An aluminium pot has a mass of 200g and contains 400g of ice at 0°C. How much heat would be needed to melt that ice and then raise the temperature of the resulting water to 20°C. The specific heat capacity of water and aluminium are 4200 J Kg ^-1 and 910 J Kg ^-1 respectively, and the latent heat of fusion of ice is 330 KJ/Kg.
My attempt so far is as follows:
Heat from ice to water - Q = mL = .4Kg x 330x10^3J = 132x10^3J
Heat for water from (0°C to 20°C) - Q = mcΔT = .4Kg x 4200 x (20-0) = 33.6x10^3J
Heat for pot from (0°C to 20°C) - Q = mcΔT = .2Kg x 910 x (20-0) = 3.64x10^3J
Thus the answer is 3.64x10^3J + 33.6x10^3J + 132x10^3J = 169.24x10^3J
I don't know how to do this question but would try go this way about it, however it looks terribly wrong to me and would like some help please.