Question

To make a tea, a tourist puts into a kettle $2$ kg of ice at a temperature of $0^o$C. What quantity of heat is required to transform the ice into boiling water at ${100}^o$C temperature?

Answer 1

Given: To make a tea, a tourist puts into a kettle 2 kg of ice at a temperature of $0^{o}C$.

To find the quantity of heat is required to transform the ice into boiling water at ${100}^{o}C$ temperature

Solution:

We know,

Specific heat of water, $s=4.18J/\left(g^{\circ }C\right)$

Latent heat of fusion of ice, $L=334J/g$

As per the given condition,

Mass of ice, $m=2kg=2\times {10}^{3}g$

The total heat required will be sum of heat required toundergo a solid to liquid phase change at its melting point plus heat required to heat the sample from $0^{\circ }C$ to ${100}^{\circ }C$

$q_{total}=q_1+q_2⟹q_{total}=mL+ms\left(\Delta T\right)⟹q_{total}=2\times {10}^3\times 334+2\times {10}^3\times 4.18(100-0)⟹q_{total}=668\times {10}^3+836\times {10}^3⟹q_{total}=1504\times {10}^{3}J=1504kJ$

is the quantity of heat is required to transform the ice into boiling water at ${100}^{o}C$ temperature.