Chemistry
posted by Chris on .
A 271g sample of nickel at 94.1°C is placed in 100.0 mL of water (density = 1.00 g/mL) at 23.9°C. What is the final temperature of the water?
[Assume that no heat is lost to or gained from the surroundings. Specific heat capacity of nickel = 0.444 J/(g·K) and of water = 4.184 J/(g·K).]

heat lost by Ni + heat gained by H2O = 0
[mass Ni x specific heat Ni x (TfinalTinitial)] + [mass H2O x specific heat H2O x (TfinalTinitial)] = 0 
Would I have to rearrange the equation to solve for the final temp of the water?

You can but that's the hard way to do it. It is much easier to substitute the individual numbers and work it out by pieces.

Do I already know the final temp of the nickel because I don't know where to start even though you have given me the equation.

No, of course you don't know the final T. That's what you're trying to find. It ways that in the problem, "What is the final T if ..."
heat lost by Ni + heat gained by H2O = 0
[mass Ni x specific heat Ni x (TfinalTinitial)] + [mass H2O x specific heat H2O x (TfinalTinitial)] = 0
mass Ni = 271 g
specific heat Ni = 0.444
Tinitial Ni = 94.1 C
Tfinal = ?
mass H2O = 100 mL and since water has density of 1.00 g/mL, this is 100 g.
specific heat H2O = 4.184
Tinitial H2O = 23.9 C
Tfinal = ?
Note: Tfinal for Ni and Tfinal for H2O will be the same T since that is where equilibrium will be attained; i.e., when the Ni has lost heat and the H2O has gained heat and both are at the same final temperature. 
Okay. Thanks for clarifying the problem for me.