Q4. Your report must include clearly labelled plots you have used to make the determination of the reaction order. Compare R2 values SUMMARY OUTPUT TIME + 1/[NO2] MOL L-1Regression StatisticsMultiple RR SquareAdjusted R SquareStandard ErrorObservationsANOVARegressionResidualTotalInterceptX Variable 1Multiple RR SquareAdjusted R SquareStandard ErrorObservationsANOVARegressionResidualTotalRegression StatisticsInterceptX Variable 10.9990753570.9981515690.9977818834.640839396Multiple RR SquareAdjusted R SquaStandard ErrorObservationsdfANOVASUMMARY OUTPUT TIME + [NO2] MOL L-1RegressionResidualTotalInterceptX Variable 1Regression Statistics7df1алнCoefficients Standard Error104.38977870.759535261560.9161433170.8393185780.8071822930.001121943df7SUMMARY OUTPUT TIME+ IN[NO2] MOL L-1SS58150.89635107.686951558258.5833156CoefficientsStandard Error0.008223571 0.000764476-1.80595E-05 3.53379E-060.9775959630.9556938670.9468326410.10672171773.162199020.01461727156Coefficients-4.773149167-0.003490881TIME (seconds) [NO2] mol L -100.010.0063601200.005181800.004182400.0035SS3.28756E-056.29379E-063.91693E-05SSMSF ignificance F58150.89635 2699.997 4.99E-0821.5373903F ignificance FMS3.28756E-05 26.11747 0.0037371.25876E-06Standard Error1/[NO2] MOL L-10.0727185920.000336142400.001/[NO2] mol L-1100.00158.73193.05239.23285.71350.00300.00In[NO2] mol L-1-4.61-5.07-5.26-5.48-5.65250.00200.00150.00100.00t StatP-value Lower 95% Upper 95% ower 95.0%Jpper 95.0%33.01176745 4.79E-07 96.26109 112.5185 96.26109 112.518551.96149855 4.99E-08 0.72196 0.79711 0.72196 0.7971150.000.00[NO2] MOL L-10.0120.010.0080.0060.004MSignificance F1.228373867 1.228373867 107.8512 0.0001430.056947624 0.0113895251.2853214910.00200050t StatP-value Lower 95% Upper 95% ower 95.0%Jpper 95.0%10.75714034 0.00012 0.006258 0.010189 0.006258 0.010189-5.11052582 0.003737 -2.7E-05 -9E-06 -2.7E-05 -9E-06IN[NO2] MOL L-1500.00-1.00-2.00-3.001/[NO2] mol L-1100-4.00-5.00-6.00-7.000100●150150200TIME[NO2] mol L -150200TIME250100t StatP-value Lower 95% Upper 95% ower 95.0%Jpper 95.0%-65.63863525 1.55E-08 -4.96008 -4.58622 -4.96008 -4.58622-10.38514299 0.000143 -0.00435 -0.00263 -0.00435 -0.00263250300150300350In [NO2] mol L-1350200TIME400400250O300350400

When the plot of [NO2] versus time(s) graph is a perfect straight line, the reaction is Zero order…

Answered: Your report must include clearly…

Your report must include clearly labelled plots you have used to make the determination of the reaction order. Compare R2 values

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Ammonium ion reacts slowly with nitrite ion: NH4+ (aq) + NO2-(aq)-> N2(g) + 2H20 (1) Rate data for this reaction, measured at a certain temperature, are shown in the attached table. Use your rate law, and the rate and concentrations for any of the experiments, to calculate the rate constant (k) for the reaction in /Ms. Type your response: Expt. [NH4+] (M) [NO₂] (M) Rate (M s-1) 1 0.150 0.220 7.00 x 10-6 2 0.600 0.220 2.80 x 10-5 3 0.600 0.110 1.40 x 10-5
(2) The reaction-rate data given below were obtained using a batch reaction system for the reaction A→products. Plot the data in appropriate form to test the fit for zero- and first-order kinetics. From the plot that gives the best fit, determine the appropriate reaction rate constant (remember the units). Time, min CA, (g/m3) 0 30 0.5 25.4 1 21.6 2 16.9 4 13.1 8 8.3 16 3.2 32 0.31
Please explain how to find rate constant (k) if reaction rate = 3.40*10^-7 I^- molar = .00200 (reaction order 1) BrO3^- molar = .00800 (reaction order 1) H^+ molar = .0400 (reaction order 2)
The overall gas phase reaction 3A --> B + 2C occurs via the following sequence of elementary steps 2A <--> I1 + B k1,k2 A + I1 --> 2I2 k2 I2 --> C k3 1. write an expression for the overall reaction rate, r, in terms of the rate step 3, r3 2. using the answer from 1, obtain an expression for the reaction rate, r, in terms of rate constants and concentrations of reactants and products, only use PSSH. 3. State the. specific inequality the must be satisfied for each of the following assumptions to hold, and use it to simplify the general rate expression from question 2. i) Step 1 is quasi-equilibrium ii) Step 1 is irreversible
3. If the slope of the following plot is equal to 'p' (order of the reaction with respect to [1]), name the X and Y axis. -5.0 -4.8 4.5 4.2 y = 1.0404x+0.4902 = 0.9973 -4.0 -3.5 4.0 4.5 -5.0
Second-order rate constants used in modeling atmospheric chemistry are commonly reported in units of cm3 molecules'. Convert 3.5 x 1027 cm3 molecule1 s to L mol-1 sl. Round vour answer to 2 decimal nlaces.
Using the data and/or graph shown below, determine the rate of the reaction A-> products over the time period from t -80 s to ty s. Express your answer in decimal form in units of M/s, but do not add the units to your answer, just give the number. Concentration of A (moles/L) vs Time 0.900 1.000 0.900 10 0.621 0.800 20 0.474 0.700 30 0.383 0.600 40 0.321 0.500 50 0.277 0.400 60 0.243 0.300 70 0.217 0.200 80 0.196 0.100 90 0.178 0.000 0. 20 40 60 80 100 120 100 0.164 time(s)
- 1 -1 At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.154M S. 2N,O5 (g) → 2N,04 (g) +O2 (g) Suppose a vessel contains N,O, at a concentration of 0.500M. Calculate the concentration of N,O, in the vessel 95.0 seconds later. You may assume no other reaction is important. ol. Round your answer to 2 significant digits. Ar | M
- 1 At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0968 s 2N,O; (g) → 2N,04 (g) + O2 (g) Suppose a vessel contains N,0g at a concentration of 1.07M. Calculate the concentration of N,O, in the vessel 6.40 seconds later. '2 You may assume no other reaction is important. Round your answer to 2 significant digits.
For the reaction 2COG) + Ozl3) → 2002(3). Reaction Trial Initial conc. COM Initial conc. O2 M Initial Rate Ms1 1 0.0204 0.000138 0.204 0.0408 0.000138 0.102 0.0102 0.000069 0.051 Use these data to determine the orders of the reaction with respect to CO- [Select] O2- [ Select ]
Arrange the following compounds in order of increasing reaction rate with HNO3/H2SO4. 1. C6H5CH=O II. C6H5OCH3 III. C6H5Br IV. C6H5CH3 O I
Determine the reaction order for HCl using calculations described in the background section. Show your work. Note that your answer will probably not be a whole number as it is in the examples, so round to the nearest whole number.