Answer:
3758 kJ
Explanation:
Given:
Mass of the ice = 10 kg = 10 × 1000 = 10,000 g
Initial temperature of the ice = -20° C
Now,
The ice will start to melt when it will reach a temperature of 0° C
and, specific heat of ice, C = 2090 J/kg
Therefore,
Heat required to heat the ice from -20° C to 0° C
Q₁ = mCΔT
or
Q₁ = 10 × 2090 × (0 - (-20 ))
or
Q₁ = 418000 J
also,
Heat of fusion required to change the ice into liquid without any change in temperature.
For ice the heat of fusion = 334 J/g
Hence,
Energy needed by ice to melt, Q₂ = 334 × 10,000 J = 3,340,000 J
Hence, the total heat required = Q₁ + Q₂
= 418000 J + 3,340,000 J
= 3758000 J
= 3758 kJ
