Reversible Reactions And Equilibria
Visão Geral
Not every chemical reaction runs to completion. Some reactions can go forward and backward at the same time, reaching a state of balance where both reactants and products coexist. Controlling this balance is the key to industrial processes like ammonia production.
In this lesson you will learn what makes a reaction reversible, how dynamic equilibrium is established in a sealed system, and how changing temperature or pressure shifts the position of equilibrium. You will also see why a catalyst speeds up both directions equally without changing the final balance.
Objetivos
- 3.18 know that some reactions are reversible and this is indicated by the symbol ⇌ in equations describe reversible reactions such as the dehydration of hydrated copper(II) sulfate and the effect of heat on ammonium chloride
- know that a reversible reaction can reach dynamic equilibrium in a sealed container
- know that the characteristics of a reaction at dynamic equilibrium are: - the forward and reverse reactions occur at the same rate - the concentrations of reactants and products remain constant.
- understand why a catalyst does not affect the position of equilibrium in a reversible reaction
- know the effect of changing either temperature or pressure on the position of equilibrium in a reversible reaction: - an increase (or decrease) in temperature shifts the position of equilibrium in the direction of the endothermic (or exothermic) reaction - an increase (or decrease) in pressure shifts the position of equilibrium in the direction that produces fewer (or more) moles of gas References to Le Chatelier's principle are not required
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- Dynamic equilibrium can only be established in: A) An open container B) A sealed container C) A vacuum D) A heated container Answer: B
- At dynamic equilibrium: A) All reactions have stopped B) The concentrations of reactants and products are equal C) The forward and reverse reactions occur at the same rate D) Only the forward reaction occurs Answer: C
- Increasing temperature shifts equilibrium towards: A) The exothermic direction B) The endothermic direction C) The side with more moles of gas D) The catalyst Answer: B
- A catalyst affects equilibrium by: A) Shifting it to the right B) Shifting it to the left C) Not changing the position but reaching it faster D) Increasing the yield of product Answer: C
- In the reaction N2(g) + 3H2(g) = 2NH3(g), increasing pressure shifts equilibrium to the: A) Left (more moles of gas) B) Right (fewer moles of gas) C) No change D) Cannot be predicted Answer: B
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