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(C) For an isobaric process (constant pressure), the work done $W$ is given by the formula $W = P \Delta V$. Using the ideal gas equation $PV = nRT$,

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$8.3 	imes 10^{2} \, J$

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(C) For an isobaric process (constant pressure), the work done $W$ is given by the formula $W = P \Delta V$. Using the ideal gas equation $PV = nRT$, for a constant pressure process, $P \Delta V = nR \Delta T$. Given: Number of moles $n = 1 \, 	ext{mol}$. Change in temperature $\Delta T = 100^{\circ}C - 0^{\circ}C = 100 \, K$. Gas constant $R = 8.3 \, J/mol \cdot K$. Substituting these values into the formula: $W = nR \Delta T = 1 	imes 8.3 	imes 100$. $W = 830 \, J = 8.3 	imes 10^{2} \, J$.

When the temperature of $1 \, \text{mole}$ of an ideal gas is increased from $0^{\circ}C$ to $100^{\circ}C$ at constant pressure, what is the work done during the process? $(R = 8.3 \, J/mol \cdot K)$

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