   Chapter 17, Problem 20QAP ### Introductory Chemistry: A Foundati...

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

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

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

# . Ammonia. a very important industrial chemical. is produced by the direct combination of the following elements under carefully controlled conditions: N 2 ( g ) + 3H 2 ( g ) ⇌ 2NH 3 ( g )    Suppose. in an experiment, that the reaction mixture is analyzed after equilibrium is reached, and it is found, at a particular temperature. that [ NH 3 ] = 0.25 M , [ H 2 ] = 3.4 × 10 − 3 M , and [ N 2 ] = 5.3 × 10 − 5 M . Calculate the value of K at this temperature.

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 NH3 is 0.25M.

The equilibrium concentration of H2 is 3.4×103M.

The equilibrium concentration of N2 is 5.3×105M.

The given equation is represented as,

N2(g)+3H2(g)2NH3(g)

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

K=[NH3]2[N2][H2]

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