Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 500. mL flask with 3.7 atm of sulfur dioxide gas and 2.3 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 2.2 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits.

The pressure equilibrium constant  is  

Explanation:

From the question we are told that

    The volume of the flask is  

    The pressure of sulfur dioxide is    

     The pressure of  oxygen gas

     The pressure of sulfur trioxide at equilibrium is

The chemical equation for this reaction is

             ⇄  

The partial pressure of  oxygen at  equilibrium is mathematically evaluated as

Substituting values

The partial pressure of  sulfur dioxide  at  equilibrium is mathematically evaluated as

Substituting values

From the chemical equation  pressure constant is mathematically represented as

Substituting values

the answer is:  

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