Answered: Second Question A + B → C +D Experiment…

Second Question A + B → C +D Experiment (A]o, M [B]o, M Initial Rate, M/min 1 1.0 1.0 0.0010 2 3.0 1.0 0.0030 3 1.0 2.0 0.0020 Write the order for each reactant and the experiment rate law?

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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Consider a chemical reaction: 3 A +2B2C+2D the initial rate was measured at three different reactant concentrations. What is the rate law for the reaction? Trial 1 2 3 Initial Initial [Α] [B] (mol/L) (mol/L) (mol/(L-min)) 0.300 0.100 0.100 0.100 Initial Rate 0.100 0.200 1.35 x 10-1 1.50 X 10-2 3.00 x 10-2
2) 2 NO₂ (g) +2 NO(g) + O₂(g) (W) [ZON] 2.5 2 1.5 1 0.5 0 10 20 Reaction Data 30 40 50 60 70 Time (s) 80 Use the experimental data for the above reaction to answer. a) What is the average rate of reaction between 50 and 70 seconds? b) Estimate the instantaneous rate of reaction at 20 seconds. 90 100 c) Estimate the instantaneous rate of formation of O₂ at 30 seconds. d) If the initial concentration of NO₂ is 2.0M how much O₂ is produced in the first 40 seconds of reaction?
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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.
▼ Part A Consider the reaction Using the information in the following table, calculate the average rate of formation of P₂O, between 10.0 and 40.0 s. Time (s) 0 10.0 20.0 30.0 50.0 40.0 [P₂05] (M) 02.10×103 5.10×10-3 6.90×103 8.10×10-3³ 8.70x103 Express your answer with the appropriate units. ▸ View Available Hint(s) Submit Previous Answers Rate of formation of P₂O5 = 2.00-10-4 Part B Complete previous part(s) Part C ■ Consider the reaction x² * Incorrect; Try Again; 5 attempts remaining Enter your answer with a different unit type. Review a list of acceptable units HÅ Submit Previous Answers O x"² 5Br (aq) + Bro, (aq) + 6H+ (aq) →3Br₂(aq) + 3H₂O(1) The average rate of consumption of Bris 1.06x104 M/s over the first two minutes. What is the average rate of formation of Brg during the same time interval? Express your answer with the appropriate units. ▸ View Available Hint(s) ||||A HÅ Rate of formation of Br₂ = 7.04.10 5 . Ms-1 * Incorrect; Try Again; 5 attempts remaining x 10" M x 10"…
The following initial rate data are for the gas phase reaction of hydrogen with iodine: H₂+I₂ → 2 HI Experiment [H₂0, M120, M Initial Rate, M.s¹ 0.0212 0.0180 7.17 x 10-22 0.0212 0.0360 1.43 x 10-21 0.0424 0.0180 1.43 x 10-21 0.0424 0.0360 2.87 x 10-21 1 2 4 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or 71. Rate = k= M-1
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The table shown below contains concentration and rate data for this reaction A + 2B ---> C Determine the rate law for this reaction. Experiment Initial [A] Initial [B] Initial Rate 1 0.23 0.17 0.33 2 0.46 0.17 2.64 3 0.23 0.51 0.33 Group of answer choices a) R = k[A]4 b) R = k[A]3[B] c) Rate = k[A]3 d) R = k[A]4[B]
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 13 of 32 Using the information in the table, the rate law for the reaction 2 A(g) + B(g) → C(g) + D(g) is Rate [A], (M) [B], (M) (M/s) A) Rate = k[A][B] 0.100 2.50 0.460 B) Rate = k[B] C) Rate = k[A]°[B] 0.200 2.50 0.920 D) Rate = k[A] 0.300 1.25 1.38 "pe here to search