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Problem- At 1 atm, how much energy is required to heat 75.0 g of H2O(s) at -12.0 degree C to H2O(g) at 153.0 degree C?

1) How much energy is needed to heat 75.0 of H2O(s) at -12.0 degree C?

2) How much energy is needed to melt 75.0 g of H2O(s) if its enthalpy of fusion is 333.6 J/g

3) How much energy is needed to heat 75.0 g of H2O (I) by 100 degree C if its specific heat is 4.184 J/(g x degree C)

4) How much energy is needed to boil 75.0 g of H2O (i) if its enthalpy of vaporization is 2257 J/g?

5) How much energy is needed to heat 75.0 g of H2O(g) by 53.0 degree C if its specific heat is 2.000 J/(g x degree C)

Please show me how work it out above problem

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