Question

3. a) An experiment was performed where a piece of metal weighing 2.948 g was heated to 98.2 °C. A 48.3-mL sample of water was added to a calorimeter and measured to be 23.4 °C. The hot metal was placed in the water and the final temperature of the mixture was found to be 32.8 °C. Calculate the heat energy change of the water (Qwater). Assume that the density of water is 1.00 g/mL and its specific heat is 1.00 cal/g·°C. Answer b) Assume that all the heat absorbed by the water was heat lost by the metal. With this information, calculate the specific heat of the metal object.

          3. a) An experiment was performed where a piece of metal weighing 2.948 g was heated to 98.2 °C. A 48.3-mL sample of water was added to a calorimeter and measured to be 23.4 °C. The hot metal was placed in the water and the final temperature of the mixture was found to be 32.8 °C. Calculate the heat energy change of the water (Qwater). Assume that the density of water is 1.00 g/mL and its specific heat is 1.00 cal/g·°C.
Answer
b) Assume that all the heat absorbed by the water was heat lost by the metal. With this information, calculate the specific heat of the metal object.

3. a) An experiment was performed where a piece of metal weighing 2.948 g was heated to 98.2 °C. A 48.3-mL sample of water was added to a calorimeter and measured to be 23.4 °C. The hot metal was placed in the water and the final temperature of the mixture was found to be 32.8 °C. Calculate the heat energy change of the water (Qwater). Assume that the density of water is 1.00 g/mL and its specific heat is 1.00 cal/g·°C.
Answer
b) Assume that all the heat absorbed by the water was heat lost by the metal. With this information, calculate the specific heat of the metal object.

Added by Dwayne J.

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