   Chapter 14, Problem 23PS

Chapter
Section
Textbook Problem

The decomposition of ammonia on a metal surface to form N2 and H2 is a zero-order reaction (Figure 14.7c). At 873 °C, the value of the rate constant is 1.5 × 10−3 mol/L · s. How long it will take to completely decompose 0.16 g of NH3 in a 1.0-L flask?

Interpretation Introduction

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

Concept introduction:

Integrated law for zero-order reactions:

Consider a reaction,

aAproducts

Then, the rate of the reaction is

Rate=k[A]0

The expression for this reaction can be written as,

Rate=k

According to this law, the rate would not change with change in concentration.

The relationship between concentration and time for a reaction that is zero-order is given as,

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

Explanation

The time required for the reaction is calculated as,

-Δ[R]Δt = k[R]0,The relation can be transformed into,[R]t-[R]0 = -ktGiven:Initialconcentration,[Ammonia]0 = (0.16g17.031g/mol)1L = 0.0094 mol/LInitially, 100% of buatadiene is present and during process, 100% of butadiene had dimerized.So,100%-100% =0%ofAmmoniais presentas[Ammonia]t.Finalconcentration,[Ammonia]t = 0

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