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Calorimetry

Water gas, a ...

Question

Water gas, a mixture of $H_{2}$ and $C O$ , is an important industrial fuel produced by the reaction of steam with red-hot coke,essentially pure carbon. Write the expression for the equilibrium constant for the reversible reaction.
$C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g) Δ H = 131.30 k J$

K = [C O] [H_{2}] / [H_{2} O]

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K = [H_{2} O] / [C O] [H_{2}]

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K = [C O] [H_{2}] / [H_{2} O] [C]

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None of these

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Solution

The correct option is A $K = [C O] [H_{2}] / [H_{2} O]$
$C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g) Δ H = 131.30 k J$
$K = [C O] [H_{2}] / [H_{2} O]$

Suggest Corrections

Similar questions

H_{2}

C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g)

Δ H = 131.30

H_{2}

C (s) + H_{2} O ⇌ C O (g) + H_{2} O, Δ H = + 131 k J

H_{2}

K_{p}

C (s) + H_{2} O_{(g)} ⇌ C O_{(g)} + H_{2 (g)}

[H_{2} O] = 1.10 M, [C O] = [H_{2}] = 0.2 M, R = 0.08206 L a t m k^{- 1} m o l^{- 1}

K_{c} = 4.24

800

C O (g) + H_{2} O ⇌ C O_{2} (g) + H_{2} (g)

C O_{2}, H_{2}, C O

H_{2} O

800

C O

H_{2} O

0.10

H_{2}

C O

C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g), Δ H = + 131 k J

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