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Question: FIRST ORDER REACTION: DECOMPOSITION OF HYDROGEN PEROXIDE EXPERIMENT WAS PERFORMEND. 100 ML 1 M OF PEROXIDE solution WAS MIXED WITH 10 ML of 1% Kl solution WITH ACTED AS A CATALYST.The progress of the reaction is now followed by titrating 10 cm3 samples at approximately 10 minutes intervals. When about 9 minutes have elapsed, a 10 cm3 sample of the reaction mixture WAS TRANSFERED by means of the 10 cm3 measuring cylinder into the 54 Erlenmeyer, 5 cm3 of dilute sulfuric acid ADDED, and titrated rapidly with permanganate. the exact time at which the first drop of the permanganate is added was recorded. In as much as the peroxide continues to decompose until all of it has reacted with permanganate, the titration should be continued as rapidly as possible. the volume of permanganate required was recorded. Titrated successively 10 cm3 samples of the reaction mixture at approximately 10 minutes interval until 8 samples have been analyzed. from the analysis peroxide concetration decreased form 1 M to 0.564 M . velocity constant was found to be 7.63×10^(-3) form the slope of the graph and 9.09×10^(-3) from calculations. half life was found to be at 76.26 minutes .abstract with 4 sentences
The experiment involved the decomposition of hydrogen peroxide, monitored by titrating samples every 10 minutes. Potassium iodide was used as a catalyst, and the reaction progress was observed through titrations with permanganate. The speed of the reaction was recorded, showcasing a decrease in peroxide concentration from 1M to 0.564M and resulting in velocity constants of 7.63x10^(-3) from graph analysis and 9.09x10^(-3) by calculations. Ultimately, a half-life of 76.26 minutes was determined for the reaction.
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