To find the total energy required to transform 25 kg of ice at 0°C into water at 20°C, we need to consider two processes:
Heating the ice from 0°C to 100°C to melt it
Heating the water from 0°C to 20°C
The total energy required will be the sum of the energy required for both processes.
Heating the ice:
Q1 = m * L1
Where:
m = mass of ice = 25 kg
L1 = latent heat of ice = 334.5 kJ/kg
Q1 = 25 kg * 334.5 kJ/kg
Q1 = 8362.5 kJ
Heating the water:
Q2 = m * c * ΔT
Where:
m = mass of water = 25 kg
c = specific heat of water = 4.18 kJ/kg°C
ΔT = temperature change = 20°C - 0°C = 20°C
Q2 = 25 kg * 4.18 kJ/kg°C * 20°C
Q2 = 2090 kJ
Total energy required:
Total energy = Q1 + Q2
Total energy = 8362.5 kJ + 2090 kJ
Total energy = 10452.5 kJ
Therefore, the total energy required to transform 25 kg of ice at 0°C into water at 20°C is 10452.5 kJ.