = K

Question 42

Which of the following statements is TRUE?

A)If Q < K,it means the reverse reaction will proceed to form more reactants.
B)If Q > K,it means the forward reaction will proceed to form more products.
C)If Q = K,it means the reaction is at equilibrium.
D)If Q << K,it means the reaction is shifted to the left.
E)If Q >> K,it means the reaction is shifted to the right.

Question 43

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

A)-1
B)1
C)∞
D)0
E)Q = K

Question 44

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [PCl₅]_eq = 0.56 mol L^-1,[PCl₃]_eq = 0.23 mol L^-1,[Cl₂]_eq = 4.4 mol L^-1. PCl₅(g)⇌ PCl₃(g)+ Cl₂(g)

A)1.8 M
B)0.93 M
C)0.55 M
D)1.1 M
E)0.76 M

Question 45

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. 2NOCl(g)⇌ 2NO(g)+ Cl₂(g)

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 46

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO₃(g). 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)K_c = 1.7 × 10⁸ M^-1
[SO₂]_eq = 0.0034 mol L^-1 [O₂]_eq = 0.0018 mol L^-1

A)1.9 mol L^-1
B)1.0 × 10³ mol L^-1
C)0.53 mol L^-1
D)9.6 × 10^-4 mol L^-1
E)0.73 mol L^-1

Question 47

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. N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

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 48

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

A)-1
B)1
C)∞
D)0
E)Q = K

Question 49

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of H₂O(g). C₂H₄(g)+ H₂O(g)⇌ C₂H₅OH(g)K_c = 9.0 × 10³ M^-1
[C₂H₄]_eq = 0.015 mol L^-1 [C₂H₅OH]_eq = 1.69 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 50

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 . 2NOCl(g)⇌ 2NO(g)+ Cl₂(g)

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

Question 51

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. 2 CO(g)+ O₂(g)⇌ 2 CO₂(g)

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 52

Consider the following reaction and its equilibrium constant: I₂(g)+ Br₂(g)⇌ 2IBr(g)K_c = 1.1 × 10²
A reaction mixture contains 0.41 mol L^-1 I₂,0.27 mol L^-1 Br₂ and 3.5 mol L^-1 IBr.Which of the following statements is TRUE concerning this system?

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

Question 53

Which of the following statements is TRUE?

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 54

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. N₂(g)+ 3H₂(g)⇌ 2NH₃(g)

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 55

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 CO₂ and 1.3 mol L^-1 H₂O.Which of the following statements is TRUE concerning this system?

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 56

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. H₂(g)+ I₂(g)⇌ 2HI(g)

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

Question 57

Which of the following statements is TRUE?

A)If Q < K,it means the reverse reaction will proceed to form more reactants.
B)If Q > K,it means the reverse reaction will proceed to form more reactants.
C)If Q = K,it means the reaction is not at equilibrium.
D)Because the equilibrium is always dynamic,Q can never be equal to K.
E)If Q < K,the reaction proceeding to the left is much faster than the reaction proceeding to the right.

Question 58

Consider the following reaction and its equilibrium constant: SO₂(g)+ NO₂(g)⇌ SO₃(g)+ NO(g)K_c = 0.33
A reaction mixture contains 0.39 mol L^-1 SO₂,0.14 mol L^-1 NO₂ ,0.11 mol L^-1 SO₃ and 0.14 mol L^-1 NO.Which of the following statements is TRUE concerning this system?

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

Question 59

Consider the following reaction and its equilibrium constant: I₂(g)⇌ 2I(g)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?

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 60

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. 2HCl(g)+ I₂(s)⇌ 2HI(g)+ Cl₂(g)

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 61

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.

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

Question 62

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO₂(g). N₂O₄(g)⇌ 2NO₂(g)K_c = 0.21 M
[N₂O₄]_eq = 0.039 mol L^-1

A)1.22 mol L^-1
B)9.0 × 10^-2 mol L^-1
C)7.8 × 10^-2 mol L^-1
D)8.2 × 10^-3 mol L^-1
E)11 mol L^-1

Question 63

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.

