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Calculate the molar concentration of FeSCN2+ in solution #3. The determined molar absorptivity of the solution at 448 nm is 333 L mol-1 cm-1.
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- List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.2. Consider the kinetic data of the reaction of P + 2 Q + 2+ - PQ, + Z*and answer the succeeding questions: Experiment P (M) Q (M) Temp ("C) Initial Rate, M/s 1 0.01150 0.01200 0.00000 25 4.80 x 10-4 2 0.02300 0.01200 0.00000 25 1.92 x 10-3 3 0.01150 0.02400 0.00000 25 9.60 x 10-4 4 0.04600 0.01200 0.00000 25 7.68 x 10-3 5 0.01150 0.04800 0.00000 25 1.92 x 10-3 6 0.01150 0.01200 0.00000 10 5.10 x 10-5 0.01150 0.01200 0.00000 40 4.55 x 10-3 0.01150 0.01200 0.00500 10 4.98 x 10-5 0.01150 0.01200 0.01050 25 4.82 x 104 10 0.01150 0.01200 0.02100 40 4.44 x 10-3 A. Determine the rate order with respect to P. Determine the rate order with respect to Q. C. Determine the rate law of the reaction. What is the average rate constant? Indicate the appropriate units. E. What is the energy of activation and frequency factor of the reaction without the additive ion? Include the equation of the best fit line of the Arrhenius equation and RSQ Note: Use the calculated rate constant in set up 1 for 25°C…DETERMINATION OF A,H FOR THE REACTION OF Mg AND HCl Minimize D The results from one run are shown below. 40 00003333333t1&C66C0000000000333333113ttteeccc000000 y = -0.51215 x + 40.274 20 10 4 5 Time (min) Q3 Use the graph to determine Tinitial and Tfinal. You must then use these values to calculate the change in temperature for the reaction. Tinitial (°C) Tinal (°C) AT (°C) 1 2 Temperature (°C) 30
- Ne(g) effuses at a rate that is ______ times that of Kr(g) under the same conditions. rateNe/rateKr=if the rate at which O2 appears change [O2]/change t=6.0 x 10-5 Mol s-1 at a partivular instant at what rate is O3, disappearing at the same time - change[O3 ]/change in timeReaction Conc, Na,d O3| Cune. HCI 4Als. | AIme (3) Rabe I1.3085840 0.10M •30M 0.4563/64 |0.028 F0913 15 M 12267196 | 0,01870913 30M 1.5360817 0.300349 2 65.56796607 5. 11431671 O.10 M 3 0.050 M 4 0.025 M 0:30M 1.54866|1 1.007568 1,358380874 4. Use experimental data and the rate law to calculate a rate constant for each reaction 1, 2, 3, 4. How do the rate constants compare? Should they be the same or different? Discuss in your conclusions. Report the average value of your calculations. Be sure to include units in your rate constant. -1-4 -2:5 Rate= k [ Naz s03] [Hc1]
- Reaction Conc. Na2S203 Conc. HCI A Abs. A Time (s) Rate (A Abs./BA Time) 1.3686611 1.5360817 1.2267196 1.007568 |0.300349 |0.01870913 |0.02870913 1 0.10 M .30 М 1.358380874 2 0.10 M .15 M 5.114311671 3 0.050 M .30 M 65.56796601 4 0.025 M .30 M 0.9563164 11.3085840 3. What is the overall order of the reaction? Write the complete rate law for this reaction.(ii) At elevated temperatures, nitrogen dioxide decomposes to nitric oxide and molecular oxygen: 2NO2(g) – → 2NO(g) + O2(g) The change in concentration of NO2 with time at 300 °C is given below: t (s) 100 200 300 400 500 [NO2]/103 (mol dm-3) 8.0 5.6 4.3 3.5 2.9 2.5 By appropriate plotting of the data and use of this graph: (a) verify that this reaction is second order with respect to NO2; (b) determine the rate constant for this reaction.Reaction Conc. Na2S2O3 Conc. HCI A Abs. A Time (s) Rate (Δ Abs./jΔ Time) 1 0.10 M .30 М 1.3686611 1.007568 1.358380874 0.300349 |0.01870913 0.10 M .15 M 1.5360817 5.114311671 3 0.050 M .30 M 1.2267196 65.56796601 4 0.025 M .30 М 0.9563164 0.02870913 11.3085840 POSTLAB QUESTIONS 1. Compare the rates of reactions 1, 3 and 4. What is the effect on the reaction rate of halving the thiosulfate concentration? What is the order of the reaction in sodium thiosulfate?
- times that of Kr(g) under the same conditions. CO(g) effuses at a rate that is rate co ratekr * TOOLS x10In a study of the conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °CCH3NC(g)CH3CN(g)the concentration of CH3NC was followed as a function of time.It was found that a graph of ln[CH3NC] versus time in seconds gave a straight line with a slope of -4.38×10-3 s-1 and a y-intercept of -2.83 . Based on this plot, the reaction is ______ order in CH3NC and the half life for the reaction is _______ seconds.Reaction Conc. Na2S½O3 Conc. HCI A Abs. A Time (s) Rate (A Abs./ga Time) 1.007568 0.300349 0.01870913 0.02870913 1 0.10 M .30 М 1.3686611 1.358380874 0.10 M .15 M 1.5360817 5.114311671 3 0.050 M .30 M 1.2267196 65.56796601 4 0.025 M .30 M 0.9563164 11.3085840 4. Use experimental data and the rate law to calculate a rate constant for each reaction 1, 2, 3, 4. How do the rate constants compare? Should they be the same or different? Discuss in your conclusions. Report the average value of your calculations. Be sure to include units in your rate constant. The rate law of the reaction is shown below: Rate = [Na2S2O3]-2