Question

Part A

It takes 55.0 J to raise the temperature of an 10.2 g piece of unknown metal from 13.0∘C to 25.0 ∘C. What is the specific heat for the metal?

Part B

The molar heat capacity of silver is 25.35 J/mol⋅∘C. How much energy would it take to raise the temperature of 10.2 g of silver by 15.4 ∘C ?

I got 36.9 J for B and its correct

Part C

What is the specific heat of silver?

Answer 1

Part A:

The amount of heat required , Q = mcdt

Where

m = mass of the metal piece = 10.2 g

c = specific heat capacity of the metal = ?

dt = change in temperature = final - initial

    = 25.0 - 13.0 oC

    = 12.0 oC

Q = heat absorbed = 55.0 J

Plug the values we get c = Q / (mdt)

                                     = 55.0 / ( 10.2 x 12.0)

                                     = 0.449 J/(g^oC)

Part B :

We knowe that the molar mass of silver is = 107.9 g/mol

Given molar heat capacity of silver is 25.35 J/mol⋅∘C

So specific heat capacity of silver = molar heat capacity of silver/molar mass

                                                  = 25.35 J/mol⋅∘C / 107.9(g/mol)

                                                  = 0.235 J/(g^oC)

So amount of heat required , q = mcdt

Where

m = mass of silver = 10.2 g

c = specific heat capacity of silver = 0.235 J/(g^oC)

dt = raise in temperature = 15.4 oC

Plug the values we get q = 10.2x0.235x15.4

                                     = 36.9 J

Part C :

specific heat capacity of silver = molar heat capacity of silver/molar mass

                                                  = 25.35 J/mol⋅∘C / 107.9(g/mol)

                                                  = 0.235 J/(g^oC)