What was Le Chatelier’s principle, in The effect on the equilibrium yield of nitric oxide of increasing the pressure?
That will depend upon the reaction that is producing NO. If the number of moles increases in that reaction, increasing the pressure will favor the reaction direction that decreases the number of moles.
I suggest
Le Chatelier's principle states that when a system at equilibrium is subjected to a change in temperature, pressure, or concentration of reactants or products, the system will shift in a direction that minimizes the effect of the change.
When it comes to the effect on the equilibrium yield of nitric oxide (NO) by increasing the pressure, Le Chatelier's principle predicts that the system will shift to oppose the increase in pressure.
In the case of the reaction for the production of nitric oxide:
N₂(g) + O₂(g) ⇌ 2NO(g)
By increasing the pressure (perhaps by compressing the system), Le Chatelier's principle suggests that the equilibrium will shift in the direction that reduces the pressure. The reaction will produce more NO in order to decrease the overall pressure, as there are fewer gas molecules on the product side.
Therefore, increasing the pressure will favor the formation of nitric oxide.
Le Chatelier's principle states that when a system at equilibrium is subjected to a change in temperature, pressure, or concentration, the system will adjust to counteract the effect of that change and maintain equilibrium.
To understand the effect of increasing pressure on the equilibrium yield of nitric oxide, you can apply Le Chatelier's principle and analyze the reaction involved. Assuming we have a reaction where nitrogen gas reacts with oxygen gas to form nitric oxide gas:
N2(g) + O2(g) ⇌ 2NO(g)
Increasing the pressure means increasing the concentration of the gases. In this case, an increase in pressure results from either adding more reactants or reducing the volume of the container.
According to Le Chatelier's principle, when the pressure increases, the system will shift in a way that reduces the total number of moles of gas. Since 2 moles of reactant gas (N2 and O2) produce only 2 moles of product gas (NO), the system will not favor either the reactants or the products as the number of gas molecules remains constant.
Therefore, increasing the pressure will not have a significant effect on the equilibrium yield of nitric oxide. Instead, the system will adjust to counteract the pressure change by redistributing the various species in a way that maintains equilibrium.