Which of the following changes would cause the reaction below to shift in the forward direction to reestablish equilibrium? 2 NBr. (g) = N₂ (g) + 3 Br₂ (g) A) adding a catalyst. B) adding Ar (g). C) increasing the total volume of the container. D) adding N₂.

I need help with this question and I know it has three parts but it counts as one question.

Decide whether each of the following statements is true or false.  If false, change the wording of the statement to make it true.   a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction.  d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.

Hydrogen fluoride is produced by reacting hydrogen with fluorine according to the following equation H₂ (g) + F2 (g) → 2 HF (g) Please use the following information to answer the next question. A stress that would shift the equilibrium towards the products would be to O add HF(g) O remove H₂(g) O decrease the volume of the reaction vessel O decrease the temperature of the reaction vessel AH = -542.2 kJ