chemistry
posted by Lauren on .
How many grams of ice at 11.2 degrees C can be completely converted to liquid at 29.8 degrees C if the available heat for this process is 4.12×10^3 kJ?
For ice, use a specific heat of 2.01 J/(g*degrees C) and delta H_fus = 6.01 kJ/mol.

How much heat is needed to raise the temperature of ice at 11.2 C to 0 C? That will x grams x 2.01 J/g*C x 11.2 = 22.51x.
How much heat is needed to melt the ice?
That will be xgrams x 333.6 J/g = 333.6x.
How much heat is needed to raise the temperature from 0C to 29.8.
That will be x grams x 4.186 x (29.8) = 124.7x
Total = 124.7x + 22.51x + 333.6x = ?x
?x = 4120J
Solve for x.