Measurement of the decrease in the concentration of a hydrogen peroxide solution as it is catalytically decomposing | CHEM 1046, Lab Reports of Chemistry

Download Measurement of the decrease in the concentration of a hydrogen peroxide solution as it is catalytically decomposing | CHEM 1046 and more Lab Reports Chemistry in PDF only on Docsity! Chemical Reaction Rate Objective: The Objective of this experiment was to measure the decrease in the concentration of a hydrogen peroxide solution as it is catalytically decomposing. Another objective of this lab was to graph the results and then from the graph deduce the first order rate constant and the half-life of the decomposition rate. Experimental Data: Time (min) Volume KMnO4 (mL) 1 6.00 6 6.22 11 5.70 16 5.22 21 4.56 31 4.14 41 3.94 51 3.61 61 3.00 Molarity of KMnO4= 0.063 Sample Calculations: Moles of KMnO4 used: = (MKMnO4)(VKMnO4) = (0.063M)(0.0060L) =3.8 x 10^-4 Moles of H2O2 = (mol # KMnO4)(5 mol H2O2)/(2mol KMnO4) = (.00038 mol)(5 mol H2O2)/(2 mol KMnO4) =9.5 x 10^-4 [H2O2]t = (mol # H2O2)/(V) = (.00095)/(.01L) =0.095M Ln[H2O2]0 (from graph) = -2.16 [H2O2]t = e^(ln[H2O2]t) = e^(-2.16) = 0.115 t1/2 =ln([H2O2]0/2)corresponding x-axis value on graph =ln(.0993/2) = -3.85  70 minutes