In the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the temperature is i

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Question: In the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the temperature is increased?

Options:

Correct Answer: Shift to the left

Solution:

If the reaction is exothermic, increasing the temperature will shift the equilibrium to the left, favoring the reactants.

In the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the temperature is increased?

In the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the temperature is increased?

Correct Answer: Equilibrium shifts to the left, favoring SO2 and O2.

Step 1: Identify the type of reaction. The given reaction is 2SO2(g) + O2(g) ⇌ 2SO3(g).
Step 2: Determine if the reaction is exothermic or endothermic. An exothermic reaction releases heat.
Step 3: If the reaction is exothermic, increasing the temperature adds heat to the system.
Step 4: According to Le Chatelier's principle, the system will try to counteract the added heat.
Step 5: To counteract the heat, the equilibrium will shift to the left, favoring the reactants (SO2 and O2).
Step 6: Therefore, increasing the temperature will result in more SO2 and O2 being produced.

Le Chatelier's Principle – This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
Exothermic vs. Endothermic Reactions – Understanding whether a reaction releases heat (exothermic) or absorbs heat (endothermic) is crucial for predicting the effect of temperature changes on equilibrium.