200 grams of metal (c = 1.25 J/g C) are combined with 80 grams of water inside a

Question

200 grams of metal (c = 1.25 J/g C) are combined with 80 grams of water inside a well insulated calorimeter. The metal starts with an initial temperature of 180 C and the water is initially at 20 C.

a) Determine the final temperature of the system upon reaching thermal equilibrium.

b) Which substance, the metal or the water, experienced a larger temperature change? Can you explain why this result occured?

c) Which substance, the metal or the water, experienced a larger transfer of heat during this process? Can you explain why this result occured?

d) Determine the change in entropy of the metal during this process.

e) Determine the change in entropy of the water during this process.

f) Determine the change in entropy of the system during this process.

Based on your answer would you conclude that this will be a reversible or irreversible process? Will there be more order or less order in the system as a result of this process.

Explanation / Answer

a)

Let the final Temperature = T

Heat lost by metal = Heat gained by water

mm cm (180 - T) = mw cw (T - 20)

200 (1.25) (180 - T) = 80 (4.2) (T - 20)

T = 88.3

b)

Metal experience larger temperature change since (180 - 88.3) > (88.3 - 20)

c)

heat transfered is equal . The heat lost by one is same as heat gained by the other. this is because no heat is allowed to leave the system.

d)

Q = mm cm (180 - T) = 200 (1.25) (180 - 88.3) = 22925 J

change in Entropy = Q / T = 22925 / 88.3 = 259.63

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