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Q.

The value of Kp for the reaction $\large 2{H_2}{S_{(g)}}\, \Leftrightarrow \,2{H_{2\left( g \right)}} + \,{S_{2\left( g \right)}}$ is 1.2 × 10^-2 at 1065⁰C. The value of Kc for this reaction is

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a

1.2\, \times \,{10^{ - 2}}

b

< \,1.2\, \times \,{10^{ - 2}}

c

$81$

d

> \,1.2\, \times \,{10^{ - 2}}

answer is B.

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Detailed Solution

\large 2{H_2}{S_{(g)}}\, \rightleftharpoons \,2{H_{2\left( g \right)}} + \,{S_2{\left( g \right)}}

\large {K_P} = 1.2 \times {10^{ - 2}}

\large T = \left( {1065 + 273} \right)K

\large {\Delta _{ng}} = 3 - 2 = 1

\large {K_P} = {K_C}{\left( {RT} \right)^{\Delta n}}

\large 1.2 \times {10^{ - 2}} = {K_C}{\left( {1338} \right)^1}

\large {K_C} = \frac{{1.2 \times {{10}^{ - 2}}}}{{1338}}

\large {K_C} = 8.96 \times {10^{ - 6}}

K_C < K_P

K_C < 1.2 $\times$ 10^-2

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