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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
25 views

. For the reaction:
3 O 2 ( g ) 2 O 3 ( g ) K = 1.8 × 10 7 at a certain temperature. If at equilibrium [ O 2 ] = 0.062 M , calculate the equilibrium O3concentration.

Interpretation Introduction

Interpretation:

The equilibrium O3 concentration is to be calculated.

Concept Introduction:

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 reaction is,

3O2(g)2O3(g).

The value of K is 1.8×107 at a certain temperature.

The concentration of O2 is 0.062M at equilibrium.

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

K=O32O23

Substitute the value of equilibrium constant and the equilibrium concentration of O2 in the above equation.

K=O32O231.8×107= O320.06231.8×107= O320

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