A 170 g copper bowl contains 190 g of water, both at 18.0 degree C. A very hot 4

Question

A 170 g copper bowl contains 190 g of water, both at 18.0 degree C. A very hot 490 g copper cylinder is dropped into the water, causing the water to boil, with 9.50 g being converted to steam. The final temperature of the system is 100 degree 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. Number Units Number Units Number Units

Explanation / Answer

a)

mw = mass of water = 190 g = 0.19 kg

c = specific heat = 4186

Ti = initial temperature = 18

Tf = final temperature = 100

L = heat of vapourization = 2230 J/g

m = mass converted to steam = 9.50 g

Heat transferred is given as

Q = mw c (Tf - Ti) + mL

Q = (0.19) (4186) (100 - 18) + (9.5) (2230)

Q = 86402.88 J

b)

for the bowl :

mc = mass of copper bowl = 0.170 kg

cc = specific heat of copper = 386

Qc = heat transferred to bowl = mc cc (Tf - Ti) = (0.170) (386) (100 - 18) = 5380.84 J

c)

heat of cylinder = heat given to water + heat given to bowl

M (386) (T - 100) = 86402.88 + 5380.84

(0.49) (386) (T - 100) = 86402.88 + 5380.84

T = 585.3

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