   Chapter 14.4, Problem 14.6CYU

Chapter
Section
Textbook Problem

Gaseous azomethane (CH3N2CH3) decomposes to ethane and nitrogen when heated:CH3N2CH3(g) → CH3CH3(g) + N2(g)The decomposition of azomethane is a first-order reaction with k = 3.6 × 10‒4 s‒1 at 600 K.(a) A sample of gaseous CH3N2CH3 is placed in a flask and heated at 600 K for 150 seconds. What fraction of the initial sample remains after this time?(b) How long must a sample be heated so that 99% of the sample has decomposed?

(a)

Interpretation Introduction

Interpretation: The fraction of initial sample which will remain after 150s has to be determined.

Concept introduction:

Integrated Rate law of first order reaction: The reaction rate is directly proportional to the concentration of R raised to the first power.

ln[R]t[R]0 = -k t

Explanation

As the reaction process follows first-order, the integrated law of first order reaction follows,

Given:[CH3N2CH3]initial = 0.020 mol/L[CH3N2CH3]final = ?k = 3.6×10-4s-1 t = 150 secTherefore,ln[CH3N2CH3]t[CH3N2CH3]0 = -k t                            = -(3

(b)

Interpretation Introduction

Interpretation: The time taken to the decomposition of 99% of the sample has to be calculated.

Concept introduction:

Integrated Rate law of first order reaction: The reaction rate is directly proportional to the concentration of R raised to the first power.

ln[R]t[R]0 = -k t

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