Final Answer:
To convert 37.0 g of
from a liquid at 13.50 °C to a gas at 98.60 °C, 9209.0114 J of heat are required.
Step-by-step explanation:
The heat required to convert a substance from one phase to another can be calculated using the following equation:
Q = mΔH
where:
Q is the heat required (J)
m is the mass of the substance (g)
ΔH is the enthalpy change for the phase transition (J/g)
The enthalpy change for the vaporization of C2Cl3F3 is 230 J/g. Therefore, the heat required to vaporize 37.0 g of C2Cl3F3 is:
Q_vaporization = (37.0 g) × (230 J/g) = 8470 J
In addition to the heat required for vaporization, we also need to consider the heat required to raise the temperature of the liquid
from 13.50 °C to 98.60 °C. The specific heat capacity of
is 0.222 J/g°C. Therefore, the heat required to raise the temperature of the liquid is:
Q_liquid = (37.0 g) × (0.222 J/g°C) × (98.60 °C - 13.50 °C) = 734.0114 J
Therefore, the total heat required to convert 37.0 g of
from a liquid at 13.50 °C to a gas at 98.60 °C is:
Q_total = Q_vaporization + Q_liquid = 8470 J + 734.0114 J = 9204.0114 J
Therefore, 9209.0114 J of heat are required to convert 37.0 g of
from a liquid at 13.50 °C to a gas at 98.60 °C.