Experiment No. Two

Exp.2 The effect of change Temperature on the Rate of Reaction and calculating the Activation Energy.
Theory:
The rate of the chemical reaction is directly proportional to the temperature and hence the chemical reactions going more quickly at high temperatures than in low temperatures based on the law of Van t Hoff s rule the velocity of chemical reactions is increased twice or more for each rise of 10°C in temperature.
Activation energy defined as the minimum energy required to start a chemical reaction. The activation energy of a reaction is usually denoted by Ea and given in units of kilojoules per mole.
When a reaction occurs at temperature, T, the variation of the rate constant, K, can be usually expressed by the Arrhenius equation:
K= A? e?^(?-E?_a/RT)
The amount of energy required is represented by the symbol, Ea and A is constant. By obtaining the logarithms for both sides of the equation, the equation becomes:
logK=logA-E_a/2.303RT


Chemicals and tools:
Hydrochloric acid (HCl).
Distill water.
Ethyl acetate? (CH?_3 ?COO?CH?_2 CH?_3).
Sodium hydroxide NaOH.
ph.ph indicator.
Conical flask.
Water bath.

Procedure:
Put in six conical flask 5 ml from distilled water in ice water bath.
Put in another conical flask 50 ml of 0.1N HCl and add to it 5 ml ethyl acetate and record time.
Take 5 ml from mixture and add it to one of conical flask contain on distilled water only and heated at 35C0 and titrate with 0.1 M NaOH by using ph.ph as indicator to calculate (V0).
After 5 min from mixing process take 5 ml from mixture and add it to one of conical flask that contain on distilled water only and heated at 35C0 and titrate with NaOH by using ph.ph as indicator.
Repeat step 4 after 10, 15, 20, and 25 min to calculate V1, V2, V3, and