Question

A copper block of mass $2kg$ is heated to temperature of ${500}^{\circ }C$ and then placed in a large block of ice at $0^{\circ }C$. What is the maximum amount of ice that can melt? The specific heat of copper is 400 J ${kg}^{-1}$ ${}^{\circ }{C}^{-1}$ and latent heat of fusion of water is $3.5\times {10}^{5}J$ ${kg}^{-1}$ .

Answer 1

Given : $S=400Jk{g}^{-1}{C}^{-1}$ and $L_f=3.5\times {10}^{5}Jk{g}^{-1}$

Mass of copper block $m=2kg$

Heat released by the copper block is equal to the heat gained by the ice to melt.

Let the mass of the ice melted be $M$.

Change in temperature of copper block $\Delta T=500-0={500}^{o}C$

$\therefore$ $mS\left(\Delta T\right)=M{L}_f$

Or $2\times 400\times 500=M\times 3.5\times {10}^5$

$⟹$ $M=1.14kg$