The elementary reaction 2H20(g)<--->2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O, H2,...

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The elementary reaction 2H20(g)<--->2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O, H2,...

The elementary reaction 2H20(g)<--->2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O, H2, and O2 reach 0.0700 atm, 0.00200 atm, and 0.00600 atm respectively. What is the value of the equilibrium constant at this temperature?

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Answer 1

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Answer #1

Concepts and reason

The concept used to solve this problem is based on equilibrium constant of a chemical reaction.

The equilibrium constant of a chemical reaction is a constant which describes the value of reaction quotient when the reaction has reached equilibrium.

Fundamentals

The equilibrium constant which depends on partial pressure exerted by gaseous components is represented by. It is known as gaseous equilibrium constant. It is the ratio of partial pressures of product and partial pressures of reactant.

For the reaction,

24,0(8)=2H,(g)+02 (8)

Now, equilibrium constant for this reaction is written as follow.

K, - (P.)( .)

Here is partial pressure of, is partial pressure of and is partial pressure of.

Substitute 0.00600 atm for , 0.00200 atm for and 0.0700 atm for in equilibrium constant formula.

(0.00600)(0.00200)
(0.0700)
= 4.90x106

Ans:

The value of is 4.90x10 .

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Answer 2

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