3. An 825 g iron block is heated to 352 °C and placed in an insulated container

Question

3. An 825 g iron block is heated to 352 °C and placed in an insulated container (of negligible heat capacity) containing 40.0 g of water at 20.0 °C. What is the equilibrium temperature of the system? If your answer is 100 °C, determine the amount of water that has vaporized. The average specific heat of iron over this temperature range is 560 J/(kg* K). 4. A large punch bowl holds 3.87 kg of Hawaiian punch (which is essentially water) at 20.1 °C. A 0.205 kg ice cube at -5.10 °C is placed in the punch. (a) How much heat is needed to melt all of the ice? (b) How much heat can be provided by the Hawaiian punch? (c) Is there any ice remaining, if so, how much? (d) What is the final temperature of the system? Ignore any heat exchange with the bowl or the surroundings.

Explanation / Answer

Answering Question 4 ( all 4 parts)

heaat gained by ice = heat supplied by hawaiian punch

specific heat of ice= 2093 J/kg C

a) Heat needed by ice = 0.205 ( 5.10 ) (2093) + 0,205 ( 334000) = 70658.23 J

b) Heaat supplied by hawaiian punch = 3.87 ( 20.1) ( 4181) = 325227.447 J

c) No

d) as heat supplied by hawaiian punch is more than heat required by ice to melt , final temp will be:

70658.23 J + 0.205 ( 4181) ( T) = 3.87 ( 20.1-T) ( 4181)

70658.23 J - 325227.447 J = - 17037.575 T

T = 14.94 C

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