QuestionWhat happens to the equilibrium when a 7.0 L container is reduced to 2.5 L for the reaction:
?
A. No change. B. Shift left. C. Shift right.
Studdy Solution
STEP 1
Assumptions1. The system is at equilibrium in a7.0 L container.
. The reaction is reversible and exothermic as indicated by the arrow and the release of energy (198 kJ).
3. The container is shrunk to.5 L, which means the volume is decreased.
4. We are assuming ideal gas behavior.
STEP 2
We need to identify the number of moles of gas on each side of the reaction.On the left side (reactants), we haveOn the right side (products), we have
STEP 3
Now, we need to understand the effect of decreasing the volume on the system at equilibrium. According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in pressure, volume or temperature, the system will adjust itself to counteract the effect of the change.
Decreasing the volume of the system increases the pressure. The system will respond by shifting the equilibrium to the side with fewer moles of gas to decrease the pressure.
STEP 4
Compare the number of moles of gas on each side of the reaction.
We have3 moles of gas on the reactant side and2 moles of gas on the product side.
STEP 5
Since the product side has fewer moles of gas, the reaction will shift to the right (towards the products) to counteract the increase in pressure caused by the decrease in volume.
So, the correct answer isC. The reactions shifts to the right (products) to produce fewer moles of gas.
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