Question

Question #8b463

Answer 1

The amount of energy that must be removed is 29.7 kJ.

Explanation:

The formula for the heat involved is

`color(blue)(|bar(ul(color(white)(a/a) q = -nΔ_"fus"H^°color(white)(a/a)|)))" "`

where

`n` = number of moles and

`Δ_"fus"H^°` = molar enthalpy of fusion

`Δ_"fus"H^° = "2.52 kJ/mol"`.

∴ `q = 1814 color(red)(cancel(color(black)("g CCl"_4))) × (1 color(red)(cancel(color(black)("mol CCl"_4))))/(153.82 color(red)(cancel(color(black)("g CCl"_4)))) × "-2.52 kJ"/(1 color(red)(cancel(color(black)("mol CCl"_4)))) = "-29.7 kJ"`