How much heat is absorbed to change 13.8 grams of H2O from a solid to a liquid at zero degrees Celsius? ΔHfusion = 6.03 kJ/mol ΔHvaporization = 40.65 kJ/mol

31.1 kJ
561 kJ
4.62 kJ
83.2 kJ

Question

How much heat is absorbed to change 13.8 grams of H2O from a solid to a liquid at zero degrees Celsius? ΔHfusion = 6.03 kJ/mol     ΔHvaporization = 40.65 kJ/mol
		
31.1 kJ
561 kJ
4.62 kJ
83.2 kJ

aaronq · Answer

The problem asks about the latent heat (the heat involved in the phase change from solid to liquid).

All you have to do it scale the given enthalpy of fusion to the grams given (which you have to convert to moles, n).

 $H=\Delta H_{fusion}*n_{water}$