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

We’re being asked to determine how much energy (heat) is required to convert 52.0 g of ice at –10°C to steam at 100°C.

We’re going to calculate for the total heat required using the following steps:

*Step 1: **Calculate the heat required in raising the temperature of 52.0 g of ice from –10°C to 0°C (q _{1}).Step 2: Calculate the heat required to melt 52.0 g of ice to 52.0 g of water at 0°C (q_{2}).Step 3: Calculate the heat required in raising the temperature of 52.0 g of water from 0°C to 100°C (q_{3}).Step 4: Calculate the heat required to evaporate 52.0 g of water to 52.0 g of steam at 100°C (q_{4}).Step 5: Calculate the total heat required (q_{total}).*

How much energy (heat) is required to convert 52.0 g of ice at –10.0°C to steam at 100°C?

specific heat of ice: 2.09 J/g·°C ∆H_{fus} = 6.02 kJ/mol

specific heat of water: 4.18 J/g·°C ∆H_{vap} = 40.7 kJ/mol

specific heat of steam: 1.84 J/g·°C

A) 32.7 kJ

B) 108 kJ

C) 158 kJ

D) 40.2 kJ

E) 229 kJ