ok my final exam for chem is tomorrow and i need help badly on this practice problem! here it is:(adsbygoogle = window.adsbygoogle || []).push({});

3. When 9.250 kJ of heat is added to 20.0 g of ice at 0.0 degrees Celcius, what is the final temperature of the water? The heat of fusion for water is 335 J/g.

I don't know how on earth to connect the fact that i was given the "fusion" (fusion - huh???) of water with the other stuff. I know that q=(c)(m)(delta T) but how do i connect all this together?

this is what i did (and failed misrebaly):

q=(c)(m)(delta T); m=20.0 g; T initial=0.0 degrees Celcius; q=9.250 kJ (which is 9250 J if i wanted to work with the same units)

so:

9250 J=[4.184J/(g*degree Celcius)](20.0 g)(T final - 0.0 deg. Celcius)

9250 J=(83.68)(T final)

111 deg. Celcius=T final

WRONG!!

HELP PLEASE! :uhh:

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# Fusion related problem (help please, chem final is tomorrow!)

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