out. When the data’s done being collected, remove the stopper and dump the products in an inorganic waste jar. On the graph, tap and hold where the curve begins to increase, slide the stylus across the graph until it starts to plateau again, click the Analyze menu and choose ‘Curve Fit’ and select ‘Linear’. Record the slope as the initial rate of reaction and hit OK, then hit the cabinet button, on the right and clean everything use in the first test. Repeat the paragraph above for the rest of the tests except… For Test #2: add 1 mL of distilled water to the 1 mL of KI, in the Beral pipette. For Test #3: use the original 1 mL of KI (no added distilled water) and dilute 2 mL of hydrogen peroxide with 2 mL of distilled, deionized water. For Test #4: put the beaker of water on a hot plate and get the water to somewhere between 40 and 45 degrees Celsius, remove the beaker from the hot plate as soon as the
reaction begins. Rate Law Expression : Rate=k[H 2 O 2 ][ I - ] Activation Energy : E a =.020 kJ/mol Discussion : The rate determining step for this experiment was the first step, H 2 O 2 + I - → IO - + H 2 O, we know this because the coefficients of the reactants correspond with their respective orders. Hydrogen peroxide and iodine are first order for the rate law expression, which was determined in the experiment. This determined rate law does match the rate proposed and have
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- Summer '10
- Chemical reaction, ml