We’re being asked to calculate the amount of energy required to convert 36.0 g of liquid water at 65 ˚C to a gas at 115 ˚C. There are three heats involved in this problem:
1. q1 which is the heat in raising the temperature of 36.0 g of water from 65 ˚C to 100 ˚C
2. q2 which is the heat in evaporating 36.0 g of water at 100˚C
3. q3 which is the heat in raising the temperature of 36.0 g of water vapor from 100˚C to 115˚C
We need to solve for each heat individually then add them together to get the final answer.
How much energy is required to heat 36.0 g H 2O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful.
ΔHvap = 40.7 kJ/mol
Cliq = 4.18 J/g°C
Cgas = 2.01 J/g°C
Csol = 2.09 J/g°C
Tmelting = 0°C
Tboiling = 100°C
A) 52.7 kJ B) 91.7 kJ C) 87.7 kJ D) 63.5 kJ E) 10.9 kJ
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