Assertion(A): The increase in internal energy ( $Δ E$ ) for the vaporisation of one mole of water at 1atm and 373K is zero.
Reason(R): For all isothermal process, $Δ E = 0$

Both A and R are true and R is the correct explanation of A.

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Both A and R are true but R is not the correct explanation of A.

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A is true but R is false.

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Both A and R are false.

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Solution

The correct option is A Both A and R are true and R is the correct explanation of A.
Change in internal energy $= Δ E = n R Δ T$
Since for vapourisation of water $Δ T = O$ (isothermal process).
$∴ Δ E = O$

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Similar questions

Assertion (A): Solvay process is used for the preparation of $N a H C O_{3}$ but not for $K H C O_{3}$

Reason (R): Solubility of $K H C O_{3}$ is more than $N a H C O_{3}$ in water

\to

80^{\circ} C

[H^{+}] a n d [O H^{-}]

\to K_{w}

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