The effect of concentration

For the following equilibrium in solution:

State what will happen to the position of equilibrium if more B is added to the mixture.

The following reversible reaction is at equilibrium in a closed container:

A chemist removes some G(g) from the equilibrium mixture.

A system is at equilibrium with the following reaction:

At equilibrium, the concentration of Z is 4.0 mol/dm^3. If 2.0 mol/dm^3 of Z is suddenly removed, how many moles per dm^3 of Z will form to restore equilibrium? Assume all change is due to the forward reaction.

The following reaction is at equilibrium in a sealed container:

Explain, in terms of concentration, what will happen to the position of equilibrium if extra KL(g) is added.

The equilibrium below is set up in a sealed vessel:

The graph shows how the concentration of AB(g) changes after some B2(g) is added:

The equilibrium below is reached in a closed vessel:

State what happens to the position of equilibrium if some HI(g) is removed.

Methanol (3e{CH3OH}) is produced in industry by the following equilibrium:

A technician increases the concentration of hydrogen gas (62e{H2}).

The reaction below is at equilibrium:

At equilibrium, [Q] is 3.0 mol/dm^3 and [P] is 1.0 mol/dm^3. If 0.5 mol/dm^3 of Q is removed, what will [Q] be after the change is compensated and equilibrium is restored? Assume the system restores [Q] to the original value.

Consider the equilibrium: A sealed vessel contains 0.20 mol of X and 0.15 mol of Y at equilibrium. If 0.10 mol of Y is removed from the vessel, predict the change in the amount of X at equilibrium. Explain your answer with a calculation showing the direction of shift.

In a laboratory, the following reversible reaction is at equilibrium: Explain, in terms of the effect of concentration, how the equilibrium position can be shifted to increase the amount of R(g) produced. Include why each change has this effect.