Question

One mole of an ideal gas at $500K$ is expended isothermally from an initial volume of $1\text{litre}$ to $10\text{litre}$. The $\Delta E$ for this process is :

• A. $163.7\text{cal}$
• B. $0\text{cal}$
• C. $1381.1\text{cal}$
• D. $9\text{L atm}$

Answer 1

The correct option is B $0\text{cal}$

For an isothermal process, $\Delta T=0$
Again, for an ideal gas, $\text{internal energy}\left(\Delta E\right)=nCv\Delta T$
Since $\Delta T=0$, hence $\Delta E=0$