Which situation would cause the following equilibrium reaction to decrease the formation of the products? 2so2 (g) + o2 (g) two arrows stacked on top of each other. the top arrow points to the right. the bottom arrow points to the left. 2so3 (g) + energy increase the temperature decrease the volume increase the pressure decrease the temperature

 increase the temperature

Explanation: Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

This is a type of Exothermic reaction because heat is released in the reaction.

Option A: Increase the temperature

If the temperature is increased, so according to the Le-Chatlier's principle , the equilibrium will shift in the direction where decrease in temperature occurs. As, this is an exothermic reaction, forward reaction will increase the temperature. Hence, the equilibrium will shift in the left direction, products will decrease.

Option B: Decrease the volume  and Option C: increase in pressure

If the volume of the container is decreased, the pressure will increase according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease in pressure is taking place. As the number of moles of gas molecules is greater at the reactant side. So, the equilibrium will shift in the right direction, products will increase.

Option D: Decrease the temperature

If the temperature is decreased, so according to the Le-Chatlier's principle , the equilibrium will shift in the direction where increase in temperature occurs. As, this is an exothermic reaction, forward reaction will increase the temperature. Hence, the equilibrium will shift in the right direction, products will increase.

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