Calorimetry

Question

10 gm of ice at -20°C is dropped into a calorimeter containing 10 gm of water at 10°C. The specific heat of water is twice that of ice. Neglect heat capacity of the calorimeter. When equilibrium is reached, the calorimeter will contain :

Moderate

Solution

Heat that can be given by water, till it reaches 0°C,

${\mathrm{Q}}_{1}=10\times \mathrm{S}\times 10=100\mathrm{S}$

Heat that can be taken by ice to reach 0°C,

$\begin{array}{l}{\mathrm{Q}}_{2}=10\times \left(\frac{\mathrm{S}}{2}\right)\times 20=100\mathrm{S}\\ {\mathrm{Q}}_{1}={\mathrm{Q}}_{2}\end{array}$

$\therefore $No ice melts and no water freezes.

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