# Homework Help: HS Thermochemistry Problem

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1. Nov 5, 2014

### ThePageHendrix

1. The problem statement, all variables and given/known data

If 13.4 kJ of heat is added 1.00 kg of ice at 0ºC, how much ice will be melted

2. Relevant equations

Change of Heat = mass*change of temperature*constant

change of heat fusion (water) = 333 J/g

change of heat water vapor = 2260 J/g

change of heat total = change of heat (state) + change of heat (temp change)

constant of water = 4.184 J/gºC

constant of ice = 2.1 J/gºC
3. The attempt at a solution

(1000g)(2.1J/gºC)(?-0) + (13400g*333J/gºC)

2. Nov 5, 2014

### Staff: Mentor

Hi ThePageHendrix. Welcome to Physics Forums!!!

If it takes 333 kj to melt the entire 1 kg of ice, how much ice will only 13.4 kj melt?

Chet

3. Nov 5, 2014

### ThePageHendrix

Sorry, but it takes 333 joules, not kj, to melt the ice. I'm sorry, but I am just really lost on how to approach this problem.

Any more help is appreciated, thanks!

4. Nov 5, 2014

### Staff: Mentor

It takes 333J to melt 1 gm; it takes 333kJ to melt 1 kg.

5. Nov 6, 2014

### Staff: Mentor

This equation describes amount of heat when dealing with the temperature change. When the ice melts, temperature doesn't change (in such cases we say it is a "latent heat"). Latent heat requires different equation. Chet already pointed you at the intuition behind the other equation you need.