Question detail
A reversible reaction reaches equilibrium with the following concentrations: [A] = 0.5 mol/dm3, [B] = 0.2 mol/dm3, [C] = 0.3 mol/dm3. If the concentration of A is decreased to 0.3 mol/dm3, what will happen to the position of equilibrium?
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At a glance
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Topic
Reversible reactions and dynamic equilibrium
Question
A reversible reaction reaches equilibrium with the following concentrations: [A] = 0.5 mol/dm3, [B] = 0.2 mol/dm3, [C] = 0.3 mol/dm3. If the concentration of A is decreased to 0.3 mol/dm3, what will happen to the position of equilibrium?
Answer
The equilibrium will shift towards the reactants to oppose the decrease in concentration of A.
Explanation
This question tests the understandingof Le chatelier's Principle, specifically how a decrease in reactant concentration affects equilibrium position. The answer demonstrates the ability to predict shifts in equilibrium based on concentration changes. This answer is strongest when it stays anchored to The effect of changingconcentration (HT only) and directly addresses (HT only) Predict that decreasingreactant concentration shifts equilibrium towards reactants.
Common mistake
Misunderstanding Equilibrium Shift
Students often think that decreasing reactant concentration will shift the equilibrium towards products instead of reactants.
Remember that according to Le Chatelier's Principle, decreasing the concentration of reactants will shift the equilibrium towards the side that produces more reactants to oppose the change.
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