What is Le Chaˆ\^{a}telier's principle? Consider the reaction 2NOCl(g)2NO(g)+2 \mathrm{NOCl}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+ Cl2( g)\mathrm{Cl}_2(\mathrm{~g}). If this reaction is at equilibrium, what happens when the following changes occur?

For this change, what happens to the value of KK for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position.

NOCl(g)\mathrm{NOCl}(\mathrm{g}) is added.

In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?


Answered 8 months ago
Answered 8 months ago
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In this task, we need to explain how does adding NOCl to the system changes the equilibrium using Le Chatelier's principle.

Le Chatelier's principle states that for any change that happens to the system in equilibrium, the position of the equilibrium changes in a way to reduce this change.

These changes are: change in pressure/volume, change in temperature, and change in the concentration of reactants or products.

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