In this reaction,
2SO2(g) + O2(g) ⇌ 2SO3(g) + Heat
Increasing the temperature will...
shift equilibrium right
shift equilibrium left
increase pressure
have no effect
Increasing the temperature in this reaction will shift the equilibrium position to the right.
This is because the reaction is exothermic, meaning heat is released in the forward direction. According to Le Chatelier's Principle, increasing the temperature will cause the system to try and counteract this by shifting the reaction to the side that produces heat. Therefore, the equilibrium will shift to favour the products, 2SO3, and the reaction will proceed in the forward direction.
Increasing the temperature in this reaction will shift the equilibrium to the right.
To understand why, we need to consider Le Chatelier's principle. Le Chatelier's principle states that if a system at equilibrium is subjected to a change, it will adjust to minimize the effect of that change and restore equilibrium.
In this reaction, the formation of SO3 is exothermic, meaning it releases heat. By increasing the temperature, we are essentially adding more heat to the system. According to Le Chatelier's principle, the reaction will try to counteract this increase in temperature by moving in the direction that consumes heat.
To consume heat, the reaction needs to produce more SO3 molecules, as 2SO2(g) + O2(g) → 2SO3(g) + Heat is the forward reaction. Therefore, increasing the temperature will shift the equilibrium to the right, favoring the formation of more SO3 molecules.
In summary, increasing the temperature will shift the equilibrium of this reaction to the right.