An 23.0-g piece of an unidentified metal was heated from 23.5°C to 89.0°C. If 362 J of heat energy was absorbed by the metal in the heating process, what was the identity of the metal?

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A. copper
Incorrect. The heat energy absorbed by copper is 587 J.

B. gold
Incorrect. The heat energy absorbed by gold is 196 J.

C. mercury
Incorrect. The heat energy absorbed by mercury is 211 J.

D. silver
Correct! The heat energy absorbed by silver is 362 J. The equation for the amount of heat energy is equal to the specific heat X mass X change in temperature.

The specific heat of copper is about 0.4 J/grams • °C. How much heat is needed to change the temperature of a 30-gram sample of copper from 20.0°C to 70.0°C?

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A. 90 J
Incorrect. Amount of Energy = Specific heat X mass X change in temperature.

B. 50 J
Incorrect. Amount of Energy = Specific heat X mass X change in temperature.

C. 600 J
Correct! Amount of Energy = Specific heat X mass X change in temperature.

D. 150 J
Incorrect. Amount of Energy = Specific heat X mass X change in temperature.

If a calorimeter's ΔH is +1550 Joules, what was the change in heat inside of the cup?

A. +1550
Incorrect. The heat gained by the calorimeter is equal to the heat lost by the system.

B. -1550
Correct! The heat gained by the calorimeter is equal to the heat lost by the system.

C. +3100
Incorrect. The heat gained by the calorimeter is equal to the heat lost by the system.

D. 0
Incorrect. The heat gained by the calorimeter is equal to the heat lost by the system.