Question

When 1 mole of ice melt at $0^{o}C$ and at a constant pressure of 1 atm, 1440 calories of heat are absorbed by the system. The molar volumes of ice and water are 0.0196 and 0.0180 litre respectively. Calculate $\Delta H$ and $\Delta E$ for the reaction

• A. $\Delta H\equiv \Delta E=1440calories$
• B. $\Delta H\equiv \Delta E=-1440calories$
• C. $\Delta H\equiv \Delta E=720calories$
• D. None of these

Answer 1

Answer: (A)

$\Delta H\equiv \Delta E=1440calories$

As we know,

$q=\Delta E-w$

Here is pressure is constant so

$\Delta H=q=1440cal$

and

$\Delta E=1440-P\Delta V=1440-1\times (0.018-0.0196)\equiv 1440cal$