   # The equation for the decomposition of NO 2 (g) at 573 K is 2 NO 2 (g) → 2 NO(g) + O 2 (g). Using the concentration-time data below, determine the order of the reaction with respect to [NO 2 ]. [NO 2 ], m Time, min 0.20 0 0.095 5 0.063 10 0.047 15 (a) first-order (b) second-order (c) zero-order ### 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 14.4, Problem 3RC
Textbook Problem
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## The equation for the decomposition of NO2(g) at 573 K is 2 NO2(g) → 2 NO(g) + O2(g). Using the concentration-time data below, determine the order of the reaction with respect to [NO2]. [NO2], m Time, min 0.20 0 0.095 5 0.063 10 0.047 15 (a) first-order (b) second-order (c) zero-order

Interpretation Introduction

Interpretation:

The order reaction should be identified.

Concept introduction:

Rate of the reaction is independent on concentration of the reactant is called zero order reaction.

Rate constant for zero order reaction can be calculated by using following formula,

Rate constant = k=[A]0 -[A]tt

Rate of the reaction is depends linearly on only one reactant concentration is called first order reaction.

Rate constant for first order reaction can be calculated by using following formula,

Rate constant = k=1ALn[A]0[A]t

Rate of the reaction is depends two reactant concentration is called second order reaction.

Rate constant for second order reaction can be calculated by using following formula,

Rate constant = k=A0AtA0At(t)

The Reaction Rate for a given chemical reaction is the measure of the change in concentration of the reactants or the change in concentration of the products per unit time.

### Explanation of Solution

(a)

The deposition reaction of NO2 is shown below,

2NO2(g)2NO(g) + O2(g)

rate=k[NO2]x

For zero order reaction,

Generally zero order reactions are,

Rate constant = k=[A]0 -[A]ttRate constant = k1=0.2 - 0.0955Rate constant = k1=0.021Mmin-1Rate constant = k2=0.2 - 0.06310Rate constant = k2=0.0137Mmin-1Rate constant = k3=0.2 - 0.04715Rate constant = k3=0.0102Mmin-1

The rate constant values are varying from each other. Therefore it is not a zero order reaction.

For first order reaction,

Rate constant = k=1ALn[A]0[A]tRate constant = k1=15Ln0.2 0.095Rate constant = k1=0.1488Mmin-1Rate constant = k2=110Ln0

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