   # At 5000 K and 1.000 atm, 83.00% of the oxygen molecules in a sample have dissociated to atomic oxygen. At what pressure will 95.0% of the molecules dissociate at this temperature? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 12, Problem 111CP
Textbook Problem
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## At 5000 K and 1.000 atm, 83.00% of the oxygen molecules in a sample have dissociated to atomic oxygen. At what pressure will 95.0% of the molecules dissociate at this temperature?

Interpretation Introduction

Interpretation: The pressure at which 95% of the Oxygen molecules dissociate is to be calculated.

Concept introduction: The equilibrium constant K describes the ratio of the reactant to the product on the equilibrium conditions in terms of molar concentration.

The equilibrium constant depends upon temperature.

Law of mass action is applicable on the equilibrium reactions.

The Le Chatelier’s principle states that the addition of the reactants shifts the equilibrium to the right while the addition of product shifts the equilibrium to the left at constant temperature.

The dissociation of the species is denotes by the symbol α .

To determine: The pressure at which 95% of the Oxygen molecules dissociate at the constant temperature.

### Explanation of Solution

Explanation

Given

From the given data the reaction is written as,

O2(g)2O(g)

The temperature is 5000K and pressure is 1.000atm .

The percent dissociation of Oxygen molecule is 83.00% .

Percentage dissociation is denoted by α ; therefore,

α=83%=83100=0.83

The ICE-table that is initial, change and equilibrium pressure for the equilibrium reaction is written as,

O2(g)2O(g)Initialpressurep0Changeinpressurepα+2pαEquilibriumpressureppα2pα

The equilibrium constant in terms of partial pressure is given as,

Kp=PO2PO2

Where,

• Kp is the equilibrium constant in terms of partial pressure.
• PO is the partial pressure of atomic Oxygen.
• PO2 is the partial pressure of Oxygen molecule.

Substitute the values of partial pressures in the above equation from the ICE table

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