The fluorocarbon C₂Cl₃F₃ has a normal boiling point of 47.6 °C. The specific heats of C₂Cl₃F₃(l)and C₂Cl₃F₃(g)are 0.91 J g^-1 °C^-1 and 0.67 J g^-1 °C^-1, respectively. The heat of vaporization of the compound is 27.49 kJ mol^-1. 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)8.19 B)1454 C)30.51 D)3031 E)10.36

Question

Quizplus · Accepted Answer

To find the total heat required, calculate the heat needed to raise the temperature of the liquid to its boiling point, the heat of vaporization, and the heat needed to raise the temperature of the gas. The calculations are as follows:  1. Heat to raise liquid from 5.0 °C to 47.6 °C: q1 = m * c * ΔT = 50.0 g * 0.91 J/g°C * (47.6 - 5.0) °C = 1935.8 J = 1.9358 kJ  2. Heat of vaporization: q2 = (50.0 g / 187.38 g/mol) * 27.49 kJ/mol = 7.33 kJ  3. Heat to raise gas from 47.6 °C to 80.0 °C: q3 = m * c * ΔT = 50.0 g * 0.67 J/g°C * (80.0 - 47.6) °C = 1086.6 J = 1.0866 kJ  Total heat = q1 + q2 + q3 = 1.9358 kJ + 7.33 kJ + 1.0866 kJ = 10.3524 kJ, which rounds to 10.36 kJ.

The Fluorocarbon C2Cl3F3 Has a Normal Boiling Point of 47

The Fluorocarbon C₂Cl₃F₃ Has a Normal Boiling Point of 47