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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

The total pressure for a mixture of N2O4 and NO2 is 0.15 atm. If Kp = 7.1 (at 25 °C), calculate the partial pressure of each gas in the mixture.

2 NO2(g) ⇄ N2O4(g)

Interpretation Introduction

Interpretation:

The partial pressure of each gas in the mixture of N2O4andNO2 has to be calculated.

Concept Introduction:

Equilibrium constant in terms of pressure[Kp]: Equilibrium constant can be expressed in terms of partial pressures in atmospheres.

aA(g)+bB(g)cC(g)+dD(g)KP=PCc×PDdPAa×PBb

The activity of solid substance will not appear in equilibrium and numerically it is considered as one.

Explanation

Given:

2NO2(g)N2O4(g)Totalpressure=0.15atmKp=7.1

Initially 2 moles of NO2 is present and the amount of N2O4 will be zero.

2NO2(g)N2O4(g)Initialconcentration20IfxmolesofNO2dissociatestoformxmolesofN2</

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