A reaction is 2nd order with respect to [ Reactant A ]. If the rateconstant from the equation of the trendline in Excel is 3.22 x 103(units deliberately omitted), and the initial concentration is0.437 M A, then what is the[ Reactant A] (in M A) at 300minutes?IMPORTANT: When entering your answer:• Enter the number only (no units)• Do not leave any spaces• Use a leading zero before the decimal when necessary• Report your number to 3 decimal places (regardless of thesignificant figures)• Correctly round your answer to the 3rd decimal place (marginof allowed error is only + 0.001, so always use un-roundednumbers in your calculations). If the last digits are zeros theywill not display once you click away, but the answer will stillbe marked correct.Examples: 0.123 or 0.045

Answered: A reaction is 2nd order with respect to…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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Related questions

Question

A reaction is 2nd order with respect to [ Reactant A ]. If the rate
constant from the equation of the trendline in Excel is 3.22 x 10
3
(units deliberately omitted), and the initial concentration is
0.437 M A, then what is the[ Reactant A] (in M A) at 300
minutes?
IMPORTANT: When entering your answer:
• Enter the number only (no units)
• Do not leave any spaces
• Use a leading zero before the decimal when necessary
• Report your number to 3 decimal places (regardless of the
significant figures)
• Correctly round your answer to the 3rd decimal place (margin
of allowed error is only + 0.001, so always use un-rounded
numbers in your calculations). If the last digits are zeros they
will not display once you click away, but the answer will still
be marked correct.
Examples: 0.123 or 0.045

Expert Solution

Step 1

For a second-order reaction, the reaction rate is proportional to the square of the concentration of the reactant. The rate law is $- r_{A} = k {C_{A}}^{2}$ . Here, k is the reaction rate constant and C_A is the concentration of reactant A at any instant of time. Also, it is known that the rate of the reaction is a change in concentration per unit of time. It is therefore equals to $- \frac{d C_{A}}{d t}$ .