Metallic cations have a pronounced catalytic effect on the rate of this reaction. Observe this effect by repeating React

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Metallic Cations Have A Pronounced Catalytic Effect On The Rate Of This Reaction Observe This Effect By Repeating React 1 (48.57 KiB) Viewed 60 times

Metallic Cations Have A Pronounced Catalytic Effect On The Rate Of This Reaction Observe This Effect By Repeating React 2 (39.01 KiB) Viewed 60 times

Metallic Cations Have A Pronounced Catalytic Effect On The Rate Of This Reaction Observe This Effect By Repeating React 3 (37.82 KiB) Viewed 60 times

Metallic Cations Have A Pronounced Catalytic Effect On The Rate Of This Reaction Observe This Effect By Repeating React 4 (47.41 KiB) Viewed 60 times

Metallic cations have a pronounced catalytic effect on the rate of this reaction. Observe this effect by repeating Reaction A (don't forget the 0.50 mL 0.050 M Na2S2O3 and the 0.50 mL of starch solution) with a catalyst at room temperature. Before mixing the three solutions, add one drop of 0.100 M CuSO4 reaction tube II. Swirl the flask for a minute to mix the catalyst thoroughly before adding the contents of tube I. Then mix the solutions, and when the color change occurs, record the time and average temperature. We will call this Reaction D. Dependence of Reaction Rate on Temperature In this part of the experiment the reaction will be carried out at several different temperatures, but with the same concentrations of all reactants at each temperature. The Table indicates the reaction conditions. Table of Reaction Mixtures at Different Temperatures Reaction Temperatures Reaction Mixture A Around 20°C as in Reaction 1 E Around 40°C as in Reaction 1 F Around 10°C as in Reaction 1

DATA AND CONCLUSIONS 1. Orders of the Reaction. Rate Constant Determination. I. Determine the initial molarities of I and S2O² for each reaction tube and write in the table below. Show calculations for I in reactions A and B and for S₂Os in reactions A and C. Initial in reaction A: Initial in reaction B: Initial [S:Os] in reaction A: Initial [S2Os] in reaction C:

II. Determine A Time for color to appear At(s) Reaction And T°C A B C D E Initial concentrations in reaction tubes (M) [S208²] (M) Moles/liter of I that reacted A (M) Relative rate of reaction A[I-]/At (M/s)

Consider the relative rates of the various reactions A to C. The changes in the rates resulted only from differences in and in [S208 2] in different solutions. Equation (2) on page 5 can be written in the form: Relative rate=k[S₂0, ²] (3) where k is a relative rate constant. Our purpose is to find n and m in (3), above. These are the orders ofthe reaction with respect to I and S2Os respectively. Reactions A to C must all obey equation (3), with the same value of k, since they were all carried out atthe same temperature and have relative rates that were calculated on the same basis. One way of doingthis is by substituting the experimental values for Reactions A and B into Equation (3): Relative rate A = k[][]"Relative rate B=_ KLF LF