Practice problem help

[Katherine Grillo 1B]

I was wondering if my answers are correct for this practice problem. Specifically a and c.

The exothermic reaction of carbon disulfide with chlorine is as follows:
CS2 (g) + 3Cl2 (g) ⇋ CCl4 (g) + S2Cl2 (g) delta H = -238 kJ
Predict the effect of the following changes to the system on the direction of equilibrium

a) The pressure on the system is doubled by halving the volume. Rxn goes to the right?
b) The pressure on the system is doubled by pumping in N2. No change?
c) CCl4 is removed as it is generated. Rxn goes to the right?
d) Heat is added to the system. Rxn goes to the left?

[ariana_apopei1K]

I think they're all correct! I was stuck on the one with N2 since it isnt a noble gas, but some places online say that it can be used as an inert gas, so yes there wouldn't be any shift

[Alysa Rallistan 2G]

All your answers are correct, specifically for a) if the volume of the container was halved, the inverse relationship between pressure and volume states that the pressure of the system should then increase by the inverse of 1/2 which is 2; for c) since CCl4 is a product (and the reaction is at equilibrium by the double arrows) then removing it as it is being generated will cause a favor for the reaction to keep making more product, and shift left