   # The following data were obtained for the gas-phase decomposition of dinitrogen pentoxide, 2N 2 O 5 ( g ) → 4 NO 2 ( g ) + O 2 ( g ) [N 2 O 5 ] 0 (mol/L) Initial Rate (mol/L · s) 0.0750 8.90 × 10 −4 0.190 2.26 × 10 −3 0.275 3.26 × 10 −3 0.410 4.85 × 10 −3 Defining the rate as −∆[N 2 O 5 ]/ ∆ t write the rate law and calculate the value of the rate constant ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 11, Problem 32E
Textbook Problem
59 views

## The following data were obtained for the gas-phase decomposition of dinitrogen pentoxide, 2N 2 O 5 ( g ) → 4 NO 2 ( g ) + O 2 ( g ) [N2O5]0(mol/L) Initial Rate (mol/L · s) 0.0750 8.90 × 10−4 0.190 2.26 × 10−3 0.275 3.26 × 10−3 0.410 4.85 × 10−3 Defining the rate as −∆[N2O5]/ ∆t write the rate law and calculate the value of the rate constant

Interpretation Introduction

Interpretation: A gas phase decomposition reaction of dinitrogen pentoxide and its rate expression is given. The rate law and the value of the rate constant are to be calculated.

Concept introduction: The change in the concentration of the reactants or the products formed in a chemical reaction per unit time is known as the rate of the given chemical reaction. The relation between the reaction rate and the concentration of the reactants is stated by the rate law.

To determine: The rate law for the given reaction.

### Explanation of Solution

Given

The stated reaction is,

2N2O5(g)4NO2(g)+O2(g)

The rate law for the given reaction is calculated by the expression,

Rate=k[N2O5]n

Where,

• [N2O5] is the concentrations of N2O5 .
• k is the rate constant.
• n is the order of the reaction.

The value of n is calculated by the comparison of the different initial rate values from the given table.

The value of n is calculated using the first and second result. Substitute the values of the concentration of [N2O5] in the last two experiments in the above expression.

Rate1=k[0.0750]n

Rate2=k[0.190]n

According to the given rate values in the table,

Rate4Rate3=2.26×103mol/Ls8.90×104mol/Ls

Therefore,

k[0.190]nk[0.0750]n=2.26×103mol/Ls8.90×104mol/Ls(2.53)n=2.53n=1

Substitute the values of n in the rate law expression.

Rate=k[N2O5]1

To determine: The value of the rate constant, k

### 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
What are the three suborders of primates?

Biology (MindTap Course List)

To prevent wasting of dietary protein, which of the following conditions must be met? a. Dietary protein must b...

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

What are the three most common chronic conditions affecting men over age 65?

Nutrition Through the Life Cycle (MindTap Course List)

A metal rod having a mass per unit length carries a current I. The rod hangs from two wires in a uniform verti...

Physics for Scientists and Engineers, Technology Update (No access codes included)

a 7.11 hg to g, b 5.27 x 107 m to pm, c 3.63 x 106 g to dag.

Introductory Chemistry: An Active Learning Approach 