Question

How much energy must be supplied to change 36 g of ice at $0^\circ C$ to water at room temperature $25^\circ C$ ?

Data for water
$\Delta H_{f u s i o n}^{o}$	$\text{6} \text{.01} \, \text{kJ/mol}$
$\left(\text{C}\right)_{\text{p} \, \text{(liquid)}}$	$\text{4} \text{.18} \, \text{JK}^{- \text{1}} \text{g}^{- \text{1}}$

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

Answer 1

Answer: (B)

$\Delta H=\left(\right.\Delta H_{f u s i o n}\left.\right)$ of two moles $+ms\Delta t$
$=6.01\times 2+36\times 4.18\times 25\times 10^{- 3}$
= 16 kJ.