Objective: To study the effect of reactant concentration on the rate of the reaction between sodium thiosulfate and hydrochloric acid and to determine the order of each reactant and the rate law for the reaction.
2 HCI(aq) + NaS2O3 (aq) --> S(s) + SO2 (aq) + H2O(l) + 2NaCL(aq)
(a) Calculate the initial and final concentrations as needed to complete tables 1 and 2.
(b) Calculate the average reaction time for each reaction by adding the times for the two trials and dividing by 2.
(c) Calculate the reaction rate by taking the inverse of the average reaction time.
(d) Write the rate law for the reaction.
Please see the attached file for full solutions.
Assume that each drop is 1 ml.
Trial 1 => Vtotal = 12 ml + 8 ml = 20 ml
nHCl = 12 ml * 1 M = 12 * 10-3 moles = 12 mmol
=> Final HCl => 12 mmol / 20 ml = 0.6 M
Trial 2 => Vtotal = 6 ml + 6 ml + 8 ml= 20 ml
nHCl = 6 ml * 1 M = 6 * 10-3 moles = 6 mmol
=> Final HCl => 6 mmol / 20 ml = ...
This solution provides a guide with completed trial data, calculations and answers for this type of lab report.
The Oxidation of Alcohol by Dichromate Ion
1) I'm given a spectrophotometer. How can I determine the rate law? I can only use the spectrophotometer to determine %T. How can I get from %T to concentration? What strategy do I have to use? Can you provide me a step by step strategy about how to get "from %T to concentration" and how to get "from concentration to rate law"?
3) I will need to compare the class data after lab (average and Std dev) with my own data. What is standard deviation? When I'm asked to compare AVERAGE and STD DEV, what exactly do I need to write? Can you give me an example?
4) What is the purpose of this experiment? Is it to determine the rate law?
5) What will be my source of error? What can I do to improve it?View Full Posting Details