RE: Le Chatelier's principle.
this was the whole question i was given.
Write a short account of around 250 words in total, with reference to Le Chatelier’s principle, in which you explain the following:
(i)
The effect on the equilibrium yield of nitric oxide of increasing the pressure.
(ii)
The effect on the equilibrium yield of nitric oxide of increasing the temperature.
(iii) The effect on the rate of reaction of increasing the temperature.
There is more than one reaction in which nitric oxide,NO, could be a reactant of product. Which reaction is your question about? What is the chemical equation for it?
i. I answered the effect of increasing pressure previously.
N2 + O2 ==> 2NO
Since mole on the left (2) equals moles on the right (2), pressure has no effect on the equilibrium; i.e., the reaction will not shift either direction as the result of increasing or decreasing P.
ii. Here is a site that gives Kp for the reaction at 530 C and a Kp for the reaction at 25 C. From these data you should be able to figure out how the yield will be affected by increasing T.
iii. Since increasing T increases the motion of molecules and that will increase the chances for collisions, the rate of reaction should increase.
That isn't 250 words, but it tells you what is going on. Now put all of that into a nice sounding two pages (about 125 words to a page handwritten) and you will be done.
iii. The effect of increasing T, should provide more energy to the molecules, that
By the way, if the reaction you are studying is different from that which I described previously and above, my pat answers above may change.
Here are some guidelines on equilibria involving gases:
1. Increasing the pressure causes a shift toward the side with the smallest number of gas molecules.
2. Increasing the temperature causes a shift in the direction of the endothermic change. That could be the forward or the reverse reaction. I assume you were told which.
3. Increasing the temperature increases both reaction rates (forward and reverse). The rate increase will be larger for the rate that would help reestablish equilibrium.
To write a short account explaining the effects of pressure and temperature on the equilibrium yield of nitric oxide, as well as the effect of temperature on the rate of reaction, we will need to understand and apply Le Chatelier's principle. Le Chatelier's principle states that when a system at equilibrium is subjected to a stress, the system will shift in a way that minimizes the effect of the stress.
(i) Effect of Increasing Pressure on Equilibrium Yield of Nitric Oxide:
To determine the effect of pressure on the equilibrium yield of nitric oxide, we need to consider the balanced equation for the reaction. Without the equation, it is not feasible to explain the specific reaction. However, generally speaking, if the reaction involves a decrease in the number of moles of gas (i.e., a decrease in volume), increasing the pressure will favor the side with fewer moles of gas. This is because the increased pressure will counteract the stress by shifting the equilibrium towards the direction that reduces the pressure. If the reaction produces more moles of gas, then increasing the pressure will favor the side with more moles of gas.
(ii) Effect of Increasing Temperature on Equilibrium Yield of Nitric Oxide:
When the temperature is increased, Le Chatelier's principle states that the equilibrium will shift in the endothermic direction to absorb the added heat. This means that increasing the temperature will favor the reaction that absorbs heat. If the reaction is exothermic (releases heat), increasing the temperature will shift the equilibrium towards the reactant side to consume the excess heat.
(iii) Effect of Increasing Temperature on the Rate of Reaction:
Increasing the temperature generally increases the rate of a chemical reaction. This happens because higher temperatures provide more energy to reactant particles, leading to increased collision frequency and more successful collisions. According to the collision theory of chemical reactions, the rate of reaction is directly proportional to the number of successful collisions with sufficient energy.
In conclusion, Le Chatelier's principle helps predict the effects of pressure and temperature changes on the equilibrium yield of nitric oxide, as well as the rate of reaction. By understanding the principles behind the theory and having knowledge of the specific reaction, we can analyze and explain how these factors influence the chemical system.