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11 Nov 2019

You are doing Kinetics experiment and this is the eqaution for the reaction.

A ----> 2B

You added 0.100M of A in the beaker and observed the concentration of B over time at 25'C.

You have your data on three graphs.

1. What is the rate equation for the reaction?

2. What is the rate constant for the reaction?

3. If you want this reaction to have a concentration of A corresponds to 0.00100 M, how long do you have to wait?

4. Another student is doing the same reaction experiment. He started the reaction with 0.200M of A and it took 22.5 minutes for the concentration of A to reach 0.100M. Do you think you this student ran his reaction at the same temperature as you did?

Change in In[S] Over Time y=-0.0231x-2.3024 Change in Concentration ofS Over Tim e 0.1000 (2.000) 0.0800 (2.500) 2 0.0600 (3,000) 0.0400 (3.500) 0.0200 (4.000) 2 9 2 2 2 Time (min) Time (m in) Change in 1/[S] Over Tim

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Lelia LubowitzLv2

7 Feb 2019

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Related questions

A student studies the kinetics of reaction 1 below using a clock reaction technique, reaction 2, and the procedures given in this experiment. For reaction mixture 1, he measures a time to color change of 121 seconds and for reaction mixture 2, he measures a time of 58 seconds. The temperatures of the reaction mixtures were the same for both experiments.

6Iâ (aq)+ BrO3â (aq) + 6H+(aq) --> 3I2 (aq) + Brâ (aq) + 3H2O(l) (Reaction1,slow)

I2 (aq) + 2 S2O32â (aq) --> 2 Iâ (aq) + S4O62â (aq) (Reaction 2, fast)

a. Determine the change in concentration of S2O32â that occurred during the time period measured. This should be the same for both the reaction mixtures. First, use M1V1=M2V2 to determine the initial concentration of the S2O32â after mixing the contents of the two flasks but before the reaction begins. Next, find the final concentration of S2O32â by remembering that all the S2O32â is consumed when the color change occurs. You can then find the change in the concentration of S2O32â.

[S2O32â]0 =

â[S2O32â] =

b. Use the stoichiometry of Reactions 1 and 2 to determine the change in concentration of BrO3â during

the same time period. â[BrO3â] =

c. Calculate the initial rate for each reaction mixture. Recall that Rate = â â[BrOâ ] / ât

Rate for mixture 1:

Rate for mixture 2:

d. Method of Initial Rates

Complete the table below using M1V1=M2V2 to find the initial concentration of each reactant after mixing the contents of flasks I and II for both reaction mixtures. Enter the initial rates computed above.

Rxn Mixture [Iâ]0(M) [BrO3â]0(M) [H+]0 (M) Rate (M/s)

Use the method of initial rates and the relevant data above to determine the order of reaction 1 with respect to the concentration of iodide ions.

Order with respect to [Iâ]:_________________________

e. It is critical for the success of this experiment that the concentrations of the reactants Iâ, BrO3â, and H+ do not change significantly over the time period measured.

Why is this important?

f. By what percent did the bromate ion concentration change during the time period considered for mixture 1 in this experiment?

PercentChange = (|â[BrO3â ]| / [BrO3â ]0 ) x 100%

Please help me understand this!

Suppose the concentration of the receptor in the stock solution dropped to 50.0 uM. If you ran the experiment again with the same initial concentration of free modified insulin as above, what would you expect the free modified insulinâs equilibrium concentration to be? (10 pts)

	[free modified insulin]	[receptor]	[Insulin-receptor]
I
C
E

4. The equilibrium results on your modified insulin look promising, but it seems like it took forever for the reaction to reach equilibrium. Your supervisor now wants you to study the reaction rate for the binding of your modified insulin to the cell receptor. Show all work.

A. Using the chemical equation from Question 3 write the mathematical relationship between the rate of disappearance of free insulin and the rate of appearance of the insulin-receptor complex. (10 pts)

B. As mentioned above, you devised a method for measuring the concentration of free insulin in solution. You are able to get an estimate of the initial rate of reaction by adding a known concentration of insulin, [I]_o,to a known concentration of receptor, [R_o] and then taking a measurement of the free insulin, [I_t], 60 seconds after mixing. From the data in Table 3 calculate the initial rate for each experiment in uM/s. Show all work. (10 pts)

Table 3: Initial rate data for insulin/receptor binding. [I_t] measured after 60 seconds.

	[I_o]	[R_o]	[I_t]	Initial Rate (uM/s)
Experiment 1	100 uM	70.0 uM	95.0 uM
Experiment 2	100 uM	35.0 uM	95.0 uM
Experiment 3	50.0 uM	70.0 uM	47.5 uM

C. How does the initial rate of reaction change with changing insulin concentration? How does it change with changing receptor concentration? (5 pts)

D. Write the rate law for this reaction with its correct reaction orders and calculate the rate constant. Show your calculation. (10 pts)

E. If modified insulin has a higher equilibrium constant than normal insulin does that mean the modified insulin will have a higher reaction rate than normal insulin? Explain your answer. (5 pts)

Hi, i completed a kinetic experiment

That involves adding 20ml of persulfate and 10 ml Iodine with 10ml thiosulfate ... A reaction ( Rxn) occurs in the 50 ml mixture and all the thiosulfate was consumed in a given time ( 97sec) indicated by the starch turning blue ...

The lab instructions asks me to calculate the reaction rate ( initial rate) but i have trouble understanding what the instruction is asking me to do .. Can someone show me ( visually) how to perform this reaction rate calculation ?

Thank You