Reverse reactions and Le Chateliers principle

In summary, in acid-base reactions, the reaction does not go 100% toward the product and a reverse reaction occurs, reaching equilibrium. In industrial processes, the reaction mixture is sent to a separation equipment to purify the products and recycle the reactants. This can be done through methods such as distillation, precipitation, or removal to shift the equilibrium. Equilibrium stability can be affected by concentration, temperature, and pressure-volume effects, which can be visualized through the "seesaw analysis" method.
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Yield in acid-base reaction low due to reverse reaction
In acid-base reactions, the reaction never goes 100% toward the product, right? A reverse reaction will occur and eventually reaction toward product and reactant will reach equilibrium. In lab/industry conditions where yield is important, how does they push the reaction toward product? I am guessing this is where Le Chatelier's principle may come in handy but I am having a hard time seeing it.
 
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  • #2
In industrial processes, if the reaction does not go to completion in the reactor, the reaction mixture next goes to a piece of separation equipment (like a distillation column) where the products and reactants are purified, and the reactants are recycled to the reactor to be combined with new reactants, while the products experience subsequent processing. This applies to both batch processes and continuous flow processes.
 
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You can distill/remove/precipitate (whichever works best for a given reaction) the product out to shift the equilibrium.
 
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... but I am having a hard time seeing it.

Generally, equilibrium stability is affected by one, two or a combination of three factors. These are concentration effects, temperature affects & pressure-volume effects. One way that is used to visualize the effect of concentration and/or temperature effects is the 'seesaw analysis'. Pressure-Volume effect follows after concentration & temperature effects.
Consider the following hypothetical reaction (A + B <=> C + D) and assume while at equilibrium it is balanced on a seesaw...

Concentration Effects can be perceived as follows ...
Le Chateliers Principle - Concentration Effects_0001.jpg

Le Chateliers Principle - Temp Effects_0001.jpg

Le Chateliers Principle - Press-Vol Effects.jpg


 
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1. What is a reverse reaction?

A reverse reaction is a chemical reaction that occurs in the opposite direction of the forward reaction. It is also known as a backward reaction or a reverse process.

2. How does Le Chatelier's principle relate to reverse reactions?

Le Chatelier's principle states that when a system at equilibrium is subjected to a change, the system will shift in a way that minimizes the effect of the change. In the case of reverse reactions, this means that if the reverse reaction is exothermic, an increase in temperature will shift the equilibrium towards the reactants, while a decrease in temperature will shift it towards the products.

3. What factors can affect the rate of a reverse reaction?

The rate of a reverse reaction can be affected by factors such as temperature, concentration of reactants and products, and the presence of a catalyst. Changes in these factors can shift the equilibrium towards the reactants or products, ultimately affecting the rate of the reverse reaction.

4. Can a reverse reaction reach equilibrium?

Yes, a reverse reaction can reach equilibrium just like a forward reaction. At equilibrium, the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant.

5. How is the equilibrium constant affected by a reverse reaction?

The equilibrium constant, represented by K, is a measure of the extent to which a reaction proceeds towards products. In a reverse reaction, the equilibrium constant will have a different value than in the forward reaction, but it will still represent the ratio of products to reactants at equilibrium.

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