Calculate the total quantity of heat required to convert 25.0 g of liquid ccl4(l) from 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 j/(g ∙ °c) its heat of fusion is 3.27 kj/mol and its heat of vaporization is 29.82 kj/mol.

The heat will be required for following processes

Q1 = heat required for heating of CCl₄ from 35⁰C to 76.8⁰C

Q2= heat required to convert liquid CCl₄ to gaseous CCl₄

Q1 = mass of CCl₄ X specific heat of CCl₄ X change in temperature

Q1 = 25 X 0.857 X (76.8-35) = 895.565J

Q2 = moles of CCl₄ X heat of vapourization of CCl₄

moles of CCl₄ = mass of CCl₄ / molar mass of CCl₄

moles ofCCl₄ = 25 / 153.82 = 0.162

Q2 = 0.162 X 29.82 kJ = 4.84575 kJ = 4845.75 J

Total energy = 895.565 + 4845.75 = 5741.315 J

the temperature of the gas, in k, not celsius.