1. Define:

a. Kinetic Energy:

Potential Energy:

Heat:

Law of conservation of energy:

System:

Surrounding:

b. Exothermic and Endothermic reaction in details with example.

2. Give unit of energy:

Define specific heat:

Calculate the heat released by 1.00 X 10^2 g.solution raise its temperature from 25.0C to 31.5 C. the specific heat of the solution is 1.00 cal/g.C

3. State first law of Thermodynamics:

State second law of thermodynamics:

Explain what is meant by enthalpy and Entropy, and free energy.

Give difference between spontaneous and non spontaneous reaction.

Predict whether a reaction with a -ve H and -ve S will be spontaneous, nonspontaneous, or temperature dependent.

4. State factors affect on reaction rate.

Define activation energy.

Draw energy level diagram for exothermic and endothermic reaction and label it.

Give value of     H for exothermic and endothermic reactions.

5. Define chemical equilibrium and equilibrium constant.

Write equilibrium constant expression for following reaction.

2H2(g)  +  S2 (g) _______  2H2S (g)

State Le Chatterley's principle.

Use this principle and describe changes for following reaction.

      C(s)  + 2H2O (g) ________  CH4 (g)  + O2 (g)  + 18 Kcal

a. C is added

b. H₂O is added

c. CH₄ is removed

d. Temperature is added

e. A catalyst is added.