Verified answer

OK There are two parts to this.

First you have to heat the solid silver from 20 °C to solid silver at 962 °C

Heat required = mass * specific heat * (change in temperature)

{Using my value for specific heat of silver}

= 1.55 kg * 238.6 J/(kg°C) * (262 - 20) °C

= 89500 J

= 89.5 kJ

Then you have to provide enough extra [latent] heat to turn the solid silver at 962 °C into liquid silver at 962 °C

Heat required = mass * latent heat of fusion

{Using your value for latent heat of fusion (Hf) of silver}

= 1.55 kg * 111 kJ/kg

= 172 kJ

Total heat energy = 89.5 + 172 = 261.5 kJ

you have to define "Hf" otherwise it is meaningless but we can look up the needed numbers

Molar heat capacity: 25.350 J/(mol·K)

Molar heat capacity: 25.350 J/(mol·K) / 107.9 g/mol = 0.235 J/gK

Heat of fusion: 11.28 kJ/mol

heat of fusion: 11.28 kJ/mol / 107.9 g/mol = 0.1045 kJ/g = 104.5 J/g

atomic mass 107.9 g/mol

melt point 962ºC

Energy to warm silver from 20º to 962ºC = 1550g x 0.235 J/gK x (962–20) = 343000 J

Energy to melt silver = 1550g x 104.5 J/g = 162000 J

total = 505000 J or 505 kJ