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For the reaction: \mathrm{Fe_{2}N(s)+\frac{3}{2}H_{2}(g)\rightleftharpoons 2Fe(s)+NH_{3}(g)}
Option: 1 K_{c}=K_{p}(RT)^{-\frac{1}{2}}
Option: 2 K_{c}=K_{p}(RT)^{\frac{1}{2}}
Option: 3 K_{c}=K_{p}(RT)  
Option: 4 K_{c}=K_{p}(RT)^{\frac{3}{2}}

Answers (1)

best_answer

The reaction occurs as follows:

\mathrm{Fe_{2}N(s)\: +\: \frac{3}{2}H_{2}(g)\: \rightleftharpoons \: 2Fe(s)\: +\: NH_{3}(g)}

\mathrm{\Delta n\: =\: -\frac{1}{2}}

We know that:

\\\mathrm{k_{p}\: =\: k_{c}(RT)^{\Delta n}}\\\\\mathrm{Thus,\: k_{p}\: =\: k_{c}(RT)^{-\frac{1}{2}}}\\\\\mathrm{k_{c}\: =\: k_{p}(RT)^{\frac{1}{2}}}

Therefore, Option(2) is correct.

Posted by

Kuldeep Maurya

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