Part BThe integrated rate law allows chemists to predict thereactant concentration after a certain amount of time, orthe time it would take for a certain concentration to bereached.What is the rate constant of a first-order reaction that takes 307 seconds for the reactant concentration to drop to half of its initial value?The integrated rate law for a first-order reaction is:Express your answer with the appropriate units.[A] = [A]oe kt• View Available Hint(s)Now say we are particularly interested in the time it wouldtake for the concentration to become one-half of its initial[A],for [A] and?value. Then we could substitute2rearrange the equation to:ValueUnits0.693t1/2 =kThis equation calculates the time required for thereactant concentration to drop to half its initial value. Inother words, it calculates the half-life.Submit

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The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: What the rate constant of a first-order reaction that takes 307 seconds for the reactant concentration to drop to half of its initial value? Express your answer with the appropriate units. [A] = [A]ge kt > View Available Hint(s) Now say we are particularly interested in the time it would take for the concentration to become one-half of its initial value. Then we could substitute for [A and ? rearrange the equation to: Value Units 0.693 This equation calculates the time required for the reactant concentration to drop to half its initial value, In other words, it calculates the half-life. Submit

The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: What the rate constant of a first-order reaction that takes 307 seconds for the reactant concentration to drop to half of its initial value? Express your answer with the appropriate units. [A] = [A]ge kt > View Available Hint(s) Now say we are particularly interested in the time it would take for the concentration to become one-half of its initial value. Then we could substitute for [A and ? rearrange the equation to: Value Units 0.693 This equation calculates the time required for the reactant concentration to drop to half its initial value, In other words, it calculates the half-life. Submit

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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Part A A first-order reaction (AB) has a half-life of 25 minutes. If the initial concentration of A is 0.900 M, what is the concentration of B after 50 minutes? (Do not use a calculator to solve this problem.) Express your answer with the appropriate units. [B] = Submit ovide Feedback ■ μA Value Request Answer @ C Units ? Review | Constants I Periodic Table P Pearson MacBook Pro Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us | Nex
A plot of In[A] versus time (in seconds) for a First Order Reaction has the following trendline equation: y = -0.006283x -0.639 Calculate the concentration of the reactant at time=72 seconds. (Report your answer to 3 SF. Include units of M in your answer) Answer:
After gathering rate data, a chemist graphed the data to obtain a linear representation of the data. The graph shown below best depicts a time (s) A) zero order reaction with respect to reactant A B) first order reaction with respect to reactant A C) second order reaction with respect to reactant A D) third order reaction with respect to reactant A (W) [V]
Based on the data below. Graphically determine the rate law for the reaction, and extract the rate constant and initial concentrations. 2 A -----> B Time [A] 5 11.4730407 10 7.6906092 15 5.15516951 20 3.45561346 25 2.31636698 30 1.55270722 35 1.04081077
Can someone please help with question 11 a and b
Current Attempt in Progress The following reaction is investigated to determine its rate law: 2NO(g) + 2H2(g) → N2(g) + 2H2O(g) Experiments yielded the following results: Initial Concentrations (mol L-1) Initial Rate of Formation of N, (mol L-s-) [NO) [H,1 0.40 x 10-4 0.30 x 10-4 1.0 x 10- 0.80 x 10-4 0.30 x 10-4 4.0 x 10- 0,80 x 10-4 0.60 x 10-4 8.0 x 10- What is the rate law for the reaction? O rate = k [NO][H2]² O rate = k [NO]?[H2] O rate = k (NO]?[H2]? O rate = k (NO][H2] What is the value of the rate constant? k= i x 105 O L mol 1s1 O s-1 O L³mol 3s1 O mol L1s-1 O L² mol-2s 1
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A certain reaction is second order in N₂ and first order in H₂. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. 1.58 M 0.540 M 3.89 M 0.382 M 0.382 M 0.155 M Explanation initial rate of reaction Check 0.440 M/s Mis MIS X S tv W MacBook Air © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center C 5 Accessibility
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0125s−1:→2SO3g+2SO2gO2g Suppose a vessel contains SO3 at a concentration of 0.270M. Calculate the concentration of SO3 in the vessel 98.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M