Potassium Iodide Reaction Lab
ID:
CHEM1010H – Report 3
(Be sure to state references for any cited value at the end of this report. Additionally, all report material must be in INK – pencil or white-out will render the work ineligible for mark appeal)
1. What observations and conclusions can you note about each of the three reactions that occurred in the test tubes where you combined potassium iodide, KI, and hydrogen peroxide, H2O2 (in part 1) of the experiment? (Give a detailed explanation of any observations that you made, i.e., what made the colour change, what reactions happened?)
ANSWER:
2. Use the information below to develop the necessary calculations for the rate of reaction from the solutions in part B of the experiment
• Calculate the initial molarity …show more content…
However, at the start of the reaction you must account for the fact that the total volume of each solution was 200 mL.
ANSWER:
• Calculate the initial molarity of the hydrogen peroxide in each of your solutions, once the solutions have been mixed.
Remember: The H2O2 stock solution concentration was known: , and you used a specific volume of the solution, . However, at the start of the reaction you must account for the fact that the total volume of each solution was 200 mL.
ANSWER:
• Calculate the number of moles of sodium thiosulfate, Na2S2O3, that was initially present in each solution.
Remember: The Na2S2O3 stock solution concentration was known: and you used a specific volume of the solution, . This information is used to determine the number of moles.
ANSWER:
• Balance the reaction that occurred in each of the solutions. Refer to Eq. 1, 3, and 4 in the laboratory instructions for the components that are involved.
ANSWER:
• Calculate the number of moles of hydrogen peroxide that has reacted: Note: You will need to use stoichiometry to determine this. …show more content…
i.e., the numbers of moles per litre of peroxide consumed divided by the number of seconds required to react completely.
ANSWER:
• Complete the table below – you can manually do the calculations to fill all of the cells, or it is possible to use a spreadsheet program to calculate the values. (RECOMMENDED) The process you have used above can be repeated to provide the values for each of the entries in the table.
ANSWER:
3. Use the following steps to calculate the values of a and b as described in the lab procedure (under the heading: The rate law and our process for obtaining a, b, and k.)
In the solutions A, B and C, the concentration of hydrogen peroxide used was the same. Therefore, these solutions are a suitable series for an examination of the dependence of the rate of reaction on the concentration of the iodide ion. Similarly, solutions C, D, and E have the same concentration of iodide ion. Therefore, those solutions can be used to examine the dependence of the rate of reaction on the concentration of hydrogen
CHEM1010H – Report 3
(Be sure to state references for any cited value at the end of this report. Additionally, all report material must be in INK – pencil or white-out will render the work ineligible for mark appeal)
1. What observations and conclusions can you note about each of the three reactions that occurred in the test tubes where you combined potassium iodide, KI, and hydrogen peroxide, H2O2 (in part 1) of the experiment? (Give a detailed explanation of any observations that you made, i.e., what made the colour change, what reactions happened?)
ANSWER:
2. Use the information below to develop the necessary calculations for the rate of reaction from the solutions in part B of the experiment
• Calculate the initial molarity …show more content…
However, at the start of the reaction you must account for the fact that the total volume of each solution was 200 mL.
ANSWER:
• Calculate the initial molarity of the hydrogen peroxide in each of your solutions, once the solutions have been mixed.
Remember: The H2O2 stock solution concentration was known: , and you used a specific volume of the solution, . However, at the start of the reaction you must account for the fact that the total volume of each solution was 200 mL.
ANSWER:
• Calculate the number of moles of sodium thiosulfate, Na2S2O3, that was initially present in each solution.
Remember: The Na2S2O3 stock solution concentration was known: and you used a specific volume of the solution, . This information is used to determine the number of moles.
ANSWER:
• Balance the reaction that occurred in each of the solutions. Refer to Eq. 1, 3, and 4 in the laboratory instructions for the components that are involved.
ANSWER:
• Calculate the number of moles of hydrogen peroxide that has reacted: Note: You will need to use stoichiometry to determine this. …show more content…
i.e., the numbers of moles per litre of peroxide consumed divided by the number of seconds required to react completely.
ANSWER:
• Complete the table below – you can manually do the calculations to fill all of the cells, or it is possible to use a spreadsheet program to calculate the values. (RECOMMENDED) The process you have used above can be repeated to provide the values for each of the entries in the table.
ANSWER:
3. Use the following steps to calculate the values of a and b as described in the lab procedure (under the heading: The rate law and our process for obtaining a, b, and k.)
In the solutions A, B and C, the concentration of hydrogen peroxide used was the same. Therefore, these solutions are a suitable series for an examination of the dependence of the rate of reaction on the concentration of the iodide ion. Similarly, solutions C, D, and E have the same concentration of iodide ion. Therefore, those solutions can be used to examine the dependence of the rate of reaction on the concentration of hydrogen