Lab III - Exploring the Method of Initial Rates
Lab III - Exploring the Method of Initial Rates
Lab III - Exploring the Method of Initial Rates
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• The general rate law for <strong>the</strong> reaction• The concentrations <strong>of</strong> each reactant for each experiment• The rate <strong>of</strong> each experiment1. To begin, write down <strong>the</strong> general rate law for <strong>the</strong> reaction, recalling that <strong>the</strong> balancedchemical equation is:Rate Law:S 2 O 3 2− (aq) + 2H + (aq) → S(s) + SO 2 (g) + H 2 O(l)Based on <strong>the</strong> experiment, explain why we can effectively ignore <strong>the</strong> effects <strong>of</strong> HCl on<strong>the</strong> rate in this experiment.2. Determine <strong>the</strong> initial concentrations <strong>of</strong> thiosulfate and HCl in each well, showing twosample calculations and <strong>the</strong>n completing <strong>the</strong> appropriate values in <strong>the</strong> table below:WellNumber12345678<strong>of</strong>Concentration<strong>of</strong> HCl (M)Concentration<strong>of</strong> Thiosulfate(M)DropsThiosulfateAvg. ReactionTime (sec)“Rate”(1/s)Table 4: Concentration and Rate Calculations
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