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When a mixture of \( \mathrm{N}_{2} \) and \( \mathrm{H}_{2} \) in the volume ratio of \( 1: 5 \) is allowed to react at \( 700 \mathrm{~K} \) and \( 10^{3} \mathrm{~atm} \) pressure, \( 0.4 \) mole fraction of \( \mathrm{NH}_{3} \) is formed at equilibrium. The value of \( K_{\mathrm{P}} \) for the below reaction
\[
\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})
\]
(a) \( 2.6 \times 10^{-5} \mathrm{~atm}^{-2} \)
(b) \( 2.6 \times 10^{-4} \mathrm{~atm}^{-2} \)
(c) \( 2.6 \times 10^{3} \) atm \( ^{-2} \)
(d) \( 5.1 \times 10^{-3} \mathrm{~atm}^{-2} \)
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