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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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. The equilibrium constant for the reaction
H 2 ( g ) + F 2 ( g ) 2HF ( g )    has the value 2.1 × 10 3 at a particular temperature. When the system is analyzed at equilibrium at this temperature, the concentrations of both H2(g) and F2(g) are found to be 0.0021 M. What is the concentration of HF(g) in the equilibrium system under these conditions?

Interpretation Introduction

Interpretation:

The concentration of HFg in the equilibrium system under the given conditions 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=CcDdAaBb.

Explanation

The given reaction is,

H2g+F2g2HFg

The expression of equilibrium constant for general reaction is,

K=ProductsReactants

Therefore, the expression of equilibrium constant for given reaction is,

K=ProductReactant=HF2H2F2 (1)

The above expression can be written as,

K=HF2H2F2HF=KH2F2 (2)

The given concentration value of H2 is 0

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