Question

The following system is at equilibrium:

3M(g)+N(s)⇌2L(g)
Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction.
Drag the appropriate items to their respective bins: (Leftward shift, Rightward Shift, No Shift).
1) Add more N
2) Remove some N
3) Increase the volume
4) Decrease the volume

Answer 1

1) No shift

2) No shift

3) Leftward shift

4)Rightward sifht

Step-by-step explanation:

1) 2) Adding N or Removing N in the equilibrium will produce No shift, because of its solid state, the N is not contemplated in the equilibrium equation:

`K=([L]^2)/([M]^3)`

3) Increasing the volume produces a decrase in the preassure due to the expansion of the gases. This will cause a leftward shift, because the system will try to increase the moles of gas and in consecuence of this, also increase the preassure.

4) Decreasing the volume has the opposite effect of the item 3): the preassure will increase and the system will consume moles of gas to decrease it, producing a rightward shift.