QUESTION 1The following data may be used for the questions that follow:NH 3(g) + BF 3(g) →F 3BNH 3(s).Initial RateExperiment[BF3][NH3](M)(M/s)10.2500.2500.213020.2500.1250.10653.0.2000.1000.068240.3500.1000.11930.1750.1000.0596Based on the data in the preceding table, what is the reaction order with respect to NH 3?Zero orderFirst orderSecond orderCannot be determinedQUESTION 2The following graphs can be used for the questions that follow: The following graphs can be used for the questions that follow:0807040302011102050180time(min)10203002-D4y = -0.0358x + 0.1058Linsar (Serie16-18time(min)The data for the decomposition of N 20 5 is shown in the graph. What is the rate law for this reaction?rate = k%3Drate = k[N2O5]3rate = k[N2O5]%3Drate =K[N2O5?SauSave All AnswersClick Save and Submit to save and submit. Click Save All Answers to save all answers.['o°N]

#Question-1: We are given the experimental concentration of reactants and rate data, and we have to…

Answered: QUESTION 1 The following data may be…

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

Section: Chapter Questions

Problem 36QRT

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Rate Law find the initial rate N2O4 - 2 NO2 experiment initial (N2O4) (M) initial rate (M/sec) 1 0.50 0.050 2 1.00 0.200 3 1.50 0.450
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.360 0.290 0.0144 2 0.360 0.580 0.0144 3 0.720 0.290 0.0576 k=
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.360 0.330 0.0164 2 0.360 0.660 0.0164 3 0.720 0.330 0.0656 ?=? Units =?
Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law. Express your answer to three significant figures. Include units for k.
These questions are based on a reaction rate lab for my Chemistry homework. I attached my data values that I have already calculated. I think I am supposed to show more work for 4 and 5. I am genuinely confused on how to plot the graph too (6-7). Lastly, I am not sure if I got 8-10 correct? I think the rate law might be Rate = k [HCl] [Na2S2O3] but I am not sure if it needs an exponent or not?
Rate = k[acetone]1[I2]0[H+]1 rate = 0.001M/ 332.26s = 3.01 x 10-6 my question is what is the S.I unit of this answer? 3.01 x 10-6 = k[0.80M]1 [0.001M]0 [0.20]1 k= (3.01 x 10-6)/ (0.16) k = 1.88 x 10-5 also S.I unit of this answer with clear explanation and steps
Calculate the full rate law using the information below: 2 NACHOS (g) → 12 CHIPS (g) + 3 CHEESE (g) [NACHOS]0 (M) Initial Rate (M–1s–1) 0.101 0.00484 0.0910 0.00437 Group of answer choices Rate = 5.61 × 10–2 M–1 s–1 [NACHOS]2 Rate = 6.03 × 10–1 M–2 s–1 [NACHOS]3 Rate = 4.79 × 10–2 s–1 [NACHOS] Rate = 1.66 × 10–3 M1/2 s–1 [NACHOS]2/3 Rate = 1.78 × 10–2 M–1/2 s–1 [NACHOS]3/2
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.340 0.210 0.0204 2 0.340 0.420 0.0204 3 0.680 0.210 0.0816 ?=
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Determine the missing initial rate: 2N2O5 → 4NO2 + O2 [N2O5] Initial rate (Ms-1) 0.093 4.84x10-4 0.084 4.37x10-4 0.224 ??
Determine the average rate of change of BB from ?=0 st=0 s to ?=272 s.t=272 s. A⟶2BA⟶2B Time (s) Concentration of A (M) 0 0.7300.730 136136 0.4450.445 272272 0.1600.160 rateB= __________M/s

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