Question

You drop 330 g of solid ice at −35°C into a bucket of water (1,200 g) at 45°C. Eventually, the ice all melts, and the entire system comes into thermal equilibrium. Find the final temperature of the system.

Answer 1

Using principle of caloriemetry

heat lost by water = heat gained by water

m_w*S_w*dT1 = (m_ice*S_ice*dT2) + (m_ice*Lf) + (m_ice*S_water*T)

m_w is the mass of the water

S_w is the specific heat capacity of water

dT1 is the change in temperature of water

dT2 is the change in temperature of ice
L_f is the latent heat of fusion of ice

S_ice is the specific heat capacity of ice

1200*4.186*(45-T) = (330*2.108*(35-0)) + (330*333.55)+(330*4.186*T)

final temperature is T = 14.306deg C