For the equilibrium reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the temperature is de

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Question: For the equilibrium reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the temperature is decreased, what will be the effect?

Options:

Correct Answer: Shift to the right

Solution:

Decreasing the temperature for an exothermic reaction will shift the equilibrium to the right, favoring the formation of products.

For the equilibrium reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the temperature is decreased, what will be the effect?

For the equilibrium reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the temperature is decreased, what will be the effect?

Step 1: Identify the reaction type. The reaction CO(g) + 2H2(g) ⇌ CH3OH(g) is an exothermic reaction, meaning it releases heat.
Step 2: Understand 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 3: Recognize the disturbance. In this case, the disturbance is a decrease in temperature.
Step 4: Determine the effect of decreasing temperature. Since the reaction is exothermic, decreasing the temperature will favor the side that produces heat, which is the product side (CH3OH).
Step 5: Conclude the effect. Therefore, decreasing the temperature will shift the equilibrium to the right, favoring the formation of CH3OH.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in temperature, pressure, or concentration, the system will adjust to counteract that change and restore a new equilibrium.
Exothermic vs. Endothermic Reactions – Understanding the difference between exothermic reactions (which release heat) and endothermic reactions (which absorb heat) is crucial for predicting the effects of temperature changes on equilibrium.