🤓 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 (q1).
Step 2: Calculate the heat required to melt 52.0 g of ice to 52.0 g of water at 0°C (q2).
Step 3: Calculate the heat required in raising the temperature of 52.0 g of water from 0°C to 100°C (q3).
Step 4: Calculate the heat required to evaporate 52.0 g of water to 52.0 g of steam at 100°C (q4).
Step 5: Calculate the total heat required (qtotal).
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 ∆Hfus = 6.02 kJ/mol
specific heat of water: 4.18 J/g·°C ∆Hvap = 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