A 5.00-g piece of lead at 85.0C and a 20.00g piece of aluminum at 65.0C are placed into a container of cold 20.0C water. After the two metals have attained thermal equilibrium with each other and the water, a thermometer on the water reads 25.0C. The specific heat of aluminum is 0.897 J/gC. The specific heat of lead is 0.129 J/gC. The specific heat of water is 4.184 J/gC.

1. Which metal had the higher initial temperature?

2. Which had the greater change in temperature as it cooled?

3. Which one lost more heat (q)?

4. How much energy did the water gain?

5. How much water was in the container?

Question

04-09-2022
Chemistry

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A 5.00-g piece of lead at 85.0C and a 20.00g piece of aluminum at 65.0C are placed into a container of cold 20.0C water. After the two metals have attained thermal equilibrium with each other and the water, a thermometer on the water reads 25.0C. The specific heat of aluminum is 0.897 J/gC. The specific heat of lead is 0.129 J/gC. The specific heat of water is 4.184 J/gC.

1. Which metal had the higher initial temperature?

2. Which had the greater change in temperature as it cooled?

3. Which one lost more heat (q)?

4. How much energy did the water gain?

5. How much water was in the container?

Sagot :

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