Consider the following equation:2 SO_{2(g)} + | vedclass

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(D) The given reaction is $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ with $\Delta H = -190 \ kJ$.$1$. Increasing temperature: Since the r

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$3$

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(D) The given reaction is $2 SO_{2(g)} + O_{2(g)} ightleftharpoons 2 SO_{3(g)}$ with $\Delta H = -190 \ kJ$.$1$. Increasing temperature: Since the reaction is exothermic $(\Delta H $2$. Increasing pressure: The reaction involves a decrease in the number of moles of gas $(3 	ext{ moles of reactants} ightarrow 2 	ext{ moles of products})$. According to Le Chatelier's principle,increasing pressure shifts the equilibrium to the right,increasing the yield of $SO_3$.$3$. Adding more $SO_2$ or $O_2$: Increasing the concentration of reactants shifts the equilibrium to the right,increasing the yield of $SO_3$.$4$. Addition of catalyst: $A$ catalyst only increases the rate of reaction and does not change the position of equilibrium or the yield of products.Therefore,the factors that increase the yield are $B, C,$ and $D$. The total number of such factors is $3$.

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