Answer:
(a) 672000 J
(b) 258300 J
(c) 30.75 °C
Explanation:
(a) Energy required to melt the ice = Latent heat of fusion of ice
Latent heat of fusion of ice (Q₁) = lm............................. Equation 1
Where l = specific latent heat of fusion of ice, m = mass of ice
Given: m = 2.00 kg
Constant : l = 336000 J/kg
Substituting these values into equation 1,
Q₁ = 336000 × 2
Q₁ = 672000 J.
Energy required to melt the ice = 672000 J
(b) The Energy remains to raise the temperature of the liquid water = Total Energy - Energy requires to melt the ice.
Given: Total Energy = 9.303 × 10⁵ J, = 930300 J
Energy remain to raise the temperature of the liquid water =
930300 - 672000
Total Energy = 258300 J
Energy remain to raise the temperature of the liquid water = 258300 J.
(c): Q = cmΔT ............. equation 2
Where c = specific heat capacity of water, m = mass of water, ΔT = change in temperature, Q = Energy required to change the temperature of liquid water
Making ΔT the subject of formula in the equation above,
ΔT = Q/cm........................................... Equation 3
Given: m = 2.00 kg, Q = 258300 J
Constant: C = 4200 J/kg. K
Substituting these values into equation 3
ΔT = 258300/(4200×2)
ΔT = 258300/8400
ΔT = 30.75 K
But ΔT = T₂ - T₁
Where T₁ initial temperature, T₂ = final Temperature
T₂ = T₁ + ΔT,
Given: T₁ = 0 °C
Therefore,
T₂ = 30.75 + 0 = 30.75
T₂ = 30.75 °C
Final temperature of water = 30.75 °C
