Need help with a,b,c,d, and e 4. Plotting Concentration versus time for Trial #1 to determine reaction order of Red Dye #3order with respect to [OCI].b. The reaction isThe total reaction order isc.d. The value of k ise. The overall rate equation isFlon Excel add additional columns to your time and absorbance data for Trial 1Set up an equation using Beer's Law (A=abc) to calculate [Red Dye #3] at each timepoint.Set up an equation to calculate Ln([Red Dye #3]) at each time point.Set up an equation to calculate 1/[Red Dye #3] at each time point.Time (sec)Absorbance[Red Dye #3]Ln([Red Dye #3]).1/[Red Dye #3]b. Make three graphs and determine the curve fit for each graph. Submit all three graphsfor grading.1) [Red Dye #3] vs Time2) Ln([Red Dye #3]) vs Time3) 1/[Red Dye #3] vs Timec. Based on the curve fit of each of the three graphs, what is the reaction order of Red Dye# 3? Explain your answer.11 ben b iovoid bind Chemicahdiam (red dye 3)TescopCalculate the concentration of Red Dye #3 and hypochlorite (OCF) in each trial. Show2. Determine the concentration of each substance and the rate of the reaction and fill-in theSpectroAvoid brathing vaB. Kineticse Documents, Ete of thee reacti1. Concentration of hypochlorite [OCF] in bleach from bottleM0.805chart.eCR ed La.all calculations below the chart.b. Determine the rate of the reaction from the slope of the straight portion of ueabsorbance vs. time graph for each trial.Vol. ofTrial#Vol. ofVol. ofSoln 3Water[Red Dye #3][OCF]RateBleach12 mL3 mL * 1 mL-니3.26x10-66:51x10-62 mL 326x10-60.2680-1343.3x 104 mL1 mL1 mLO.1340.001532 mL6.67X10-42 mL41 mL3 mL 3.26x10-0.4032 mL0.0022.0 ml o 9.77X 100 =3.26x10-6 [Red dy#3]Trial #1 Calculations:61.0x 0.805 = 0.134 OCI]1.OX 0-8050,134COCI2.0x 0.80S e0.26&Trial #2 Calculations:4.0mL o 9.77x!0-6=6.51 x 10-6CRed dye#3コTrial #3: Calculations:= 3.26x10-6(Red dye #3]2. OML9.77x 10-6.Trial #4 Calculations:3.0x0.80S2.0mL•9.77X10-6=3.26x10-6[Red dye #3]%3D3. Determine the rate equation using the data from the chart above. Show calculations in the 0.463space provided.6a. The reaction is Second order with respect to [Red Dye #3].10Rate= K. Am B

We are given all the experimental data, we have to find the order of the reaction with respect to…

Answered: order with respect to [OCI]. b. The…

order with respect to [OCI]. b. The reaction is c. The total reaction order is d. The value ofk is e. The overall rate equation is

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

See similar textbooks

Similar questions

Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3
Go to the PhET Reactions and change to Angled shot to see the difference. (a) What happens when the angle of the collision is changed? (b) Explain how this is relevant to rate of reaction.
Use the data provided in a graphical method to determine the order and rate constant of the following reaction: 2PQ+W Time (s) 9.0 13.0 18.0 22.0 25.0 [P] (M) 1.077103 1.068103 1.055103 1.046103 1.039103
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
Assume the reaction: CH3CH=CHCOONa + H2 + Ni ----> ??? a. Determine the correct rate law expression based on the elementary reaction. b. Draw the structure of the transition state. c. Draw the reaction coordinate diagrams for: the reaction with the catalyst and the reaction without the catalyst, but adjacent graphs. (Assume that the reaction is exothermic and has 1 transition state.) d. Does heat increase the rate of the forward reaction in the given? Why or why not?
Clearly label the energy diagram below when answering each part. If there is more than one specific type of label, give an appropriate number afterwards (i.e. Int. 1, Int. 2, etc). State how many step(s) are in the overall reaction, if more than one, clearly label where they start and end Identify the rate determining step (rds) Label all transition state(s) (TS) Label all intermediate(s) (Int.) Label all activation energy(ies) (Ea) Label the heat of the reaction (ΔH) State whether the overall reaction is endothermic or exothermic. please explaing each step. Thank you.
A certain first order reaction has k = 0.706 s-1 . What fraction of the reactant remains after 0.100 s. (Give you answer to 3 sig figs)
Final Reactant Concentrations and Reaction Rates [I-] [BrO3-] [H+] Reaction Time Rate of Reaction 2.8 x 10-5/time Expt. # M M M sec. M/sec 1 0.00166 0.0066 0.0166 258 2 0.0033 0.0666 0.0166 135 3 0.00166 0.0133 0.0166 132 4 0.00166 0.0066 0.033 78 FIND THE RATE?
A first order reaction takes 69.3 min for 50% completion. Set up on equationfor determining the time needed for 80% completion.
A reaction is found to undergo a multi step mechanism, with the steps outlined below step 1 E+D --------2C+B step 2 B+2D-----C+E -the intermediate reaction is : ?.The catalysts in this reaction is :?. The overall reaction is :?---------?.
Deducing a rate law from initial reaction rate data #1