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