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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
144 views

. Suppose that for a hypothetical reaction:
A 2 ( g ) + 2B ( g ) 2AB ( g )    It is determined that at a certain temperature the equilibrium concentrations are: [ A 2 ] = 0.0090 , [ B ] = 0.940 , and [ AB ] = 5.3 × 10 4 . Calculate the numerical value of K for the reaction.

Interpretation Introduction

Interpretation:

The numerical value of K for the reaction is to be calculated.

Concept Introduction:

In a chemical equilibrium the concentration of the reactants and products remain constant. The rate of the forward reaction is equal to the rate of backward reaction. The equilibrium constant of a reaction is expressed as the ratio of the concentration of the products and reactants, each raised to the power of their stoichiometric coefficients. The general equilibrium reaction is represented as,

aA+bBcC+dD

The equilibrium constant for the above chemical reaction is expressed as,

K=CcDdAaBb

Where,

  • A represents the concentration of reactant A at equilibrium.
  • B represents the concentration of reactant B at equilibrium.
  • C represents the concentration of product C at equilibrium.
  • D represents the concentration of product D at equilibrium.
  • a represents the stoichiometric coefficient of reactant A.
  • b represents the stoichiometric coefficient of reactant B.
  • c represents the stoichiometric coefficient of product C.
  • d represents the stoichiometric coefficient of product D.
Explanation

The given hypothetical reaction is,

A2(g)+2B(g)2AB(g)

The equilibrium concentrations are,

A2=0.0090B=0.940

AB=5.3×104

The equilibrium constant for the given hypothetical chemical reaction is expressed as,

K=AB2A21B2

Substitute the value of equilibrium concentration in the above equation.

K=  AB2A21B2= 5

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