The specific heat capacity of silver is 0.235 J/g ∙ K. Its melting point is 962 °C, and its enthalpy of fusion is 11.3 kJ/mol. What quantity of energy, in joules, is required to change 9.70 g of silver from a solid at 25 °C to a liquid at 962 °C?

The total heat required for the conversion process is 1228.5 J

Explanation:

The processes involved in the given problem are:  

To calculate the amount of heat absorbed, we use the equation:

where,

= amount of heat absorbed = ?

= specific heat capacity = 0.235 J/g.K

m = mass of silver = 9.70 g

= final temperature = 1235 K

= initial temperature = 298 K

Putting all the values in above equation, we get:

To calculate the amount of heat released, we use the equation:

where,

= amount of heat absorbed = ?

m = mass of silver = 9.70 g

= latent heat of fusion = 11.3 kJ/mol =   (Conversion factor:  1 kJ = 1000 J; Molar mass of silver = 108 g/mol)

Putting all the values in above equation, we get:

Total heat required for the conversion =

Total heat required for the conversion =

Hence, the total heat required for the conversion process is 1228.5 J