How Does Dropping a Hot Copper Cylinder into Water Lead to Boiling?

[Ready2GoXtr]

Homework Statement

A 150 g copper bowl contains 220 g of water, both at 20C. A very hot 300 g copper cylinder is dropped into the water, causing the water to boil, with 5.00 g being converted to steam. The final temperature of the system is 100C. Neglect energy transfers with the environment. (a) How much energy (incalories) is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature of the cylinder?

Homework Equations

Q=C(delta)T
Lv = 539cal/g

The Attempt at a Solution

Q=(1cal/g*k)(220g)(80k) = 17.6 kcal
Lv = 539cal/g 539cal/g(5) =2.69kcal
a)Q water = 17.6 + 2.69 = 20.3 Kcal
b)Q = (.0923/g*k) (150g) (80k) = 1.11 K cal
c) Not sure.

 

[anathema]

But since the final temperature is 100C and the original temperature of the water and bowl is 20C, it can be assumed that the original temperature of the cylinder was much higher, possibly above 100C.

 

[baba89]

Need more information about the specific heat capacity of the cylinder and its initial temperature in order to calculate the energy transferred to it.