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Standard XII

Chemistry

Molality

Calculate the...

Question

Calculate the equilibrium constant $K_{p}$ for the reaction $C_{(s)} + C O_{2 (G)} ⇌ 2 c o_{(g)}$ at 1300K from the following data $C_{(s)} + 2 H_{2} O_{(g)} ⇌ C O_{2 (g)} + 2 H_{2 (g)} K_{p} (1300 K) = 3.9 a t m$
$H_{2 (g)} + C O_{2 (g)} ⇌ C O_{(g)} + H_{2} O_{(g)} K_{p} (1300 K) = 0.7 a t m$

0.49 atm

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1.911 atm

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0.7 atm

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2.73 atm

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Solution

The correct option is B 1.911 atm
$K_{p} = \frac{[C O]^{2} [H_{2} O]^{2}}{[H_{2}]^{2} [C O_{2}]^{2}} \times \frac{[H_{2}]^{2} [C O_{2}]}{[H_{2} O]^{2}} = \frac{[C O]^{2}}{[C O]^{2}} = (0.7) 2 \times 3.9 = 1.911 a t m$

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Similar questions

Calculate the equilibrium constant ( $K_{p}$ ) for the reaction, $C (s) + C O_{2} (g) ⇌ 2 C O (g)$ , at $1300 K$ from the following data:
$C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g); K_{p} (1300 K) = 3.9 a t m$

$H_{2} (g) + C O_{2} (g) ⇌ C O (g) + H_{2} O (g); K_{p} (1300 K) = 0.623 a t m$

Q. The following equilibrium constants were determined at

1120 K

2 C O (g) ⇌ C (s) + {C O}_{2} (g); K_{p_{1}} = 10^{- 14} {a t m}^{- 1}

C O (g) + C l_{2} (g) ⇌ C O {C l}_{2} (g); K_{p_{2}} = {6 \times 10}^{- 3} {a t m}^{- 1}

What is the equilibrium constant

K_{c}

for the following reaction at

1120 K

C (s) + {C O}_{2} (g) + 2 C l_{2} (g) ⇌ 2 C O {C l}_{2} (g)

Q. The following equilibrium constants were determined at 1120 K:

2 C O (g) ⇌ C (s) + C O_{2} (g) K p_{1} = 10^{- 14} a t m^{- 1}

C O (g) + C l_{2} (g) ⇌ C O C l_{2} K p_{2} = 6 \times 10^{- 3} a t m^{- 1}

What is the equilibrium constant

K_{p}

for the following reaction at 1120 K.

C (s) + C O_{2} (g) + 2 C l_{2} (g) ⇌ 2 C O C l_{2} (g)

Q. The following equilibrium constants were determined at

1120 K

2 C O (g) ⇌ C (s) + C O_{2} (g); K_{P_{1}} = 10^{- 14} a t m^{- 1} C O (g) + C l_{2} (g) ⇌ C O C l_{2} (g); K_{p_{2}} = 6 \times 10^{- 3} a t m^{- 1}

What is the equilibrium constant

K_{C}

for the following reaction at

1120 K

;

C (s) + C O_{2} (g) + 2 C l_{2} (g) ⇌ 2 C O C l_{2} (g)

Q. Considerthe following reactions,
I.

C (s) + \frac{1}{2} O_{2} (g) \to C O (g); Δ H_{1} = a

II.

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g); Δ H_{2} = b

III.

C (s) + C O_{2} (g) \to 2 C O (g); Δ H_{3} = c

Select the correct statement

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Calculate the equilibrium constant Kp for the reaction C(s)+CO2(G)⇌2co(g) at 1300K from the following data C(s)+2H2O(g)⇌CO2(g)+2H2(g)Kp(1300K)=3.9atm H2(g)+CO2(g)⇌CO(g)+H2O(g)Kp(1300K)=0.7atm

The correct option is B 1.911 atmKp=[CO]2[H2O]2[H2]2[CO2]2×[H2]2[CO2][H2O]2=[CO]2[CO]2=(0.7)2×3.9=1.911atm

The correct option is B 1.911 atm
$K_{p} = \frac{[C O]^{2} [H_{2} O]^{2}}{[H_{2}]^{2} [C O_{2}]^{2}} \times \frac{[H_{2}]^{2} [C O_{2}]}{[H_{2} O]^{2}} = \frac{[C O]^{2}}{[C O]^{2}} = (0.7) 2 \times 3.9 = 1.911 a t m$