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

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Heating and Cooling Curves concept. You can view video lessons to learn Heating and Cooling Curves. Or if you need more Heating and Cooling Curves practice, you can also practice Heating and Cooling Curves practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Brydges' class at UCSD.