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Chemistry · THERMODYNAMICS
हिन्दीCalculate the work done when \( 56\text{ g} \) of nitrogen gas (assumed ideal) expands isothermally at \( 27^\circ\text{C} \) from a pressure of \( 5\text{ atm} \) to \( 1\text{ atm} \) in a reversible manner. (Molar mass of \( \text{N}_2 = 28\text{ g}\cdot\text{mol}^{-1} \), \( R = 8.314\text{ J}\cdot\text{K}^{-1}\cdot\text{mol}^{-1} \), \( \ln 5 = 1.609 \))
Correct answer · Option 1
\( -8027\text{ J} \)
Explanation
\( n = 56 / 28 = 2\text{ mol} \). \( w_{\text{rev}} = -nRT \ln(p_i/p_f) = -2 \times 8.314 \times 300 \times 1.609 = -8026.8\text{ J} \approx -8027\text{ J} \).
