For the balanced reaction 2SO_2(g) + O_2(g) r | vedclass

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(D) The given reaction is an exothermic reaction: $2SO_2(g) + O_2(g) ightleftharpoons 2SO_3(g) + 	ext{Heat}$.According to Le Chatelier's principle,

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Adding oxygen

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(D) The given reaction is an exothermic reaction: $2SO_2(g) + O_2(g) ightleftharpoons 2SO_3(g) + 	ext{Heat}$.According to Le Chatelier's principle,for an exothermic reaction,decreasing the temperature favors the forward reaction.Additionally,increasing the concentration of reactants (like $O_2$ or $SO_2$) or decreasing the concentration of products (like $SO_3$) shifts the equilibrium in the forward direction.Among the given options,adding oxygen $(O_2)$ increases the concentration of reactants,which shifts the equilibrium to the right (forward direction).

For the balanced reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) + \text{Heat}$,which of the following conditions will favor the forward reaction?

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