An insulated container has 1.40 kg of water at a temperature of 62.0°C. The temperature of a 700-g copper block is 24.0°C. We drop the block into the water and wait until thermal equilibrium is established. Assume that the amount of heat lost to the container and the surroundings is negligible. Take the specific heats of copper and water to be 385 J/kg K and 4180 J/kg K, respectively. (a) Determine the final temperature of the water. D.
An insulated container has 1.40 kg of water at a temperature of 62.0°C. The temperature of a 700-g copper block is 24.0°C. We drop the block into the water and wait until thermal equilibrium is established. Assume that the amount of heat lost to the container and the surroundings is negligible. Take the specific heats of copper and water to be 385 J/kg K and 4180 J/kg K, respectively. (a) Determine the final temperature of the water. D.
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Answer A - D
Transcribed Image Text:An insulated container has 1.40 kg of water at a temperature of 62.0 C. The temperature of a 700-g
copper block is 24.0°C. We drop the block into the water and wait until thermal equilibrium is established.
Assume that the amount of heat lost to the container and the surroundings is negligible. Take the specific
heats of copper and water to be 385 J/kg K and 4180 J/kg K, respectively.
(a) Determine the final temperature of the water.
°C
(b) Determine the change in temperature of the copper block.
(c) Determine the amount of heat gained by the copper block.
J.
(d) The specific heat of silver is smaller than that of copper. If the bock were made of silver instead of
copper and everything else in the statement of the problem is the same, the final temperature of the
water would be higher.
O True
O False
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