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JEE Main levelSingle correct optionDifficulty 2 of 3td070

One mole of an ideal gas at $300 K$ is compressed reversibly and isothermally from $1.00 bar$ to $10.0 bar$ . Using $R = 8.314 J mo l^{- 1} K^{- 1}$ and $ln 10 = 2.303$ , the work done on the gas is

A $- 5.74 kJ$
B $+ 2.49 kJ$
C $+ 5.74 kJ$
D $+ 0.57 kJ$

Answer: C

For reversible isothermal compression

w_{o n} = n RT ln (P_{2} / P_{1}) = 8.314 \times 300 \times 2.303 J = 5.74 kJ

. It is positive because work is done on the gas.

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