Chapter 15, Problem 17PS

### Chemistry & Chemical Reactivity

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

Chapter
Section

### Chemistry & Chemical Reactivity

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

# Carbonyl bromide decomposes to carbon monoxide and bromine.COBr2(g) ⇄ CO(g) + Br2(g)Kc is 0.190 at 73 °C. If you place 0.0500 mol of COBr2 in a 2.00-L flask and heat it to 73 °C, what are the equilibrium concentrations of COBr2, CO, and Br2? What percentage of the original COBr2 decomposed at this temperature?

Interpretation Introduction

Interpretation: The concentration of COBr2,COandBr2 when the system comes to equilibrium and the percentage of the original CoBr2 decomposed at 700C has be to determined.

Concept introduction:

• Equilibrium constant: At equilibrium the ratio of products to reactants has a constant value. And it is represented by the letter K.

For a general reaction, aA+bBcC+dD

The equilibrium constant Kc = [C]c[D]d[A]a[B]b, where a, b, c and d are the stoichiometric coefficients of reactant and product in the reaction. Concentration value for solid substance is 1.

If the value of Kc and the concentration of any of the reactant of a reaction is known then the concentration of product can be determined by multiplying Kc with the concentration of reactant.

• Concentration =AmountofsubstanceVolume
• Amountofsubstance=Concentration×Volume
• ICE (reaction initial concentration equilibrium) table is mainly used to calculate the value of K for a reaction. This table contains the concentration of reactant and product in various stage of reaction.
Explanation

Carbonyl bromide decomposes to carbon monoxide and bromine.

â€ƒâ€‚Â â€‚Â COBr2(g)â€‰â€‰â€‰â‡„â€‰â€‰CO(g)â€‰â€‰+Br2(g)

The value of Kc for this decomposition reaction is 0.190â€‰â€‰atâ€‰730â€‰â€‰C

The concentration of COBr2 = 0.05â€‰â€‰mol2Lâ€‰â€‰=â€‰â€‰0.025â€‰mol/L

By using this concentration ICE table for this reaction can be constructed as follows,

 Reaction COBr2(g)â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â‡„â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰CO(g)â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰+â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰Br2(g) Initial concentration(mol/L) 0.025 0 0 Change in concentration (mol/L) âˆ’x +x +x EquilibriumÂ  (mol/L) 0.025â€‰âˆ’x x x

The equilibrium constant for the reaction can be written as,

Kc = [CO][Br2][COBr2]

Kcâ€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰â€‰=â€‰â€‰x20

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