\( \mathbf{P}(g) + \mathbf{Q}(g) \leftrightarrow 3\mathbf{R}(s) + \mathbf{S}(g) \) ΔH is negative Which of the following will increase the yield of \(\mathb...

The chemical equation provided shows a reaction where reactants P and Q form products R and S, and the reaction is exothermic (ΔH is negative). The question asks which of the given options will increase the yield of R. , using a larger closed vessel, will not affect the yield of R because the reaction vessel size does not have an effect on the amount of product formed. , increasing the temperature, will favor the reverse reaction and decrease the yield of R, as the reaction is exothermic. Therefore, this option is incorrect. , removing some S, will drive the reaction towards the product side, according to Le Chatelier's principle. As a result, the yield of R will increase. Therefore, this option is correct. , adding a positive catalyst, will not change the position of the equilibrium or the yield of R because the reaction is not mentioned as being a reversible reaction. Therefore, this option is incorrect. In conclusion, the correct option that will increase the yield of R is removing some S.