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Chemistry · EQUILIBRIUM
हिन्दीA sample of \( 13.8\text{ g} \) of \( \text{N}_2\text{O}_4 \) (molar mass \( = 92\text{ g mol}^{-1} \)) is placed in a \( 1\text{ L} \) vessel at \( 400\text{ K} \) and decomposes according to \( \text{N}_2\text{O}_4(\text{g}) \rightleftharpoons 2\text{NO}_2(\text{g}) \). If the total pressure at equilibrium is \( 9.15\text{ bar} \), what is the partial pressure of \( \text{NO}_2 \) at equilibrium? (Take \( R = 0.083\text{ bar L mol}^{-1}\text{K}^{-1} \))
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Correct answer · Option A
\( 8.34\text{ bar} \)
Explanation
Initial pressure \( p_0 = \frac{nRT}{V} = \frac{0.15 \times 0.083 \times 400}{1} = 4.98\text{ bar} \). Total pressure \( = 4.98 + x = 9.15 \implies x = 4.17\text{ bar} \). Thus, \( p_{\text{NO}_2} = 2x = 2 \times 4.17 = 8.34\text{ bar} \).
