Which of the following changes will cause the reaction to move to the right?

Question

The following system is at equilibrium:
NH4Cl(s) = NH3(g) + HCl(g)

Which of the following changes will cause the reaction to move to the right?

The changes are:

adding NH3
removing NH3
removing NH4Cl
Adding NH4Cl
Adding HCl

Answer 1

Remember that the K expression will only be:

K = [NH3][HCl]

as solids and liquids have no role in the equilibrium expression. So the amount of NH4Cl present has NO effect on the equilibrium. Removing or adding it does not change the reaction.

Adding a product (either NH3 or HCl) will drive the equilibrium to the left. Removing one will drive it to the right.

Answer 2

firstly if u will increase the amount the the reactant i.e. ammonium chloride(NH4Cl) the eqilibrium will shift towads right or u say in the forward dir.
pressure is also a factor
when u increase the pressure of the container in which the reaction is proceding the equilibrium will shift towards the forward reaction(right as u say)
tempreture dependence-
when the reaction is exothermic and tempreture is raised then the equilibrium shifts towards the reverse reaction(left)
if the reaction is endothermic it would go towards the forward reaction
since i am not sure the given reaction is endothermic or exothermic so i wrote both the things.

Answer 3

adding NH4Cl or removing NH3 and/or HCl