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5 Paragraph vol 0.200M Na2S208 mL vol starch mL vol 0.0100M vol 0.200M Na2S203, NH4S04 mL mL vol 0.200M Vol 0.200M KI, mL KNO3, mL Trial 1 2 3 4 5 25.00 25.00 25.00 12.50 6.25 0.00 0.00 0.00 12.50 18.75 5.00 5.00 5.00 5.00 5.00 25.00 12.50 6.25 25.00 25.00 0.00 12.50 18.75 0.00 0.00 10.00 10.00 10.00 10.00 10.00 Because the calculations require the molarity at the beginning of the reactions and each solution was diluted by all the other solutions, the molarity has to be updated. Initial M in the columns refers to the actual concentration at reaction time. Rate is calculated by dividing time into 1. Kl initial M total vol mL Na2S208 initial M Trial 1 2 3 65 65 65 65 65 0.0769 0.0769 0.0769 0.0385 0.0192 CAWN Time, s for indicator to change 33 55 133 76 138 0.0769 0.0385 0.0192 0.0760 0.0760 rate of reaction 1/time, si 0.03 0.02 0.008 0.01 0.007 5
6. (5 pts) The overall order for this reaction is 7. (5 pts) Write the rate equation for this reaction. 8. (10 pts) Calculate the rate constant, k, for the 5 experiments. Complete the following Table. Rate Constant for Kl-Na2S208 reaction, k Trial 1 2 3 4 5 average k value = Standard Deviation = % Relative Standard Deviation = Show all your work for Trial 3. 9. (5 pts) Now that the overall rate of the reaction is known, how would doubling the concentration of both iodide and persulfate ions affect the rate?