The enthalpy of fusion of ice is 6.020 kJ/mol. The heat capacity of liquid water is 75.4 J/mol$\infty$C. What is the smallest number of ice cubes at 0$\infty$C, each containing 1 mol of water, necessary to cool 500. g of liquid water initially at 20$\infty$C to 0$\infty$C?

Question

Quizplus · Accepted Answer

To cool 500 g of water (which is approximately 27.78 mol) from 20°C to 0°C, the heat removed is calculated using q = m * C * ΔT. This equals 27.78 mol * 75.4 J/mol°C * 20°C = 41,888 J or 41.888 kJ. Each mole of ice absorbs 6.020 kJ when melting. Therefore, the number of moles of ice needed is 41.888 kJ / 6.020 kJ/mol ≈ 7 moles.

The Enthalpy of Fusion of Ice Is 6 ∞\infty∞ C What Is the Smallest Number of Ice Cubes at Heat

The Enthalpy of Fusion of Ice Is 6 $\infty$ C What Is the Smallest Number of Ice Cubes at Heat