Heat curve problem 1 in page 10 of workbook

[204635822]

Isnt the heat capacity of a liquid greater than that of a solid? SO shouldnt the answet to #1 on pg 10 of workbook supposed to be B?

[Chem_Mod]

Hi can you post the question in full so that we can help you?

[Anthony Rosas 2K]

You're thinking about trends you've seen. Maybe that's the case usually, maybe not, but you cannot generalize. Look at the actual heating curve given in the question.

Heat capacity is the energy required to raise the temperature of any substance by 1 degree C, or whatever the units of temperature you'd like to use. The greater the heat capacity, the less of an affect or change in temperature there will be on the substance. Look at the curve again. The slope of the solid is smaller (not as steep of a rise) than the slope of the liquid which is much steeper. As you increase heat in kJ/mol (read the curve from left to right), the slope of the liquid rising much more quickly shows that it is more affected by the change in heat, therefore has a smaller heat capacity than the solid. So this answer is true.

The same goes for the next answer choice. The slope of the gas is much steeper, therefore has a smaller heat capacity, than the slope of the liquid. Basically, the greater the heat capacity, the less of an affect a temperature change has on a substance, hence the more horizontal and less steep of a slope and vice versa. I hope this helps.

[DrewGomberg_1D]

I struggled with the idea of which heat capacity / phase change involved greater heat to raise in temperature per mole as well. I believe the easier way to think about it is that the higher the slope of the line is the more temperature increase you get per mole with a given amount of heat added. So the higher the slop the lower the standard heat capacities should be because you essentially get more temperature increase with the allotted amount of energy.

[Chem_Mod]

Your method of thinking about the slope is right. Well done!