A zero-order reaction has a constant rate of 4.20×10-4 M/s. If after 80.0 seconds the concentration has dropped to 3.50×10-²M, what was the initial concentration?Express your answer with the appropriate units.► View Available Hint(s)μᾶ[A]o = ValueSubmitUnits?

Integrated rate equation for a zero order reaction is,[A]t = [A]0 - kt[A]0 - Initial concentration…

A zero-order reaction has a constant rate of 4.20x10-4 M/s. If after 80.0 seconds the concentration has dropped to 3.50x10-² M, what was the initial concentration? Express your answer with the appropriate units. ► View Available Hint(s) μA [A]o = Value Submit W Units

A zero-order reaction has a constant rate of 4.20x10-4 M/s. If after 80.0 seconds the concentration has dropped to 3.50x10-² M, what was the initial concentration? Express your answer with the appropriate units. ► View Available Hint(s) μA [A]o = Value Submit W Units

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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A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step 1 slow: F2 + ClO2 FClO2 + F step 2 fast: F + ClO2 FClO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]m[B]n... , where '1' is understood (so don't write it) for m, n etc.) Rate =
Part B Consider the second-order reaction: 2HI(g)→H₂(g) + I₂(g) Use the simulation to find the initial concentration [HI], and the rate constant k for the reaction. What will be the concentration of HI after t = 5.44x10¹0 s ([HI]) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. ► View Available Hint(s) for Part B for Part do for Part redo for Part B res@or Part B keyboard shortcuts for Part B help for Part B [HI] = 1.6810³ Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining mol L
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The rate law for the reaction NH (aq) + NO₂(aq)- N₂(g) + 2H₂O() is given by rate=1 NH][NO] At a certain temperature, the rate constant is 4.10 × 10 Mis Calculate the rate of the reaction at that temperature if [NH]- -0.301 M and [NO] -0.170 M. Round your answer to 3 significant digits Check x D.O 100
Question 13 of 26 Using the data in the table, calculate the rate constant of this reaction. A+B C + D Incorrect k= O ÏI Trial 1 2 3 Units. Incorrect [A] (M) 0.390 0.390 0.624 60°F [B] (M) 0.360 0.972 0.360 O Attempt 1 Rate (M/s) 0.0146 0.106 0.0234 10:23 PM 5/30/2022 11
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Enabled: Exam 2 Be sure to answer all parts. Consider the reaction A+B Products From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. [A] (M) | [B] (M) Rate (M/s) A. 匚 1.50 1.50 2.50 01 x 07 Reaction 1.50 6.40 x 10 Proctorio is sharing your screen. Stop sharing < Prev 10 of 17
11:20 PM Sat Feb 4 The reaction A + 2B + C → Products has a rate law of Rate = k[A]2[B]. By what factor would the reaction rate change if [A] is tripled? Tap here or pull up for additional resources ! # $ Question 18 of 34 % A *00 8
1:18 Sun, 16 June bb. = University of South Australia Dashboard Course Outline Content Academic Integrity Assessment In Grades Ө SP2 2024 Chemistry 100 Dashboard > CHEM 1006 > Online Quizzes > Online quiz 4 Question 4 If the rate law for the reaction Correct Mark 1.00 out 2A + 3B → products of 1.00 Remove flag is first order in A and second order in B, then the rate law is rate = a. k[A][B] b. k[A][B]² c. K[A]²[B]² d. k[A][B] e. k[A]²[B] Extensions Resources Your answer is correct. The correct answer is: k[A][B]² Recordings 16 b *༢ དཱི51% 10 ? Yunseo Kwon = ||| о Sunday, 16 June 2024 1:18 am ACST ←
Remaining Time: 2 hours, 22 minutes, 53 seconds. Question Completion Status: Below is the initial rate data from a few experiments on the reaction: A+B> Products. [A]; (M) Experiment # 11 12 3 The reaction is first order in A. The rate constant is thus: O 5.656 Ms-1 O 2.828 M-1-1 O 11.31 s-1 O 1.414 M-25-1 1.00 2.00 2.00 QUESTION 7 Consider the following reaction: O Equal to the rate of reaction. O Three times the rate of reaction O Twice the rate of reaction One third of the rate of reaction [B]; (M) 2 03(g) -> 3 O2(g) What is the rate of consumption of O3 compared to the rate of reaction? O Half of the rate of reaction. 1.00 .00 2.00 Click Save and Submit to save and submit. Click Save All Answers to save all answers. Rate; (M s-1) 1.414 2.828 11.31 İy S
tab 11:36 AM Thu Feb 23 < aps lock Tap here or pull up for additional resources What is the half-life for a particular reaction if the rate law is rate= (1261 M-¹*min-¹) [A]² and the initial concentration of A is 0.250 M? ! 1 Q A N 2 W S X #3 E D $ 4 R TI F de 5 % V T G 6 ... Question 9 of 26 Y & 1% 7 H U : 8 00 J I ( 9 = K 1 4 7 +/- -0 0 V L P
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