Question

The fluorocarbon c,cif has a normal boiling point of 47.6°c. the specific heats of c,cif3 (1) and c, cf3 (g) are 0.91 j/g-k and 0.67 j/g-k, respectively. the heat of vaporization of the compound is 27.49 kj/mol. the heat required to convert 50.0 g of the compound from the liquid at 5.0°c to the gas at 80.0°c is kj.

a) 276.68 kJ
b) 289.51 kJ
c) 305.24 kJ
d) 318.07 kJ

Answer 1

To calculate the energy required to heat and vaporize 50.0 g of the compound C2ClF3 from 5.0°C to 80.0°C, we must consider the heat needed to raise the temperature of the liquid and vapor, and the heat of vaporization.

Step-by-step explanation:

The heat required to convert 50.0 g of the compound from the liquid at 5.0°C to the gas at 80.0°C can be calculated by adding the heat required for three processes: heating the liquid from 5.0°C to its boiling point, vaporizing the liquid at its boiling point, and heating the vapor from the boiling point to 80.0°C.

To calculate the total heat (Q) required:
Then, sum these values: Q = Q1 + Q2 + Q3.
To find Q1 and Q3, we use the specific heats of the liquid and gas phases, respectively. For Q2, we use the heat of vaporization given in kJ/mol, converting it to J/g using the molar mass of C2ClF3, which is required to be known or given for calculation.

Finally, summing all heats calculated for the three steps gives the total energy required in kJ.