HW #14 for 4/18

1.) A process is exothermic if:
A.) Energy flows into the system
B.) Energy flows out of the system
C.) The energy level remains constant
D.) The temperature of the system increases

2.) How many CALORIES of heat must be added to 3.0 x 102 g of water in order to raise its temperature by 40.0 degrees C? (Hint: first find Joules and then convert to calories)

3.) If the same quantity of heat is supplies to 100 g of each of the following substances, which substance will increase the most in temperature? (look at table on pg. 329): Water, iron, gold, ice, or carbon

4.) When 100 g of ice melts to form 100 g of water, the process is exothermic or endothermic? Explain why.

5.) Knowing that 1 calorie = 4.184 Joules, how many calories of energy are reguired to raise the temperature of 10.0 g of water by 1 degree Celsius?

6.) Which change results in a release of energy?
A. The melting of water
B. The boiling of water
C. The evaporation of water
D. The condensation of water

7.) Compare the amount of energy and molecules in 1 mole of water at 0 degrees Celsius and 1 mole of water at 23 degrees Celsius.
A. The amount of energy is the same and the number of molecules is the same in both
B. The amount of energy is the same, but the number of molecules is greater at 23 degrees Celsius
C. The amount of energy is greater at 23 degrees and the number of molecules is greater
D. The amount of energy is greater at 23 degrees and the number of molecules is the same