🤓 Based on our data, we think this question is relevant for Professor Woolman's class at MSCD.

The ** amount of energy (q)** needed to freeze a given mass is calculated using:

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{n}}{\mathbf{\times}}{{\mathbf{\Delta H}}}_{{\mathbf{vaporization}}}}$

where:

**n** = number of moles

**ΔH _{vaporization}** = heat of vaporization (in J/mol)

We’re given:

m = **422** ** g**

ΔH_{vaporization}** = 40.65 kJ/mol**

Since we are given the mass of liquid water, we need to determine the number of moles of water.

The molar mass of H_{2}O is 18.016 g/mol.

How much heat is required to convert 422 g of liquid H_{2}O at 23.5 °C into steam at 150 °C?