Le Chatelier's Principle

Le Chatelier's Principle [more detail]

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Carbon disulfide, CS2, and chlorine gas react according to the following exothermic equilibrium reaction:

CS2(g)+3Cl2(g)⇌S2Cl2(g)+CCl4(g)CS_2 (g)+3Cl_2 (g)⇌S_2 Cl_2 (g)+CCl_4 (g)CS2​(g)+3Cl2​(g)⇌S2​Cl2​(g)+CCl4​(g)

If a vessel containing a mixture of these compounds starts at equilibrium and is exposed to a change, which of the following statements is TRUE?

Heating the reaction mixture (at constant pressure) will cause an increase in [CCl4].

Increasing the vessel pressure by adding H2 gas will cause an increase in [CCl4].

Increasing the vessel pressure by compressing the container will cause an increase in [CCl4].

Adding powdered Pt (a catalyst) will cause an increase in [CCl4].

Increasing the vessel pressure by adding S2Cl2 gas will cause an increase in [CCl4].

I don't know

Le Chatelier's Principle

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Le Chatelier's Principle [more detail]