Normal boiling point of water is 373 K (at 7 | vedclass

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(B) Applying the Clausius-Clapeyron equation: $\log \frac{P_2}{P_1} = \frac{\Delta H_{vap}}{2.303R} \left[ \frac{T_2 - T_1}{T_1 T_2} \right]$ Given: $

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$294$

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(B) Applying the Clausius-Clapeyron equation: $\log \frac{P_2}{P_1} = \frac{\Delta H_{vap}}{2.303R} \left[ \frac{T_2 - T_1}{T_1 T_2} ight]$ Given: $P_2 = 760 \ mm$,$T_2 = 373 \ K$,$P_1 = 23 \ mm$,$\Delta H_{vap} = 40656 \ J/mol$,$R = 8.314 \ J/K \cdot mol$. Substituting the values: $\log \frac{760}{23} = \frac{40656}{2.303 	imes 8.314} \left[ \frac{373 - T_1}{373 T_1} ight]$ $1.519 = 2123.5 	imes \left[ \frac{373 - T_1}{373 T_1} ight]$ $0.000715 = \frac{373 - T_1}{373 T_1}$ $0.2667 T_1 = 373 - T_1$ $1.2667 T_1 = 373$ $T_1 \approx 294.4 \ K$.

Normal boiling point of water is $373 \ K$ (at $760 \ mm$). Vapour pressure of water at $298 \ K$ is $23 \ mm$. If the enthalpy of evaporation is $40.656 \ kJ/mole$,the boiling point of water at $23 \ mm$ pressure will be ............. $K$.

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