Determine the amount of heat that is required to turn 2 kg ice taken at 0 ° C into water and when the resulting water

Determine the amount of heat that is required to turn 2 kg ice taken at 0 ° C into water and when the resulting water is heated to a temperature of 30 ° C. The specific heat of melting of ice is 34 · 10 ^ 4 J / kg, and the specific heat of water is 4200 J / (kg · ° C).

The amount of energy required to melt and heat:
Q = Q1 + Q2.
Q1 = λ * m, λ is the specific heat of melting of ice (λ = 34 * 10 ^ 4 J / kg), m is the mass of ice (m = 2 kg).
Q2 = C * m * (tк – tн), C – specific heat capacity of water (С = 4200 J / (K * kg)), tк – final temperature (tк = 30 ºС), tн – initial temperature (tн = 0 ºС ).
Let’s calculate the required amount of energy:
Q = Q1 + Q2 = λ * m + C * m * (tк – tн) = (34 * 10 ^ 4) * 2 + 4200 * 2 * 30 = 680000 + 252000 = 932000 J = 932 kJ.
Answer: You need to spend 932 kJ of energy.