Answer:
3.75×10⁴ J
Explanation:
We'll begin by calculating the heat required to change the temperature of the ice. This can be obtained as follow:
Mass (M) = 0.1 Kg
Initial Temperature (T₁) = –20 °C
Final temperature (T₂) = 0 °C
Specific heat capacity (C) = 2060 J/kg°C
Heat (Q₁) required to change the temperature of ice =?
Q₁ = MCΔT
Q₁ = 0.1 × 2060 × (0 – –20)
Q₁ = 0.1 × 2060 × (0 + 20)
Q₁ = 206 × 20
Q₁ = 4120 J
Next, we shall determine the heat required to melt the ice. This can be obtained as follow:
Mass (M) = 0.1 Kg
Heat of fusion (Hբ) = 334000 J/kg
Heat (Q₂) required to melt the ice =?
Q₂ = MHբ
Q₂ = 0.1 × 334000
Q₂ = 33400 J
Finally, we shall determine the total heat absorbed. This can be obtained as follow:
Heat (Q₁) = 4120 J
Heat (Q₂) = 33400 J
Total heat (Q) =?
Q = Q₁ + Q₂
Q = 4120 + 33400
Q = 37520
Q = 3.75×10⁴ J
