How much energy ( in kilojoules) is required to melt 160 g of ice and raise the temperature to 77°c

Given:  

Mass of ice, m = 160 g

Initial temperature of ice T1 = 0 c

Final temperature, T2 = 77 C

 To determine:

The heat required to melt ice

Explanation:

The heat (Q) required is given as:

Q = Heat of fusion of ice + Heat required to raise the temperature of water

Q = mΔHfusion + mcΔT

Now, ΔH(fusion of ice) = 333.55 J/g

specific heat of water, c = 4.18 J/gC

Q = 160 g * 333.55 J.g-1 + 160 g * 4.18 J/gC *(77-0) C

Q = 53368 J + 51498 J  = 104866 J

Ans: Heat required = 104.87 kJ

the product of the pressure and volume is also constant