Determine the following regarding both sensible and latent heat:?

Question

60 Calories is added to 1 gram of water at an initial temperature of 80 degrees Celcius. What is the water's final temperature and state (solid, liquid, or vapor)?

Answer 1

1 Calorie is the amount of heat needed to raise the temp of liquid water in 1 degree C. Assuming constant pressure of 1 ATM, you would need 20 calories to raise the temp of 1gr of water from 80 to 100 C(Sensible heat), where it starts the vaporization at constant temperature (Latent heat of vaporization). So you would need something around 540 Cal to fully evaporate 1 g of water (I don't remember the exact number, you would have to search it). So you only have 40 extra calories left, this way you would only evaporate a fraction of the water (40 divided by 540) and in the end you will have both liquid and vapor phases at the equilibrium temp of 100 C.

I wish to clarify one thing, the specific heat of water, as with most substances in the universe, varies with temperature. The above assumption that you need 20 Cal to raise temperature from 80 to 100C is not entirely accurate (and would need to investigate an empyrical equation and integrate it using the limits 80 and 100C), but for most school homework, it is ok to assume 1 Cal/g as specific heat at all temperature ranges.