A copper calorimeter can with mass 0.100kg contains 0.160kg of water and 0.018kg of ice in thermal equilibrium at atmospheric pressure.
Part A
If 0.750kg of lead at a temperature of 255 c is dropped into the calorimeter can, what is the final temperature? Assume that no heat is lost to the surroundings

Explanation:

The given data is as follows.

  Mass of copper calorimeter, () = 0.1 kg

 specific heat of copper calorimeter, () = 390 J/kg K

  mass of water, () = 0.160 kg

  specific heat of water, () = 4190 J/kg K

    mass of ice, () = 0.018 kg

latent heat of ice =

mass of lead, () = 0.75 kg

specific heat of lead, () = 130 J/kg K

Heat lost by the lead is

           Q =

               =

                = 97.5 (255 - T)

Now, heat gained by calorimeter is calculated as follows.

        Q =

           =

Hence, heat loss by lead is equal to heat gained by calorimeter .

So,      97.5 (255 - T ) = 745.82 T + 39 T + 6012

             18850.5 = 882.32 T

                 T =

Thus, we can conclude that the value of final temperature is .

see earlier answer