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0.835 kJ is added to 10g ice @ zero-Celsius. The enthalpy of fusion for ice is 6 kJ/mol. What is the final temperature??

I do: (10g/1)*(1mol/18g)*(6.0kJ/mol) and get 3.33kJ to change the zero-

celsius ice to zero-celsius water; thus, my answer is zero-degrees Celsius.

Something MUST be wrong---What is it??

Perhaps I should use specific heat instead of enthalpy of fusion?....

Specific heat of ice = 1.8 J/C = 0.0018 kJ/C

if so, I find the temperature change as q/(m*Cp), and get

(835 J)/((10g/1)*(1mol/18g)*(1.8 J/C)) = 835 Change in Celsius??

(where 0.835 kJ = 835 J)

(so i convert everything to joules)