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For the reversible reaction $\large {N_{2(g)}}\, + \,3{H_{2\left( g \right)}}\, \rightleftharpoons \,2N{H_{3\left( g \right)}}$ at 500⁰C. The value of K_p is 1.44×10^-5, when partial pressure is measured in atmospheres. The corresponding value of K_c with concentration in mol L^-1 is

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\frac{{1.44\, \times \,{{10}^{ - 5}}}}{{{{\left( {0.082 \times 500} \right)}^{ - 2}}}}

\frac{{1.44\, \times \,{{10}^{ - 5}}}}{{{{\left( {8.314 \times 773} \right)}^{ - 2}}}}

\frac{{1.44\, \times \,{{10}^{ - 5}}}}{{{{\left( {0.082 \times 773} \right)}^{ - 2}}}}

answer is D.

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Detailed Solution

K_p = K_c ${[RT]}^{∆ n_{g}}$

K_c= $\frac{K_{p}}{{[RT]}^{∆ n_{g}}}$

$\frac{1.44 \times 10^{- 5}}{{(0.082 \times 773)}^{- 2}}$

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