At 1.0133 bar,the heat of sublimation of gallium is 277 kJ $\mathrm { mol } ^ { - 1 }$ and the heat of vaporization is 271 kJ $\mathrm { mol } ^ { - 1 }$ .To the correct number of significant figures,how much heat is required to melt 5.50 mol of gallium at 1.0133 bar?

Question

Quizplus · Accepted Answer

The heat of fusion can be calculated by subtracting the heat of vaporization from the heat of sublimation: 277 kJ/mol - 271 kJ/mol = 6 kJ/mol. For 5.50 mol, the heat required is 5.50 mol * 6 kJ/mol = 33 kJ.

At 10133 Bar,the Heat of Sublimation of Gallium Is 277 KJ