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A coffee cup calorimeter containing 200 g of water at 24°C had a 200 g sample of metal heated to 90°C placed in it. The final temperature of the water was measured to be 32°C. If no heat was lost to the surroundings, which of the following statements can be made about this experiment? The final temperature is less than the average starting temperature of the metal and the water; therefore the total energy of the metal and water decreased. The metal temperature changed more than the water temperature did, but the metal lost the same amount of thermal energy as the water gained. The metal temperature changed more than the water temperature did; therefore the heat capacity of the metal must be greater than the heat capacity of the water. O The metal temperature changed more than the water temperature did; therefore the metal lost more thermal energy than the water gained.

A coffee cup calorimeter containing 200 g of water at 24°C had a 200 g sample of metal heated to 90°C placed in it. The final temperature of the water was measured to be 32°C. If no heat was lost to the surroundings, which of the following statements can be made about this experiment? The final temperature is less than the average starting temperature of the metal and the water; therefore the total energy of the metal and water decreased. The metal temperature changed more than the water temperature did, but the metal lost the same amount of thermal energy as the water gained. The metal temperature changed more than the water temperature did; therefore the heat capacity of the metal must be greater than the heat capacity of the water. O The metal temperature changed more than the water temperature did; therefore the metal lost more thermal energy than the water gained.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.28QP: Consider the following specific heats of metals. Metal Specific Heat copper 0.385 J/(gC) magnesium...
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A coffee cup calorimeter containing 200 g of water at 24°C had a 200 g sample of metal heated to 90°C placed in it. The final temperature of the water was measured to be 32°C. If no heat was lost to the surroundings, which of the following statements can be made about this experiment? The final temperature is less than the average starting temperature of the metal and the water; therefore the total energy of the metal and water decreased. The metal temperature changed more than the water temperature did, but the metal lost the same amount of thermal energy as the water gained. The metal temperature changed more than the water temperature did; therefore the heat capacity of the metal must be greater than the heat capacity of the water. O The metal temperature changed more than the water temperature did; therefore the metal lost more thermal energy than the water gained.
Transcribed Image Text:A coffee cup calorimeter containing 200 g of water at 24°C had a 200 g sample of metal heated to 90°C placed in it. The final temperature of the water was measured to be 32°C. If no heat was lost to the surroundings, which of the following statements can be made about this experiment? The final temperature is less than the average starting temperature of the metal and the water; therefore the total energy of the metal and water decreased. The metal temperature changed more than the water temperature did, but the metal lost the same amount of thermal energy as the water gained. The metal temperature changed more than the water temperature did; therefore the heat capacity of the metal must be greater than the heat capacity of the water. O The metal temperature changed more than the water temperature did; therefore the metal lost more thermal energy than the water gained.
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