pls complete the table [S208 2-], M[H), M[S203 2-], MReaction time,s Rate, M/sRuns0.08000 8.0*10-40.04000 8.0*10-40.02000 8.0*10-40.04000 8.0*10-40.04000 8.0*10-410.0200049.108.147*10-62a0.02000106.103.770*10-60.02000197.442.026*10-669.2053.055.780*10-67.540*10-640.030000.04000 RunsTemperature, °C Temperature, K [S208 2-], M[-), MReaction time,s Rate, M/sRate constant2a2b2c2dRT302.15000106.1058331.1500015.500.020000.0400019292.15000231.04RT302.1500066.35RunsIn k1/T2a2b2cSlopeInterceptr2 valueEa (kJ/mol)ARunsReaction time,s2a2dConclusion(Faster, slower,no effect)Jcolo H

With, an increase in reaction time, the rate constant decrease. Retention time= 1/ rate constant.…

Answered: Runs 2a 2b 2c Slope Intercept r2 value…

Runs 2a 2b 2c Slope Intercept r2 value Ea (kJ/mol) A Runs 2a 2d Conclusion (Faster, slower, no effect) In k Reaction time,s 1/T

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.1: Reaction Rate

Problem 11.2CE: Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of...

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Time (sec) PH [RX] [H30+] Ln[RX] 0.000 7.000 0.00002344 0.0000001 -10.6610666 15.000 6.400 0.00001954 0.00000039 -10.8430469 30.000 5.410 0.00001955 0.00000389 -10.8425353 45.000 5.230 0.00001756 0.00000588 -10.94988696 60.000 5.070 0.00001493 0.00000851 -11.11213794 75.000 4.920 0.00001142 0.00001202 -11.3801444 90.000 4.840 0.00000899 0.00001445 -11.6193977 105.000 | 4.780 0.00000685 0.00001659 -11.8912619 120.000 4.750 0.00000566 0.00001778 -12.08208666 135.000 4.720 0.00000439 0.00001905 -12.33618133 150.000 4.700 0.00000349 0.00001995 -12.56569882 165.000 4.670 0.00000207 0.00002137 -13.08796195 180.000 4.670 0.00000207 0.00002137 -13.08796195 195.000 4.660 0.00000157 0.00002187 -13.3644349 210.000 4.650 0.00000061 0.00002283 -14.30980687 225.000 4.650 0.00000061 0.00002283 -14.30980687 240.000 4.640 0.00000061 0.0000229 -14.30980687 255.000 4.640 0.00000061 0.0000229 -14.30980687 270.000 4.640 0.00000061 0.0000229 -14.30980687 285.000 4.630 0.00002344 Undefined 300.000 4.630…
Time (sec) pH [RX] [H30+] Ln[RX] 0.000 7.000 0.00002344 0.0000001 -10.6610666 15.000 6.400 0.00001954 0.00000039 -10.8430469 30.000 5.410 0.00001955 0.00000389 -10.8425353 45.000 5.230 0.00001756 0.00000588 -10.94988696 60.000 5.070 0.00001493 0.00000851 -11.11213794 75.000 4.920 0.00001142 0.00001202 -11.3801444 90.000 4.840 0.00000899 0.00001445 -11.6193977 105.000 | 4.780 0.00000685 0.00001659 -11.8912619 120.000 4.750 0.00000566 0.00001778 -12.08208666 135.000 4.720 0.00000439 0.00001905 -12.33618133 150.000 4.700 0.00000349 0.00001995 -12.56569882 165.000 4.670 0.00000207 0.00002137 -13.08796195 180.000 4.670 0.00000207 0.00002137 -13.08796195 195.000 4.660 0.00000157 0.00002187 -13.3644349 210.000 4.650 0.00000061 0.00002283 -14.30980687 225.000 4.650 0.00000061 0.00002283 -14.30980687 240.000 4.640 0.00000061 0.0000229 -14.30980687 255.000 4.640 0.00000061 0.0000229 -14.30980687 270.000 4.640 0.00000061 0.0000229 -14.30980687 285.000 4.630 0.00002344 Undefined 300.000 | 4.630…
pls complete the 2nd table given the data1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)
pls complete the table below using the given data
A student completed the lab and obtained the following concentration vs rate data: Trial [CV*L (M) [OH-1L(M) Rate 1st 30 sec(M/s) 1.00E-05 5.00E-03 6.290E-09 4.00E-06 5.00E-03 2.610E-09 3 1.00E-05 1.00E-03 1.320E-09 Based on their data, complete the following regarding the rate order dependence and rate law. Give your answer as a decimal to the nearest hundredth. [CV*] (OH'] Rate=k[CV*] [OH']
NH4+ {aq) + NO2(aq) -> N2(g) +2H2O{l} Data Initial [NH4+] Initial [NO2-] rate 1 0.0100 0.200 5.4 x10-7 2 0.0200 0.200 10.8x10-7 3 0.0400 0.200 21.5x10-7 4 0.200 0.0202 10.8x10-7 5 0.200 0.0404 21.6x10-7 6 0.200 0.0808 43.3x10-7 Find x,y,k
A+B-C A(M) B(M)Initial Rate (M/h) 0.154 0.189 163 0.684 0.189 726 0.154 0.809 892 Find the order with respect to A. Round to the nearest whole number.
please complete the table
I need help finding the rate law for each graph. The first graph is in order zero, the middle is in order first and the last is in order second.
Given: A + B + C ----> Prods. Find the rate law and k (specific rate constant). [A] [B] [C] initial rate (Ms-1) exp.1 0.20 0.10 0.90 1.8 x 10-2 exp.2 0.10 0.20 0.30 3.0 x 10-3 exp.3 0.20 0.20 0.30 1.2 x 10-2 exp.4 0.20 0.20 0.10 4.0 x 10-3 rate = k[A]x[B]y[C]z
A+B+CD Exp. Initial A (mol/dm³) Initial B (mol/dm³) Init. Rate of Formation of D (mol/dm³ min-¹) 1 0.10 0.10 3.0 x 10-4 2 0.30 0.30 9.0 x 10-4 3 0.10 0.30 3.0 x 10-4 4 0.20 0.40 6.0 x 10-4 5 0.10 0.10 1.2 x 10-3 The student concluded that the rate equation should be: rate = K[A] [B][C]² ii) Using the data for experiment 4, calculate the value of the rate constant, k, using the correct rate equation, making sure that you include the correct units. Initial C (mol/dm³) 0.10 0.10 0.10 0.10 0.20
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