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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
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. At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide.
N 2 ( g ) + O 2 ( g ) 2NO ( g )    Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations arc found to be [ N 2 ] = 0.041 M . [ O 2 ] = 0.0078 M , and [ NO ] = 4.7 × 10 M . Calculate the value of K for the reaction.

Interpretation Introduction

Interpretation:

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

Concept Introduction:

The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,

aA+bBcC+dD

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

K=[C]c[D]d[A]a[B]b

Where,

  • [A] represents the equilibrium concentration of reactant A.
  • [B] represents the equilibrium concentration of reactant B.
  • [C] represents the equilibrium concentration of product C.
  • [D] represents the equilibrium concentration of product D.
  • 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 equilibrium concentration of NO is 4.7×104M.

The equilibrium concentration of O2 is 0.0078M.

The equilibrium concentration of N2 is 0.041M.

The given equation is represented as,

N2(g)+O2(g)2NO(g)

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

K=[NO]2[N2][O2

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