An iodine-clock kinetics experiment was performed by varying the composition of reactant solutions and measuring the resulting rates of reaction.
1) How do Trials 2 and 3 in the table differ?
2) Of the proposed mechanisms, which would be supported by the results in the table?
(If possible please include an explanation/thought process)
Homework Answers
Trials 2 and 3 differ in two respects: 1. Trial 2 has twice as much I- as trial 3. 2.Trial 3 has twice as much S2O82- as trial 2.
MECHANISM DETERMINATION: According to the data given in the table, rate of reaction is halved when concentration of I- is halved (comparing trial 1 and 3). Also, the rate is halved when the concentration of S2O82- is halved (comparing trial 1 and 2). So, the rate is directly proportional to concentration of I- and S2O82- . Hence the rate equation becomes:
R= [I- ][S2O82- ]
Writing rate equations for all the mechanisms proposed and comparing it with the actual rate equation: Rate is always calculated from the slow step. Therefore, the rate equations are:
Mechanism 1: R = [I-]2. Therefore, this is incorrect.
Mechanism 2: R = [I- ] [S2O82-] Therefore, this is correct.
Mechanism 3: R = [S2O8·I]3-[I-]. Therefore, this is incorrect.
Mechanism 4: R = [I- ]2 [S2O82-]. Therefore, this is incorrect.
Answer: Mechanism 2
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An iodine-clock kinetics experiment was performed by varying the
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An iodine-clock kinetics experiment was performed by varying the composition of reactant solutions and measuring the resulting rates of reaction. Initial Rate Experiment 1 Initial Rate Experiment 2 Initial Rate Experiment 3 Test tube contents 10.0 mL 0.10 M NaI(aq) 10.0 mL 0.10 M Na2S2O8(aq) 5.0 mL 0.0050 M Na2S2O3(aq) 1.0 mL starch solution 10.0 mL 0.10 M NaI(aq) 5.0 mL 0.10 M Na2S2O8(aq) 5.0 mL 0.10 M Na2SO4(aq) 5.0 mL 0.0050 M Na2S2O3(aq) 1.0 mL starch solution 5.0 mL...
Chemical Kinetics Kit for AP Chemistry Student Guide d. Is it likely that this reaction occurs...
Chemical Kinetics Kit for AP Chemistry Student Guide d. Is it likely that this reaction occurs in one step? Explain. 2. A student would like to determine the orders of the reaction for an iodine clock reaction that occurs in three steps 3r(aq)+ H,O:(aq) + 2H'(aq )-,(aq) +2H 2O0) slow I(aq) + 25,0,(aq) 3r(aq) + S40(aq) 21, (aq) + starch-starch-I" complex + r(aq) fast fast Write the rate law for this reaction, using variables in place of the exponents a...
equations that may be useful are: 2I(-)+SO2O8(2-)->I2+2SO4(2-) and I2+2S2O3(2-)->2I(-)+S4O6(2-) THE IODINE CLOCK- REACTION KINETICS IN-LAB GUIDELINES...
equations that may be useful are:
2I(-)+SO2O8(2-)->I2+2SO4(2-)
and
I2+2S2O3(2-)->2I(-)+S4O6(2-)
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Student Name: Instructor Name: EXP #4: POST-LAB 1. A proposed mechanism for the iodine clock reaction is shown below: Iodine Clock Reaction Mechanism: 1 HSoS0+HIO2 ki-2.95 x 10-1M-'s-1 2-2.0 x 1010 AM-2s-1 ka 1.0 x 105 M-'s-1 ka-3.0 x 105 M-3s-1 HIO2+I +H+2HOI HIO2+ HOI IO +I + 2H+ IO I+2H HIO2 + HOI HOI+I+H I2+H20 ks 3.0 x 1012M-2s-1 I+ H20 HOI+ I +H ke -2.2s-1 I2+HSO+H20+21 +SO- +3H+ -1.0 x 100 M-1-1 where the values of k are...
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In this lab we will be expressing rate as a change in
concentration of reactants over time. In order to calculate this,
we need to know the initial concentrations of our reagents after
they are combined but before the reaction occurs. This is a
dilution process. Recall that the calculation for a dilution is
accomplished using the relationship M1V1 = M2V2.
If the [S2O3 2- ] is initially 2.49x10-4 M, and the reaction
takes 145 seconds for the solution to...
