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(A) For an ideal gas at constant pressure,the work done $W$ is given by the formula $W = P \Delta V$.According to the ideal gas equation,$PV = nRT$,so

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$2R$

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(A) For an ideal gas at constant pressure,the work done $W$ is given by the formula $W = P \Delta V$.According to the ideal gas equation,$PV = nRT$,so at constant pressure,$P \Delta V = nR \Delta T$.Given:$n = 1 \, mol$$\Delta T = 2 \, ^oC = 2 \, K$ (since the change in temperature is the same in Celsius and Kelvin scales).Substituting the values:$W = nR \Delta T = 1 \, mol 	imes R 	imes 2 \, K = 2R$.Since the gas expands when heated at constant pressure,the work is done by the system,which is conventionally represented as negative in some sign conventions,but in standard thermodynamic problems,the magnitude $2R$ is the expected answer. Given the options provided,the magnitude is $2R$.

The temperature of $1 \, mol$ of a gas is increased by $2 \, ^oC$ at constant pressure. The work done will be:

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