   # The decomposition of N 2 O 5 in CCl 4 is a first-order reaction. If 2.56 mg of N 2 O 5 is present initially and 2.50 mg is present after 4.26 minutes at 55 °C, what is the value of the rate constant, k ? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 14, Problem 16PS
Textbook Problem
628 views

## The decomposition of N2O5 in CCl4 is a first-order reaction. If 2.56 mg of N2O5 is present initially and 2.50 mg is present after 4.26 minutes at 55 °C, what is the value of the rate constant, k?

Interpretation Introduction

Interpretation: The rate constant of the reaction has to be found.

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

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

Rate constant, k: It is a proportionality constant that relates rate and concentration at a given temperature.

### Explanation of Solution

The reaction rate of the chemical reaction is calculated as,

Given:The reaction is first order reaction,rate law is , ln[N2O5]t=-kt+ln[N2O5]0time = 27minsTherefore,ln[N2O5]t=-kt+ ln[N2O5]0ln (2.50 mg) = (k)(4.26mins)+ ln(2

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