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
С-2 (i) Write the rate formula for the following reaction in terms of both reactants and products. GaFa + 3 Cs > 3 CsF + Ga (ii) The following data is given for the decomposition of N2O5. 2N2OS(g) > 4NO2(g) + O2(g) [N2O5] (M) 0.0200 0.0142 0.0086 Time (second) 200 500 Determine the average rate of disappearance of N2Os between 0s and 200 s, and between 200 s and 500 s. (iii) Identify the reactant and product from the concentration vs. time graph as given below. Time (iv) A 11.5 M Solution of hydrochloric acid of volume 8 L needed to be diluted to reduce its concentration to 3.5 M. How much of water was added to do this? Concentration
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
for the following reaction mechanism: 1) H2(g) 2NO(g) -> N2O(g)+H2O(g)2) N2O(g)+H2(g) -> N2(g) +H2O(g) A) Write an expression for H2 decrease rate in relation to reactantsB) Write an expression for N2 Increase rate in relation to reactantsC) What is the rate determining step? provide an explanation.