Question

How much energy must be supplied to change $36g$ of ice at $0^{o}C$ to water at room temperature ${25}^{o}C$?
Data for water:
$\Delta H_{fusion}=6.01kJ/mol$
$C_{Pliquid}=4.18J{K}^{-1}{g}^{-1}$

• A. $12kJ$
• B. $16kJ$
• C. $19kJ$
• D. $22kJ$

Answer 1

Answer: (B)

$16kJ$

Energy to supplied $=n\Delta H_{fusion}+m{C}_P\times \Delta T$

$n=\frac{36g}{18g}=2moles$

$m=36g$

$\therefore$ Energy to be supplied $=(2\times 6.01\times {10}^3)+(36\times 4.18\times 25)$

$=15782J$

$=16KJ$