What is the rate of disappearance of I- when [S2082-] 2.2\times 10-2 M and [1-] = 4.0\times 10-2 M? Express your answer using two significant figures.Activate to select the appropriates template from thefollowing choices. Operate up and down arrow forselection and press enter to choose the input valuetypeActivate to select the appropriates symbol from thefollowing choices. Operate up and down arrow forselection and press enter to choose the input value typerate nothing M/s

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Answered: What is the rate of disappearance of I-…

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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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
Experiment 1: Determination of the Rate, Order, and Rate Constant Table 3: Data for Trial 1 Water displaced in mL Time (seconds) 2 mL 49 4 mL 84 6 mL 116 8 mL 145 10 mL 174 12 mL 202 14 mL 230 16 mL 253 18 mL 280 20 mL 313 22 mL 350 Table 4: Data for Trial 2 Water displaced in mL Time (seconds) 2 mL 78 4 mL 144 6 mL 175 8 mL 205 10 mL 255 12 mL 308 14 mL 330 16 mL 409 18 mL 463 20 mL 515 22 mL 575 Table 5: Data for Trial 3 Water displaced in mL Time (seconds) 2 mL 53 4 mL 100 6 mL 139 8 mL 178 10 mL 213 12 mL 247 14 mL 282 16 mL 319 18 mL 363 20 mL 412 22 mL 463 help me with this part Order with respect to H2O2 ___________________ Order with respect to KI ______________________
Set up an ice table, find the Kb expression and find the initial concentration for C6H5NH3+
Experiment 1: Determination of the Rate, Order, and Rate Constant Table 3: Data for Trial 1 Water displaced in mL Time (seconds) 2 mL 49 4 mL 84 6 mL 116 8 mL 145 10 mL 174 12 mL 202 14 mL 230 16 mL 253 18 mL 280 20 mL 313 22 mL 350 Table 4: Data for Trial 2 Water displaced in mL Time (seconds) 2 mL 78 4 mL 144 6 mL 175 8 mL 205 10 mL 255 12 mL 308 14 mL 330 16 mL 409 18 mL 463 20 mL 515 22 mL 575 Table 5: Data for Trial 3 Water displaced in mL Time (seconds) 2 mL 53 4 mL 100 6 mL 139 8 mL 178 10 mL 213 12 mL 247 14 mL 282 16 mL 319 18 mL 363 20 mL 412 22 mL 463 Help me with this part Trial 1 (Table 3) Slope ______________________ Reciprocal Slope _______________ Trial 2 (Table 4)…
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Experiment 1: Determination of the Rate, Order, and Rate Constant Table 3: Data for Trial 1 Water displaced in mL Time (seconds) 2 mL 49 4 mL 84 6 mL 116 8 mL 145 10 mL 174 12 mL 202 14 mL 230 16 mL 253 18 mL 280 20 mL 313 22 mL 350 Table 4: Data for Trial 2 Water displaced in mL Time (seconds) 2 mL 78 4 mL 144 6 mL 175 8 mL 205 10 mL 255 12 mL 308 14 mL 330 16 mL 409 18 mL 463 20 mL 515 22 mL 575 Table 5: Data for Trial 3 Water displaced in mL Time (seconds) 2 mL 53 4 mL 100 6 mL 139 8 mL 178 10 mL 213 12 mL 247 14 mL 282 16 mL 319 18 mL 363 20 mL 412 22 mL 463 help me with this part 1. Should the rate constant (k) be the same for all three trials in this experiment? Explain your answer.…
ucose-cocp-2000+100g ge Find Cyoy the value of the [HgCl2] (M) [C2042-1 (M) | Rate (Mis) 0.10 0.10 1.3.10-7 0.10 0.20 5.2.10-7 0.20 0.20 1.0-10-6 A) 1.4 x 10-8 1/M2-s B) 1.3 x 10-7 1/M2-s C) 1.4 x 10-5 1/M2-s D) 1.3 × 10-4 1/M2-s
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']
Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. Reaction Molecularity Rate expression CH3 + 0z + N2 - (a) CH30,N2 rate unimolecular bimolecular (b) НСО + 0, HO2 + CO rate = - termolecular (c) NO,C1 NO, + Cl rate = Submit Answer Try Another Version 10 item attempts remaining
Experiment Initial [Br–] (M) Initial [BrO3–] (M) Initial [H+] (M) Rate of Disappearance of BrO3– (M s-1) 1 0.00100 0.00500 0.100 2.50x10-4 2 0.00200 0.00500 0.100 5.00x10-4 3 0.00100 0.00750 0.100 3.75x10-4 4 0.00100 0.01500 0.200 3.00x10-3 Determine the order of the reaction for [H+]
Which of the following parameters do you need to optimize before carrying out the experiments that will test your hypothesis. Select all that apply. OExtinction coefficient of pNP O Peak absorbance wavelength of pNP O Optimal reaction pH O Optimal reaction incubation time
Plot a Graph and Determine the Rate: Make a graphical plot of reaction time (x-axis) and spectrophotometer readings [Use the calculated average] (y-axis). Determine the initial velocity (rate) of the reaction by extending the initial straight-line portion of your reaction curve and calculating the gradient of the straight line (difference in y/ difference in ×). The units of the rate will be in absorbance units min' (abs min-"). What is the rate of the reaction based on your plotted values:

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