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Assertion : The increase in internal energy $(\Delta E)$ for the vapourization of one mole of water at $1 \mathrm{~atm}$ and $373 \mathrm{~K}$ is zero.
Reason : For all isothermal processes, $\Delta E=0$.
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Reason : For all isothermal processes, $\Delta E=0$.
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The correct answer is:
If both assertion and reason are true and the reason is the correct explanation of the assertion
At $373 \mathrm{~K}$ or $100^{\circ} \mathrm{C}$, the water starts boiling and at this temperature the vaporization of water is an isothermal process.
The internal energy change $(\Delta E)$, depend only on temperature, it follows that at constant temperature, the internal energy of the gas remains constant, i.e. $\Delta E$ is zero.
The internal energy change $(\Delta E)$, depend only on temperature, it follows that at constant temperature, the internal energy of the gas remains constant, i.e. $\Delta E$ is zero.
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