What was Le Chatelier's principle on
the effect on the equilibrium yield of nitric oxide of increasing the pressure and
The effect on the equilibrium yield of nitric oxide of increasing the tempreture
it depends on the reaction, can you type the reaction equation?
for the Le Chatelier's principle you need to know the whole reaction, not just the product
Le Chatelier's principle states that when a system in equilibrium is subjected to a change, it will react in a way that opposes the change in order to restore equilibrium.
In the case of the effect of increasing pressure on the equilibrium yield of nitric oxide:
1. Understand the chemical equation: For the reaction in question, you need to know the balanced chemical equation that represents the formation of nitric oxide. Let's assume the reaction is as follows:
N2(g) + O2(g) ⇌ 2NO(g)
2. Consider the impact of pressure: Increasing the pressure in a reaction system affects the equilibrium position if there is a different number of moles of gases on both sides of the reaction. From the balanced chemical equation, we see that there are fewer moles of gases on the right side (2 moles of NO) compared to the left side (1 mole of N2 and 1 mole of O2).
3. Predict the effect: According to Le Chatelier's principle, increasing the pressure would cause the system to shift in the direction that reduces the total number of moles of gas. In this case, it means the system will shift towards the side with fewer moles of gas, which is the left side. Hence, increasing the pressure would increase the yield of nitric oxide.
Regarding the effect of increasing temperature on the equilibrium yield of nitric oxide:
1. Analyze the chemical equation: Assuming the reaction equation is the same as before:
N2(g) + O2(g) ⇌ 2NO(g)
2. Assess the impact of temperature: The effect of temperature on an equilibrium reaction depends on whether the reaction is exothermic (releases heat) or endothermic (absorbs heat). Without specific information, we cannot determine the exact nature of the reaction.
3. Predict the effect: For an exothermic reaction, increasing the temperature would shift the equilibrium position in the direction that absorbs heat. Conversely, for an endothermic reaction, increasing the temperature would shift the equilibrium in the direction that releases heat. Depending on the nature of the reaction, the yield of nitric oxide could either increase or decrease when the temperature is raised.
To fully answer the question, we would need to know whether the reaction is exothermic or endothermic.
For NO, the equation probably is
N2 + O2 ==> 2NO
There are two mols gases on the left and 2 mols on the right; therefore, changing the pressure will not change the equilibrium. I need more information before answering the part about temperature.