$\mathrm{K}_{\mathrm{c}}$ for the reaction $\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g})…

$\mathrm{K}_{\mathrm{c}}$ for the reaction $\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) ightleftharpoons 2 \mathrm{NO}(\mathrm{g})$
at $300 \mathrm{~K}$ is $4.0 \times 10^{-6} . \mathrm{K}_{\mathrm{p}}$ for the above reaction will be $\left(\mathrm{R}=2 \mathrm{cal} \mathrm{mol}^{-1} \mathrm{~K}^{-1}ight)$
  1. $2.4 \times 10^{-3}$
  2. $4 \times 10^{-6}$
  3. $4 \times 10^{-6}(\mathrm{RT})^{2}$
  4. $16 \times 10^{-12}$

Solution

$\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{\Delta \mathrm{n}}$ since $\Delta \mathrm{n}=0, \mathrm{~K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}$.

Asked in: JEE-TOPICTESTS-CHEMISTRY

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