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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 reaction H 2 ( g ) + I 2 ( g ) 2HI ( g ) has K p = 45.9 at 763 K. A particular equilibrium mixture at 763 K contains HI at a pressure of 4.94 atm and H2at a pressure of 0.628 atm. Calculate the equilibrium pressure of I2(g) in this mixture.

Interpretation Introduction

Interpretation:

The equilibrium pressure of I2g in the given mixture is to be calculated.

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,

aAg+bBgcCg+dDg

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

K=CcDdAaBb

The equilibrium constant in terms of pressure is expressed as,

Kp=pCgcpDgdpAgapBgb.

Explanation

The given reaction is,

H2(g)+I2(g)2HI(g).

The value of KP=45.9 at 763 K.

The pressure of HI=4.94 atm.

The pressure of H2=0.628 atm.

The equilibrium constant in terms of pressure for the given chemical reaction is expressed as,

KP=pHIg2pH2gpI2g

Substitute the value of equilibrium constant and the pressure of HI and H2 in the above equation

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