Question
A 170g copper bowl contains 200g of water, both at 21C. A very hot 490g copper cylinder is dropped into the water, causing the water to boil with 16.8 g being changed to steam. The final temp of the system is 100C. Ignore energy transfers with the environment.
(a) How much energy (in calories) is transferred to the water as heat?
(b) How much to the bowl?
(c) What is an original temp (in Celsius) of the cylinder? The specific heat of water is 1 cal/g*K, and a copper is 0.0923 cal/ g*K. The latent heat of vaporization of water is 539 Cal/Kg.