Final answer:
The total heat required to melt 20.50 kg of silver, initially at 15 °C, is calculated by first raising the temperature of the silver to its melting point and then melting it, which results in a total heat requirement of 6276.17 kJ.
Step-by-step explanation:
To calculate the amount of heat required to melt 20.50 kg of silver, we'll first need to raise its temperature from 15 °C to its melting point at 961 °C using its specific heat capacity, and then melt it using the heat of fusion. The heat needed to raise the temperature, Q1, is calculated using the formula Q1 = m * c * ΔT, where m is the mass of the silver, c is the specific heat, and ΔT is the change in temperature. And to calculate the heat needed to melt the silver, Q2, use the formula Q2 = m * Lf, where Lf is the latent heat of fusion.
Firstly, to raise the silver to its melting point:
Mass of silver, m = 20.50 kg
Initial temperature, T1 = 15 °C
Final temperature (melting point), T2 = 961 °C
Specific heat of silver, c = 230 J/kg°C
ΔT (change in temperature) = T2 - T1 = 961 °C - 15 °C = 946 °C
Q1 = 20.50 kg * 230 J/kg°C * 946 °C = 4,472,170 J or 4472.17 kJ
Secondly, to melt the silver:
Latent heat of fusion of silver, Lf = 88 kJ/kg
Q2 = 20.50 kg * 88 kJ/kg = 1,804 kJ
Therefore, the total heat required to melt 20.50 kg of silver equals the sum of Q1 and Q2: 4472.17 kJ + 1804 kJ = 6276.17 kJ.