For each event stated below, indicate how the concentration of each species in the chemical equation then change to reach equilibrium. Click in the blue box below to toggle the relative change in concentration (up=increases, down=decreases leave the box blank for no change). 2CO(g)+O2(g) 2CO2 (g) increasing the concentration of CO increasing the concentration of CO2 decreasing the the volume of the system

Answers are in the explanation

Explanation:

It is possible to know the effect of change the conditions in an equilibirum based on LeChatelier's principle that says any change in conditions of a chemical system produce in the system an opposite response to counteract the initial change.

For the reaction:

2CO(g) + O₂(g) ⇄ 2CO₂(g)

Increasing the concentration of CO: The system will response producing more CO₂ counteracting the increasing of CO. CO concentration decreases, O₂ concentration decreases, CO₂ concentration increases

Increasing the concentration of CO₂: Here, the system response producing more CO and O₂ decreasing the concentration of CO₂

Decreasing the volume of the system: Here, the system will try to go in the direction that occupy less volume to counteract the increase of pressure because of decreasing of volume. In the left of the reaction there are three moles of gas and in the right there are just two. That means the system will produce more CO₂ decreasing, thus, concentration of CO and O₂.

I hope it helps!

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