For most solids at room temperature, the specific heat is determined by oscillations of the atom cores in the lattice (each oscillating lattice site contributes 3kT of energy, by equipartition), as well as a contribution from the mobile electrons (if it's a metal). At room temperature the latter contribution is typically much smaller than the former, so we will ignore it here. In other words, you can reasonably estimate the specific heat simply by counting the number of atoms! Use this fact to estimate the specific heat of copper (atomic mass = 63.6), given that the specific heat of aluminum (atomic mass = 27.0) is 900 J/kg-K.

The specific heat of copper is  

Explanation:

From the question we are told that

The amount of energy contributed by each oscillating lattice site  is  

       The atomic mass of copper  is  

        The atomic mass of aluminum is  

        The specific heat of aluminum is  

 The objective of this solution is to obtain the specific heat of copper

       Now specific heat can be  defined as the heat required to raise the temperature of  1 kg of a substance by  

  The general equation for specific heat is  

Where is the change in temperature

              is the change in internal energy

The internal energy is mathematically evaluated as

      Where   is the Boltzmann constant with a value of

                    T is the room temperature

                      n is the number of atoms in a substance

Generally number of  atoms in mass of an element can be obtained using the mathematical operation

Where is the Avogadro's number with a constant value of  

          M is the atomic mass of the element

           m actual mass of the element

  So the number of atoms in 1 kg of copper is evaluated as  

The number of atom is  

Now substituting the equation for internal energy into the equation for specific heat

Substituting values

93.2 ml + 3920 ml = 4013 ml total  

(93.2 ml) * (2.03 m) / (4013 ml) = 0.0471 m

the volume in in l of the diluted solution would be 0.0471 m.