For the reaction 4H2(g) + 2O2(g) ⇌ 4H2O(g), what is the effect of increasing the

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Question: For the reaction 4H2(g) + 2O2(g) ⇌ 4H2O(g), what is the effect of increasing the temperature?

Options:

Correct Answer: Shift to the left

Solution:

Increasing the temperature of an exothermic reaction shifts the equilibrium to the left, favoring the reactants.

For the reaction 4H2(g) + 2O2(g) ⇌ 4H2O(g), what is the effect of increasing the temperature?

For the reaction 4H2(g) + 2O2(g) ⇌ 4H2O(g), what is the effect of increasing the temperature?

Step 1: Identify the type of reaction. The given reaction is 4H2(g) + 2O2(g) ⇌ 4H2O(g). This reaction is exothermic, meaning it releases heat.
Step 2: Understand what happens when temperature increases. In an exothermic reaction, increasing the temperature adds heat to the system.
Step 3: Apply Le Chatelier's Principle. This principle states that if a system at equilibrium is disturbed, it will shift in a direction that counteracts the disturbance.
Step 4: Determine the direction of the shift. Since we added heat by increasing the temperature, the equilibrium will shift to the left to absorb the excess heat.
Step 5: Conclude the effect of increasing temperature. The shift to the left favors the reactants (H2 and O2) over the products (H2O).

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 Reactions – In exothermic reactions, heat is released, and increasing temperature can shift the equilibrium towards the reactants.