 # Rate Of Reaction Lab Report

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AIM:
The experiment is to investigate the effect of the change in the concentration of Hydrogen peroxide and sodium thiosulphate on the rate of reaction between potassium iodide (KI), hydrogen peroxide, Sodium thiosulfate (Na2S2O4) under acidic condition.

Introduction:
The rate of reaction can be defined as the rate at which the reactants are consumed of the rate at which product is formed.
It is the ratio of the concertation of reactant used of concentration product to time, it measured in mol.dm-3.S-1.
This can be expressed as Rate of reaction = - (∆[reactant])/∆time = (∆[product])/∆time
This implies that the rate of reaction is directly proportional to the concentration of reactant/product but inversely proportional to the
THEORY OF THE EXPERIMENT
In this experiment change in the volume of reagents by diluting with water is used as change in the concentration and reciprocal of the time taken for the appearance of blue black colour as the reaction rate.

Equation of reaction
H2O2 (aq) + 2H+ (aq) +2I- (aq) I2 + 2H2O

Hypothesis
Hypothesis 1: Decrease in concentration of hydrogen peroxide (H2O2) decreases the rate of reaction (that is, increases the time for reaction to come to completion). In the reaction between potassium iodide (KI), hydrogen peroxide, Sodium thiosulfate (Na2S2O4) under acidic condition.

Hypothesis 2: Decrease in the concentration of potassium iodide decreases the rate of reaction (that is increases the time for the reaction to come to completion). In the reaction between potassium iodide (KI), hydrogen peroxide, sodium thiosulfate (Na2S2O3) under acidic condition.

Apparatus:
The apparatus used in this experiment are as follow: 50cm3 measuring cylinder 25cm3 measuring cylinder 100cm3 beaker White