Spectrophotometric determination of the emperical formula

December 24, 2017 Law

The reaction rate or the oxidation-reduction between oxalic acid and potassium permanganate, Kinks is measured by recording the time elapsed for the purple color of the permanganate ion to disappear in the reaction. As the temperature increases, the rate constant also increases and the rate of reaction increases as well. Addition of a catalyst reduced the height of the energy barrier and thus increases the rate of reaction. When the temperature is increased by ICC ,the reaction Factor 1. 55*AAA-2 which is calculated by using the value o the activation energy and changes in temperature Introduction

Kinetic analyses are often performed in order to refine our understanding of what happens on the molecular level during a chemical reaction. The main use of chemical kinetics is to measure the speed of a chemical reaction. But more importantly, in measuring the speed of a reaction. Rate law is a relationship between concentrations and rate. The reaction rate or the oxidation-reduction between oxalic acid and purple color of the permanganate ion to disappear in the reaction. The rate of discharge of the purple color of permanganate can thus be used as a measure o the rate of the reaction.

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The over-all reaction between permanganate and oxalic acid is expressed: Amman- (as) +CHIC (as)+OH+ mummer+ (as)+CACHE When a solution of permanganate ion is added to one of monogamous ion in which acid and oxalate ion are also present, a cherry-red solution of a complex ion formed from managing ion and oxalate ion results, whereas in the absence of oxalate ion or other anion capable of forming a complex, a precipitate of manganese dioxide is obtained Experimental procedure Preparation of the solutions 1 ml of potassium permanganate and ml of sulfuric acid were pipettes into mm test tube. L o oxalic acid was pipettes into the second test-tube Record the time for the reaction at room temperature(ICC) Oxalic solution was then poured into the potassium permanganate solution. The time taken for the purple color of the permanganate ion to disappear was recorded. Room temperature was recorded using all certain digits. Record the time or the reaction at higher temperature The second pair o the test tube were placed in a warm water bath at 40, 50 and 60 degrees Celsius until the equilibrium is established.

Discussions The concentration of oxalate ion is inversely proportional to the concentration of hydrogen ion, since oxalic acid is weak. The experiment show that acid is without influence on the rate if the concentration of oxalate ion is fixed. The effect of temperature: Rate is proportional to concentration/Time. If the time decreases by a factor of 3 (say), the rate correspondingly increases by a factor of 3. Addition of a few crystals of Mains greatly accelerates the reduction by oxalic acid of purple permanganate to the nearly colorless manganese(al).

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