Equilibrium Problems (Help!)?

NetherCraft 0

Consider the following system at Equilibrium.

2CO(g) + O2(g) <—> 2CO2(g)

1) How will increasing the concentration of CO shift the equilibrium?

a)to the right b)to the left c)no effect

2) How will increasing the concentration of CO2 shift the equilibrium?

a)to the right b)to the left c)no effect

3) How will adding a catalyst shift the equilibrium?

a)to the right b)to the left c)no effect

7 Answers

  • 1. You will increase the net pressure of CO, shifting the equilibrium to the right, making more products.

    1. To the left, making reactants.

    2. No change- Catalysts help reach the equilibrium fast. Since the system is already in equilibrium, adding a catalyst will not shift the reaction anywhere.

    Source(s): Science student.
  • 1) right, because adding more CO will give more reactants which then in turn to bring it back to equilibrium it must favor the products (the right) to make more products to equal it out after you added some to the reactant side.

    2) left, same thing as above but opposite, you added to the products so the reaction must favor the reactants(the left) in order to make more reactants to account for the products you added.

    3) no effect, the reaction is already at equilibrium, so there is no point and no need for a catalyst, it will do nothing at this point because “the job is already complete and it showed up late”

    Source(s): AP Chemistry Student
  • I got 3 wrong. For 3 it could go to the right

  • Decreasing the volume shifts equilibrium to the side with less moles. Increasing the volume shifts equilibrium to the side with more moles.

  • number 3 is to the right

  • I dont know the answer but i do know that number 3 is not “no effect”

  • a) right

    b) left

    c) right

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