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Sulfur dioxide and oxygen react to form sulfur trioxide, like this: (g) (g) (g) Also, a chemist finds that at a certain temperature the equilibrium mixture of sulfur dioxide, oxygen, and sulfur trioxide has the following composition: compound pressure at equilibrium Calculate the value of the equilibrium constant for this reaction. Round your answer to significant digits.

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Answer:

[tex]Kp=9.2x10^{-3}[/tex]

Explanation:

Hello!

In this case, for the undergoing chemical reaction at equilibrium:

[tex]2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g)[/tex]

Which means that pressure-based equilibrium constant is computed via the following equilibrium expression:

[tex]Kp=\frac{p_{SO_3}^2}{p_{SO_2}^2p_{O_2}}[/tex]

Thus, by plugging in the given pressures at equilibrium, the required Kp turns out:

[tex]Kp=\frac{55.0^2}{70.2^2*66.7}\\\\Kp=9.2x10^{-3}[/tex]

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