Assertion : The increase in internal energy ( | vedclass

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(D) The vaporization of water is a phase change process occurring at constant temperature $(373 \ K)$.For an ideal gas,internal energy $(E)$ is a func

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If both the Assertion and Reason are incorrect.

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(D) The vaporization of water is a phase change process occurring at constant temperature $(373 \ K)$.For an ideal gas,internal energy $(E)$ is a function of temperature only,so $\Delta E = 0$ for isothermal processes.However,for real substances like water undergoing a phase change,the internal energy changes because the intermolecular forces are overcome during vaporization.Therefore,the Assertion is incorrect because $\Delta E 
eq 0$ for the vaporization of water.The Reason is also incorrect because $\Delta E = 0$ only strictly applies to ideal gases in isothermal processes,and even then,it does not account for phase changes where potential energy changes.

Assertion : The increase in internal energy $(\Delta E)$ for the vaporization of one mole of water at $1 \ atm$ and $373 \ K$ is zero.
Reason : For all isothermal processes,$\Delta E = 0$.

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Assertion : The increase in internal energy $(\Delta E)$ for the vaporization of one mole of water at $1 \ atm$ and $373 \ K$ is zero.Reason : For all isothermal processes,$\Delta E = 0$.