Calculate the total quantity of heat required to convert 25.0 g of liquid CCl₄(l)at 35.0 °C to gaseous CCl₄ at 76.8 °C (the normal boiling point for CCl₄).The specific heat of CCl₄(l)is $0.857 \mathrm {~J} \mathrm {~g} ^ { - 1 } { } ^ { \circ } \mathrm { C } ^ { - 1 }$ its heat of fusion is $3.27 \mathrm {~kJ} \mathrm {~mol} ^ { - 1 }$ and its heat of vaporization is $29.82 \mathrm {~kJ} \mathrm {~mol} ^ { - 1 }$ A)0.896 kJ B)1.43 kJ C)5.74 kJ D)6.28 kJ

Question

Quizplus · Accepted Answer

To calculate the total heat required, we need to consider both the heat needed to raise the temperature of the liquid to its boiling point and the heat needed for the phase change from liquid to gas. First, calculate the heat required to raise the temperature from 35.0 °C to 76.8 °C using q = mcΔT. Then, calculate the heat required for vaporization using q = nΔHvap. Add these two values to get the total heat. The correct answer is 5.74 kJ.

Calculate the Total Quantity of Heat Required to Convert 25 0.857 J g−1∘C−10.857 \mathrm {~J} \mathrm {~g} ^ { - 1 } { } ^ { \circ } \mathrm { C } ^ { - 1 }0.857 J g−1∘C−1

Calculate the Total Quantity of Heat Required to Convert 25 $0.857 \mathrm {~J} \mathrm {~g} ^ { - 1 } { } ^ { \circ } \mathrm { C } ^ { - 1 }$