A copper container of 0.25-kg mass contains 0.4 kg of water. Container and water

Question

A copper container of 0.25-kg mass contains 0.4 kg of water. Container and water are initially at room temperature of 20° C as measured by a thermometer. A block of copper of 1-kg mass is heated to 100° C by placing in a steam from water boiling at normal atmospheric pressure. It is then removed from the steam and quickly placed in the water of the calorimeter. The copper block cools, the water in the container becomes warmer, and the final temperature as read on the thermometer, is found to be 34.5° C. From these data determine the specific heat capacity of the copper. A copper container of 0.25-kg mass contains 0.4 kg of water. Container and water are initially at room temperature of 20° C as measured by a thermometer. A block of copper of 1-kg mass is heated to 100° C by placing in a steam from water boiling at normal atmospheric pressure. It is then removed from the steam and quickly placed in the water of the calorimeter. The copper block cools, the water in the container becomes warmer, and the final temperature as read on the thermometer, is found to be 34.5° C. From these data determine the specific heat capacity of the copper.

Explanation / Answer

For water specific heat capacity Cp = 4180 J/kg/K

Heat lost by copper block = Heat gained by water + copper container

Heat lost = m*Cp*dT

1*Cp*(100 - 34.5) = 0.4* 4180 * (34.5 - 20) + 0.25 * Cp * (34.5 - 20)

65.5 Cp = 24244 + 3.625 Cp

Solving, Cp = 391.8 J/kg/K

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