A 150 g copper bowl contains 190 g of water, both at 22.0°C. A very hot 410 g co

Question

A 150 g copper bowl contains 190 g of water, both at 22.0°C. A very hot 410 g copper cylinder is dropped into the water, causing the water to boil, with 4.90 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature of the cylinder? The specific heat of water is 1 cal/g.K, and of copper is 0.0923 cal/g.K. The latent heat of vaporization of water is 539 Cal/kg. (a) Number (b) Number (c) Number Units Units Units

Explanation / Answer

a)

Heat Transfered to water

Qw=cwmw(T2-T1)+msLv

Qw=1*190*(100-22)+4.9*539

QW=17461 cal or 17.461 Kcal

b)

Heat transferred to bowl

QB=CBmB(T2-T1) =0.0923*150*(100-22)

QB=1080 Cal or 1.08 Kcal

c)

-QW-QB=Ccmc(Tf-Ti)

-1080-17461=0.0923*410*(100-Ti)

Ti=589.94oC

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