Please answer all, I rate, thank you. THE IODINE CLOCK- REACTION KINETICS EXPERIMENT 3 PRE-LABORATORY QUESTIONS...
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2. Determine the rate of reaction in trial 1,2,3
3. What are the experimental values for n and m?
Thank you so so much for your help.
Experiment: Reaction Kinetics Aim: To find the reaction orders and rate constants for the following reaction: 3 H2C2O4(aq) + 2 MnO4 (aq) --> 6 CO2+ 2 OH(aq) + 2 H2O + 2 MnO2s In other words to obtain m, n,...
Chemical Kinetics Kit for AP Chemistry Student Guide d. Is it likely that this reaction occurs in one step? Explain. 2. A student would like to determine the orders of the reaction for an iodine clock reaction that occurs in three steps 3r(aq)+ H,O:(aq) + 2H'(aq )-,(aq) +2H 2O0) slow I(aq) + 25,0,(aq) 3r(aq) + S40(aq) 21, (aq) + starch-starch-I" complex + r(aq) fast fast Write the rate law for this reaction, using variables in place of the exponents a...
equations that may be useful are:
2I(-)+SO2O8(2-)->I2+2SO4(2-)
and
I2+2S2O3(2-)->2I(-)+S4O6(2-)
THE IODINE CLOCK- REACTION KINETICS IN-LAB GUIDELINES (WEEK 1) This is a guide to suggest a format for you to prepare your laboratory notebook so that you can efficiently collect and record the data needed for each part of this experiment. Provide a space for observations. Record all original data directly into the laboratory notebook. Show all post-lab calculations in your laboratory notebook. If you did several trials of the same...
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In this lab we will be expressing rate as a change in
concentration of reactants over time. In order to calculate this,
we need to know the initial concentrations of our reagents after
they are combined but before the reaction occurs. This is a
dilution process. Recall that the calculation for a dilution is
accomplished using the relationship M1V1 = M2V2.
If the [S2O3 2- ] is initially 2.49x10-4 M, and the reaction
takes 145 seconds for the solution to...
Please answer all, I rate, thank you.
THE IODINE CLOCK- REACTION KINETICS EXPERIMENT 3 PRE-LABORATORY QUESTIONS (WEEK 1) Fully answer these questions in your laboratory notebook before coming to lab. Show all work for numerical calculations. 1. If the rate law for a reaction is Rate [A][B What is the overall order of the reaction? a. b. If the concentration of A is doubled and the concentration of B is tripled, how will this affect the rate of the reaction?...
answer the questions
Experiment 1084-04: lodine Clock Reaction Purpose Determine the rate law for an iodine clock reaction and study the influence of st on that reaction abruptly that it can be as startling as the sudden sound of an alarm clock, hence the clock reaction Background Information chemical equations can be written for chemical reactions, only some will proceed while others do not. Among the ones that do proceed some reactions occur as soon as reactants are mixed, while...
1. In this lab we will be expressing rate as a change in concentration of reactants over time. In order to we need to know the initial concentrations of our reagents after they are combined but before the reaction occurs. This is a dilution process. Recall that the calculation for a dilution is accomplished using the relationship MiV1 = M2V2. Complete the table below by calculating the concentrations of l'(aq) and Fe"(aq) in the initial reaction solutions. The stock solutions...
D18 Kinetics Review Sheets 8 H*(aq) + 4 Cl(aq) + MnO4 (aq) - 2 Cl(g) + Mn(aq) + 4H2O(l) 1. Cl2 (9) can be generated in the laboratory by reacting potassium permanganate with an acidified solution of sodium chloride. The net-ionic equation for the reaction is given above. a. A 25.00 mL sample of 0.250 M NaCl reacts completely with excess KMnO.(aq). The Cl(a) produced is dried and stored in a sealed container. At 22°C the pressure of the Cl2(g)...
1. Determine which reactant is limiting the rate of
reaction. Justify the answer.
2. Determine the rate of reaction in trial 1,2,3
3. What are the experimental values for n and m?
Thank you so so much for your help.
Experiment: Reaction Kinetics Aim: To find the reaction orders and rate constants for the following reaction: 3 H2C2O4(aq) + 2 MnO4 (aq) --> 6 CO2+ 2 OH(aq) + 2 H2O + 2 MnO2s In other words to obtain m, n,...
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