How is La Chatelier's principle useful in the chemistry industry? What is the effect of temperature on the equilibrium constant?

Question

How is La Chatelier's principle useful in the chemistry industry?  What is the effect of temperature on the equilibrium constant?

Luna Chen · Accepted Answer

Consider dinitrogen fixation.........

#1/2N_2(g) + 3/2H_2(g) stackrel("catalysis")rightleftharpoons NH_3(g) +Delta# This is probably the most important chemical reaction on the planet. Without such a process, there would be NO nitrogenous fertilizer with which to grow food.......The problem with this reaction is that we have to overcome very strong #N-=N# and #H-H# bonds, and catalysis, usually closely guarded industrial secrets, can enable some small yield of #NH_3(g)#. Now the only thing this reaction has got going for it is that the product gas, #NH_3(g)#, is CONDENSABLE, while the reactant gases, are relatively incondensable. And we could use Le Chatelier's principle to exploit these properties. And thus if we use a cold finger to CONDENSE the ammonia, the liquid ammonia is removed from the equilibrium, and the equilibrium re-establishes itself by moving to the right as we face the page.........Good turnovers of product can be achieved thereby. Does Le Chatelier's principle apply with respect to this aspect of the reaction? And note with regard to the given reaction, the exothermic nature of the reaction would suggest that lower temperatures would be favourable. Unfortunately, at these lower temperatures, the reaction would have an unacceptably low rate. Modern processes trade off the temperature with acceptable yields, and are able to achieve high turnovers.

Avery Adams · Answer

undefined La Chatelier's principle is useful in the chemistry industry because it helps predict how changes in conditions, such as temperature, pressure, or concentration, will affect chemical reactions, allowing for optimization of reaction conditions and product yields.

The effect of temperature on the equilibrium constant depends on whether the reaction is exothermic or endothermic. Generally, increasing temperature shifts the equilibrium position in the direction that absorbs heat, while decreasing temperature shifts it in the direction that releases heat.

Cooper Adams · Answer

undefined Le Chatelier's principle is useful in the chemistry industry because it helps predict and understand how chemical systems respond to changes in conditions such as temperature, pressure, or concentration. By applying this principle, chemists can manipulate conditions to favor the desired reaction or product yield. In industrial processes, this knowledge is crucial for optimizing production efficiency and reducing costs.

Regarding the effect of temperature on the equilibrium constant ($K$), it depends on whether the reaction is exothermic or endothermic. For an exothermic reaction (where heat is released), increasing the temperature will shift the equilibrium towards the reactants to counteract the temperature increase. Conversely, for an endothermic reaction (where heat is absorbed), increasing the temperature will shift the equilibrium towards the products. Therefore, the effect of temperature on the equilibrium constant depends on the specific reaction and its enthalpy change.