a) Why does adding gaseous/aqueous reactant cause a reaction to shift right? Justify using Q and K

b) Why does removing a gaseous/aqueous reactant cause a reaction to shift right? Justify using Q and K

c) Name 2 things that DO NOT shift a reaction's equilibrium position
==> Catalyst, inert gas  {is this correct}

d) 3 ways to increase amount of products present in equilibrium for
Endothermic reaction ===> Increase Temp, Increase Products, Decrease Reactants.{is this correct?}

e) why does increase in temperature on the reaction in (d) cause the reaction to shift the way it does? Justify using Q vs K
==> Increase in temperature will result in increase of products and decrease reactants and Reaction moves forward.
So Q becomes less than K?{ want to know more clarification on this Q<K part}

These questions are based on Le Chatelier's Principle - If some changes are done on any equilibrium system, then system will shift to nullify the change.
A(s) + B(g) +    H₂O(l) <-----> C (aq) + Heat
Now in the above system A(s) and H₂O(l) are not the part of equilibrium expression as they are considered as pure with unit concentrations.
K =  [C] /
If we add more B then Q < K so equilibrium will shift to give more product so that Q = K
If we add more of C then Q >K and equilibrium shifts in the direction of the reactants. Same effects can be observed  if they are removed from the system.
If we raise the temperature of the above system ,it means more heat is formed so system will shift in the direction of less heat.