Help with chemistry question?

[acfm]

A question has been proposed in my CHM class. I believe I have the answer but just wnated to rund it by the experts for varification.

Question: As a purity check for industrial diamonds, a 10.25 carat diamond is heated to 74.21 degree C and immersed in 26.06 g of water in a constant-pressure calorimeter (1 carat = 0.2000 g). The initial temperature of the water is 27.20 degree C. Calculate delta T, of the water and the diamond ( C diamond = 0.519 J/g. K.)

My answer:
I assumed STP. In making this assumption, the delta T of water is 2.2 degress C.
The delta T of the diamond is 49.21 degrees C.

Does this seem to be resonable? For this problem, can it be just that simple???

Thanks in advance for any inputs!

 

If I have understood you correctly:
The system (water+diamond) does not exchange any energy with the surroundings - the change in energy from start to finish equals zero.
At equilibrium the system will have the temperature Teq.

Thus,
2.05 g * 0.519 J/gK * (74.21°C - Teq) + 26.06 g * 4.18 J/gK * (27.2°C - Teq) = 0

Solve for Teq.