The value of $\mathrm{K}_{\mathrm{p}} / \mathrm{K}_{\mathrm{C}}$ for the following reactions at $300 \mathrm{~K}$ are, respectively :
(At $300 \mathrm{~K}, \mathrm{RT}=24.62 \mathrm{dm}^{3} \mathrm{~atm} \mathrm{} \mathrm{mol}^{-1}$ )
$\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})$
$\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$
$\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})$
Correct Option: , 4
$\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})$
$\frac{\mathrm{k}_{\mathrm{p}}}{\mathrm{k}_{\mathrm{c}}}=(\mathrm{RT})^{\Delta \mathrm{n}_{\mathrm{g}}}=(\mathrm{RT})^{0}=1$
$\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$
$\frac{\mathrm{k}_{\mathrm{p}}}{\mathrm{k}_{\mathrm{c}}}=(\mathrm{RT})^{1}=24.62$
$\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})$
$\frac{\mathrm{k}_{\mathrm{p}}}{\mathrm{k}_{\mathrm{c}}}=(\mathrm{RT})^{-2}=\frac{1}{(\mathrm{RT})^{2}}=1.65 \times 10^{-3}$
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