For each event stated below, indicate how the concentration of each species in t

Question

For each event stated below, indicate how the concentration of each species in the chemical equation will then change to reach equilibrium. Click in each empty space below to toggle the relative change in concentration (up=increases, down=decreases, leave the box blank for no change).

2CO(g) + O2(g) reverse sign 2CO2(g)

a.) increasing the concentration of CO        ________            __________                      _______________

b) increasing the concentration of CO2     ____________      __________                     ___________

c) decreasing the the volume of the system __________        __________                    ____________

Explanation / Answer

More correctly, your equation should be this:

2CO + O2 <---> 2CO2

because it is an equilibrium reaction, it can go both ways.

When something on the left side is increased, it throws off the equilibrium. There is too much on the left side. In order to reestablish equilibrium the left side needs to decrease and the right side needs to increase.

A) When CO is increased (note it is on the left side)
2CO will then decrease (since it's on the left)
O2 will then decrease (it's on the left)
2CO2 will then increase (it's on the right)

B) When CO2 is increased. It's on the right side, so the opposite effects will occur as in part A

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