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…

QUESTION 1 The following data may be used for the questions that follow: NH 3(g) + BF 3(g) →F 3BNH 3(s). Initial Rate Experiment [BF3] [NH3](M) (M/s) 1 0.250 0.250 0.2130 0.250 0.125 0.1065 0.200 0.100 0.0682 0.350 0.100 0.1193 0.175 0.100 0.0596 Based on the data in the preceding table, what is the reaction order with respect to NH 3? Zero order First order Second order Cannot be determined QUESTION 2 The following graphs can be used for the questions that follow:

QUESTION 1 The following data may be used for the questions that follow: NH 3(g) + BF 3(g) →F 3BNH 3(s). Initial Rate Experiment [BF3] [NH3](M) (M/s) 1 0.250 0.250 0.2130 0.250 0.125 0.1065 0.200 0.100 0.0682 0.350 0.100 0.1193 0.175 0.100 0.0596 Based on the data in the preceding table, what is the reaction order with respect to NH 3? Zero order First order Second order Cannot be determined QUESTION 2 The following graphs can be used for the questions that follow:

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...

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Question Use the initial rates method with the given data to determine the rate law for the hypothetical reaction shown below. A+B → C • Write the rate law in the form of rate = k[A]"[B]", specifying the value of the rate constant (k) and the reaction orders (m and n). • Include three significant figures in the rate constant. • Enter your answer in decimal form, do not use scientific notation. Trial [A] (mol/L) [B] (mol/L) 1 2 3 Provide your answer below: rate = 0.0300 0.0300 0.0600 0.0300 0.0600 0.0300 A[A] At (mol L-¹s-¹) 0.0004851 0.0004851 0.0019404
Question 5 The following reaction has an average rate of appearance of H20 of 0.1201 M h-1 in the first 1.5 hours. What is the average rate (in Mh 1 to 3 decimal places) of disappearance of C2H5NO02 during this time frame? 2C,H;NO2 (aq) → C,H3N2O3 (aq) + H20(1) 11:0
Given the experimental information in the following table below: Why are the rates calculated not equal? A → products Time (minutes) [A] (M) 0.00 0.1563 1.00 0.1469 2.00 0.1431
Question 1 Using the data below, report the exponent for each reactant in the rate law, as well as the overall reaction order. rate = k[A)*[B]Y 2A + B- 3C Rate Ms-1 [A)] 0.10 0.10 (B] 0.20 0.40 0.25 0.25 0.20 0.80 0.50 3 A.0 B. 1 vy= C.2 v overall reaction order D. 3 E.4 F. 5 G.6 H.Cannot be determined from the information given A Moving to another question will save this response. MacBook Air SO FB 1 %23 % 2 3 4 & 5 9 E T Y P G J K C. N nd comp B.
Question 2 options: The balanced equation for a given reaction is X + Y → P. The following data regarding initial reaction rates were collected in the lab. Fill in the blanks regarding this reaction by typing the correct number without units. Trial [X] (M) [Y] (M) Rate (M/s) 1 0.020 0.060 3.40 x 10–3 2 0.020 0.120 2.72 x 10–2 3 0.080 0.060 1.36 x 10–2 What is the order with respect to X? What is the order with respect to Y? What is the overall order of the reaction? What is the rate constant, k, written to 3 significant figures?
Question 23 (3.333333333 points) For the following gas phase reaction the average rate of disappearance of N205 over the time period t=0 s to t=100 s is 7.00 x 104 M/s. what is the average rate of formation of NO, over this same time period? 2N2O5 → 4NO2 + O2 O 2.8 x 10-3 M/s O7.0 x 102 M/s O 3.5 x 10 2 M/s O 1.4 x 10-3 M/s O7.0 x 10-4 M/s Il app.honorlock.com is sharing your screen. Stop sharing Hide > F3 F4 F5 F6 F7 F8 F9 F10 & 4 5 7 Y
A + B → C [A](M)[B](M) Initial Rate (M/h) 0.137 0.277 193 0.428 0.277 1,470 0.137 0.679 547 Find the order with respect to B. Round to the nearest whole number.
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Question 5 Initial rate data were obtained for the following reaction: 2 A (g) + B (g) → C (g) + D (g) Experiment [A], Mol/L [B) Mol/L Rate 1 0.20 0.10 2.2 x 10-3 2 0.40 0.10 4.4 x 10-3 3 0.20 0.30 1.32 x 10-2 Write the letter of the correct answer. 1. What is the order of the reaction with respect to A? 2. What is the order of the reaction with respect to B? A. Zero B. First C. Second
Question 6 For this reaction occurring at 20 °C, the following data was obtained. C6H12O + Br2 → C6H₁1OBr + HBr Run 1 2 3 C6H12O (M) 0.20 0.40 0.40 Br2 (M) 0.15 0.15 0.30 Initial Rate (M/min) 2.52 x 10-4 10-4 5.09 x 10-4 2.52 x What would be the rate constant, k, for the reaction? The answer will be in 2 significant figures.
Given the experimental data, 2 Na + Cl2 à 2 NaCl Initial [Na] Initial [Cl2] Initial Rate Experiment of Reaction (M) (M) (M/s) 1 0.440 2.40 10.00 x 10 -4 2 0.440 1.20 5.00 x 10 -4 0.220 2.40 5.00 x 10 -4 4 0.220 1.20 1.25 x 10 -4 Write the rate law expression for the reaction, the overall order of reaction; and calculate the rate constant (k).
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