Question

The enthalpy of fusion for H2O is 6.0 kJ mol-1. How many grams (to 1 decimal place) of ice can be converted to liquid water at 0°C using 43 kJ of energy?

This is what they said to work out the answer:
First calculate the number of moles of ice that can be converted, by dividing the energy supplied by the enthalpy of fusion. Then convert into grams.

But im still unsure on exactly how to work through it.

Answer 1

Answer on Question #43528 - Chemistry - Inorganic Chemistry

Question:

The enthalpy of fusion for $\mathrm{H}_2\mathrm{O}$ is $6.0\,\mathrm{kJ}\cdot\mathrm{mol}^{-1}$. How many grams (to 1 decimal place) of ice can be converted to liquid water at $0^{\circ}\mathrm{C}$ using $43\,\mathrm{kJ}$ of energy?

Solution:

Number of moles of ice, which can be converted to liquid water at $0^{\circ}\mathrm{C}$ using $43\,\mathrm{kJ}$:

$$n = \frac{Q}{\Delta H_{fus}^{o}} = \frac{43\,\mathrm{kJ}}{6.0\,\frac{\mathrm{kJ}}{\mathrm{mol}}} = 7.2\,\mathrm{mol}$$

Mass of 7.2 mol of ice:

$$m = n \cdot M_{H_2O} = 7.2\,\mathrm{mol} \cdot 18.0\,\frac{\mathrm{g}}{\mathrm{mol}} = 129.6\,\mathrm{g},$$

where $M_{H_2O}$ - molar mass of water.

Answer: 129.6 g

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