Question

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2SO3(g) -> 2SO2(g)+O2(g)
Calculate Keq for this reaction if the equalibrium concentrations are: |SO2|=0.42M; |O2|=0.21M; |SO3|=0.072M
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Answer 1

The equilibrium constant for the reaction comes out to be 7.145

Step-by-step explanation:

Given concentration of all the species at equilibrium are shown below

`\left [ SO_(2) \right ] = 0.42 \textrm{ M}, \left [ O_(2) \right ] = 0.21 \textrm{ M}, \left [ SO_(3) \right ] = 0.072 \textrm{ M}` \\

Given reaction is shown below

`2\textrm{SO}_(3)\left ( g \right )\rightleftharpoons 2\textrm{SO}_(2)\left ( g \right )+\textrm{O}_(2)\left ( g \right )`

`K_(eq) = \displaystyle (\left [ SO_(2) \right ]^(2)* \left [ O_(2) \right ])/(\left [ SO_(3) \right ]^(2)) \\K_(eq) = \displaystyle (\left ( 0.42 \right )^(2)* 0.21)/(\left ( 0.072 \right )^(2)) \\K_(eq) = 7.145`

`K_(eq)` for the reaction is 7.145