Question:
Four $2 \mathrm{~cm} \times 2 \mathrm{~cm} \times 2 \mathrm{~cm}$ cubes are taken out from a refrigerator are put in $200 \mathrm{ml}$ of a drink at $10^{\circ} \mathrm{C}$.
(a) Find the temperature of the drink when the thermal equilibrium is attained in it.
(b) If the ice cubes do not melt completely, find the amount melted. Assume that no heat is lost to the outside of the drink and that the container has negligible heat capacity. Density of ice $=900 \mathrm{~kg} / \mathrm{m}^{3}$, density of the drink=1000kg $/ m^{3}$, specific heat capacity of the drink $=4200 \mathrm{~J} / \mathrm{kg}-\mathrm{K}$, latent heat of fusion of ice $=3.4 \times 10^{5} \mathrm{~J} / \mathrm{kg}$.
Solution:
$m \approx 25 \mathrm{gm}$