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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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. For the reaction
CO 2 ( g ) + H 2 ( g ) CO ( g ) + H 2 O ( g )    the equilibrium constant. K, has the value 5.21 × 10 3 at a particular temperature. If the system is analyzed at equilibrium at this temperature, it is found that [ CO ( g ) ] = 4.73 × 10 3 M , [ H 2 O ( g ) ] = 5.21 × 10 3 M , and [ CO 2 ( g ) ] = 3.99 × 10 2 M . What is the equilibrium concentration of H2(g) in the system?

Interpretation Introduction

Interpretation:

The equilibrium concentration of H2g in the system 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,

CO2g+H2gCOg+H2Og

The expression of equilibrium constant for general reaction is,

K=ProductsReactants

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

K=ProductsReactants=COH2OCO2H2 (1)

The above expression can be written as,

K=COH2OCO2H2H2=COH2OKCO2 (2)

The given concentration value of CO is 4.73×103M

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