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Introduction

Determine K...

Question

Determine $K_{c}$ for $2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}, K_{p} = 3.4 b a r^{- 1}$ at $1000^{o} C$ :

159

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259

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359

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459

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Solution

The correct option is C $359$
Given reaction scheme

$2 S {O_{2}}_{(g)} + {O_{2}}_{(g)} ⇌ 2 S O_{3 (g)}$

∆n_g= n_products-n_reactants $= 2 - (2 + 1) = 2 - 3 = - 1$

Formula: $K_{p} = K_{c} (R T)^{Δ n}$

K_p is equilibrium constant from partial pressures = 3.4 bar^-1

K_c is the equilibrium constant from concentrations =?

R is gas constant = 0.08314 L bar^-1 K^-1 mol^-1

T is temperature = 1000^oC = 1000+273 = 1273K

On substituting we get

$K_{c} = \frac{3.4 b a r^{- 1}}{(0.08314 L b a r K^{- 1} m o l^{- 1} \times 1273 K)^{- 1}}$

$K_{c} = 3.4 \times 0.08314 \times 1273 L m o l^{- 1} = 359 L m o l^{- 1}$
Hence opt. C is correct.

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