Problem: 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/molCliq = 4.18 J/g°CCgas = 2.01 J/g°CCsol = 2.09 J/g°CTmelting = 0°CTboiling = 100°CA) 52.7 kJ      B) 91.7 kJ      C) 87.7 kJ      D) 63.5 kJ      E) 10.9 kJ

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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.


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Problem Details

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