   Chapter 14, Problem 20PS

Chapter
Section
Textbook Problem

The decomposition of nitrogen dioxide at a high temperatureNO2(g) → NO(g) + ½ O2(g)is second-order in this reactant. The rate constant for this reaction is 3.40 L/mol · min. Determine the time needed for the concentration of NO2 to decrease from 2.00 mol/L to 1.50 mol/L.

Interpretation Introduction

Interpretation: The time required for the reaction has to be calculated.

Concept introduction:

Rate law or rate equation: The relationship between the reactant concentrations and reaction rate is expressed by an equation.

aA + bBxXRate of reaction = k [A]m[B]n

Integrated rate law for second order reactions:

Taking in the example of following reaction,

aAproducts

And the reaction follows second order rate law,

Then the relationship between the concentration of A and time can be mathematically expressed as,

1[A]t=kt+1[A]0

The above expression is called as integrated rate for second order reactions.

Explanation

The time required is calculated as,

-Δ[R]Δt = k[R]2,The relation can be transformed into,1[R]t - 1[R]0 = ktGiven:[NO2]t = 1.50 mol/L[NO2]0 = 2.00 mol/Lk = 3.40  L/mol.min t = ?Therefore,1[R]t - 1

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Find more solutions based on key concepts 