Answered: The elementary reaction…

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter8: Reaction Rates And Equilibrium

Section: Chapter Questions

Problem 8.76E

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Question

The elementary reaction

2H2O(g)↽−−⇀2H2(g)+O2(g)2H2O(g)↽−−⇀2H2(g)+O2(g)

proceeds at a certain temperature until the partial pressures of H2O,H2O, H2,H2, and O2O2 reach 0.0900 atm,0.0900 atm, 0.00250 atm,0.00250 atm, and 0.00650 atm,0.00650 atm, respectively. What is the value of the equilibrium constant at this temperature?

Expert Solution

Step 1

The equilibrium reaction is as follows:

$2 H_{2} O (g) ⇋ 2 H_{2} (g) + O_{2} (g)$

The partial pressure of $H_{2} O$ at equilibrium = 0.0900 atm

The partial pressure of $H_{2}$ at equilibrium= 0.00250 atm

The partial pressure of $O_{2}$ at equilibrium= 0.00650 atm

The equilibrium constant for the reaction is written as follows:

$K_{p} = \frac{{(P_{H_{2}})}^{2} \times P_{O_{2}}}{{(P_{H_{2} O})}^{2}}$

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