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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
28 views

. For the reaction:
H 2 ( g ) + F 2 ( g ) 2HF ( g ) K = 2.1 × 10 3 at a certain temperature. At equilibrium, [ H 2 ] = [ F 2 ] = 0.08 M . What is the concentration of HF under these conditions?

Interpretation Introduction

Interpretation:

The concentration of HF under the given conditions is to be determined.

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.

Explanation

The given reaction is H2(g)+F2(g)2HF(g).

It is given that the value of K=2.1×103 at a certain temperature and at equilibrium, H2=F2=0.083M.

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

K=HF2H2F2

Substitute the value of equilibrium constant and equilibrium concentrations of H2 and F2 in the above equation.

K=HF2H2F22.1×103= HF20.0830.0832

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