Problem: The heat of vaporization of water at 373 K is 40.7 kJ/mol.Find q for the evaporation of 451 g of water at this temperature.

FREE Expert Solution

We’re being asked to determine the heat (q) of the evaporation of 451 g of water at 373 K.


Recall that heat will be absorbed when water is being evaporated (phase change). Calculate heat (q) using the equation:

q=n·∆Hvap

q = heat, J
n = number of moles (mol)
ΔHvap = heat of vaporization, kJ/mol

95% (176 ratings)
View Complete Written Solution
Problem Details

The heat of vaporization of water at 373 K is 40.7 kJ/mol.

Find q for the evaporation of 451 g of water at this temperature.

Learn this topic by watchingHeat Capacity Concept Videos
All Chemistry Practice Problems Heat Capacity Practice Problems
Q.A 1-kg cylinder of aluminum and 1-kg jug of water, both at room temperature, are put into a refrigerator. After one hour, the temperature of each obje...
Q.Which sample is most likely to undergo the smallest change in temperature upon the absorption of 100 kJ of heat?a) 15 g waterb) 15 g leadc) 50 g water...
Q.A 13.0 g sample of granite initially at 82.0 oC is immersed into 26.0 g of water initially at 23.0 oC. What is the final temperature of both substance...
Q.The heat of combustion of liquid octane (C8H18) to carbon dioxide and liquid water at 298 K is -1303 kJ/mol. Find ΔE for this reaction.
See all problems in Heat Capacity

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Heat Capacity concept. You can view video lessons to learn Heat Capacity. Or if you need more Heat Capacity practice, you can also practice Heat Capacity practice problems.