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Chapter 14, Problem 23PS
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### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

#### Solutions

Chapter
Section
BuyFindarrow_forward

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
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,

â€‚Â -Î”[R]Î”tÂ =Â k[R]0,TheÂ relationÂ canÂ beÂ transformedÂ into,[R]t-[R]0Â =Â -â€‰ktGiven:Initialâ€‰concentration,[Ammonia]0Â =Â (0.16g17.031g/mol)1LÂ =Â â€‰0.0094Â mol/LInitially,Â 100%Â ofÂ buatadieneÂ isÂ presentÂ andÂ duringÂ process,Â 100%Â ofÂ butadieneÂ hadÂ dimerized.So,â€‰100%-100%Â =â€‰0%â€‰ofâ€‰Ammoniaâ€‰isÂ presentâ€‰as[Ammonia]t.Finalâ€‰concentration,[Ammonia]tÂ =Â 0

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