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 64

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO₂(g). N₂O₄(g)⇌ 2NO₂(g)K_c = 0.21 M
[N₂O₄]_eq = 1.82 mol L^-1

A)0.38 mol L^-1
B)0.71 mol L^-1
C)0.62 mol L^-1
D)0.40 mol L^-1
E)0.095 mol L^-1

Question 65

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

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

Question 66

Consider the following reaction: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g)
A reaction mixture initially contains 0.86 bar NO and 0.86 bar SO₃.Determine the equilibrium pressure of NO₂ if K_p for the reaction at this temperature is 0.0118.

A)0.78 bar
B)0.084 bar
C)0.012 bar
D)0.85 bar
E)0.048 bar

Question 67

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.

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

Question 68

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.

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

Question 69

Consider the following reaction: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g)
A reaction mixture initially contains 1.24 bar NO and 0.92 bar SO₃.Determine the equilibrium pressure of NO₂ if K_p for the reaction at this temperature is 0.0118.

A)0.32 bar
B)1.32 bar
C)0.10 bar
D)0.74 bar
E)0.022 bar

Question 70

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of CO₂(g). NH₂COONH₄(s)⇌ 2NH₃(g)+ CO₂(g)K_c = 1.58 × 10^-8 M³
[NH₃]_eq = 2.9 × 10^-3 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 71

Consider the following reaction: CH₄(g)+ 2H₂S(g)⇌ CS₂(g)+ 4H₂(g)
A reaction mixture initially contains 0.50 mol L^-1 CH₄ and 0.75 mol L^-1 H₂S.If the equilibrium concentration of H₂ is 0.44 mol L^-1,find the equilibrium constant (mol L^-1)for the reaction.

A)0.23 mol² L^-2
B)0.038 mol² L^-2
C)2.9 mol² L^-2
D)10.mol² L^-2
E)0.34 mol² L^-2

Question 72

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO₂(g). N₂O₄(g)⇌ 2NO₂(g)K_c = 0.21 M
[N₂O₄]_eq = 0.068 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 73

Consider the following reaction: CuS(s)+ O₂(g)⇌ Cu(s)+ SO₂(g)
A reaction mixture initially contains 2.9 mol L^-1 O₂.Determine the equilibrium concentration of O₂ if K_c for the reaction at this temperature is 1.5.

A)1.9 mol L^-1
B)1.7 mol L^-1
C)2.2 mol L^-1
D)1.2 mol L^-1
E)0.59 mol L^-1

Question 74

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of NO₂(g). N₂O₄(g)⇌ 2NO₂(g)K_c = 0.21 M
[N₂O₄]_eq = 1.34 mol L^-1

A)0.25 mol L^-1
B)0.043 mol L^-1
C)0.60 mol L^-1
D)0.028 mol L^-1
E)0.53 mol L^-1

Question 75

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 K_c 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.

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 76

Consider the following reaction,equilibrium pressures,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of CO. CO(g)+ 2H₂(g)⇌ CH₃OH(l)K_p = 2.25 × 10⁴ bar^-3
P(H₂)_eq = 0.52 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 77

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^-6 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 78

Consider the following reaction: NO(g)+ SO₃(g)⇌ NO₂(g)+ SO₂(g)
A reaction mixture initially contains 0.384 bar NO₂ and 0.224 bar SO₂.Determine the equilibrium pressure of SO₂ if K_p for the reaction at this temperature is 0.0118.

A)0.220 bar
B)0.037 bar
C)0.67 bar
D)0.024 bar
E)0.0035 bar

Question 79

Consider the following reaction,equilibrium concentrations,and equilibrium constant at a particular temperature.Determine the equilibrium concentration of SO₂(g). 2SO₂(g)+ O₂(g)⇌ 2SO₃(g)K_c = 1.7 × 10⁸ M^-1
[SO₃]_eq = 0.0034 mol L^-1 [O₂]_eq = 0.0018 mol L^-1

A)2.8 × 10¹³ mol L^-1
B)1.88 mol L^-1
C)6.1 × 10^-6 mol L^-1
D)1.0 × 10³ mol L^-1
E)1.4 mol L^-1

Question 80

Consider the following reaction,equilibrium pressures,and equilibrium constant at a particular temperature.Determine the equilibrium pressure of H₂. D₂(g)+ H₂(g)⇌ 2HD(g)K_p = 1.80
P(D₂)_eq = 1.1 × 10^-3 bar P(HD)_eq = 2.7 × 10^-3 bar

A)2.7 bar
B)1.4 bar
C)0.73 bar
D)3.7 × 10^-3 bar
E)8.1 × 10^-4 bar