Question detail
A chemical reaction at equilibrium has a concentration of reactants at 0.5 mol/dm3 and products at 0.2 mol/dm3. If the concentration of the reactants is increased to 0.8 mol/dm3, what will happen to the equilibrium position?
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At a glance
Question
Type
exam_style
Style
Topic
Reversible reactions and dynamic equilibrium
Question
A chemical reaction at equilibrium has a concentration of reactants at 0.5 mol/dm3 and products at 0.2 mol/dm3. If the concentration of the reactants is increased to 0.8 mol/dm3, what will happen to the equilibrium position?
Answer
The equilibrium will shift to the right, towards the products, as the concentration of reactants increases.
Explanation
This question evaluates the ability to interpret concentration changes in equilibrium systems. It requires understandingof how changes in reactant concentration affect the equilibrium position accordingto Le chatelier's Principle. This answer is strongest when it stays anchored to The effect of changingconcentration (HT only) and directly addresses (HT only) Interpret concentration changes in industrial equilibrium examples.
Common mistake
Misinterpreting Concentration Changes
Students often confuse the effect of increasing reactant concentration with decreasing product concentration, thinking both will shift equilibrium towards products.
Remember that increasing reactant concentration shifts equilibrium towards products, while increasing product concentration shifts equilibrium towards reactants.
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