Question detail
In a closed system, the concentration of reactants in a reversible reaction is increased. Explain how this change affects the position of equilibrium and predict the direction of the shift.
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At a glance
Question
Type
exam_style
Style
Topic
Reversible reactions and dynamic equilibrium
Question
In a closed system, the concentration of reactants in a reversible reaction is increased. Explain how this change affects the position of equilibrium and predict the direction of the shift.
Answer
Accordingto Le chatelier's Principle, increasingthe concentration of reactants will shift the equilibrium position towards the products to counteract the change. This results in a higher yield of products.
Explanation
This question tests the understandingof Le chatelier's Principle and its application to concentration changes in equilibrium systems. It assesses the ability to predict the direction of equilibrium shifts based on changes in concentration. 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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