Question

For each stress, numbered 1,2, 3 on the graph, describe what has occurred and explain why the graph changed the way it did.

Answer 1

https://sites.google.com/site/kwokthechemteacher/Home/kwokthechemteacher/equilibrium/chemical-equilibrium/application-of-lcp/lcp-graphs

Answer 2

\(\color{darkgreen}{~''Hello"}\) @cutepochacco \(\color{darkgreen}{~''Nice~To~Meet~You~!!"}\)

Answer 3

nice to meet you too

Answer 4

I'm stuck on 4 questions not sure how to answer them

Answer 5

Hmm, so what kind of help you need ? Should I explain them to you or You need me to help you with your Ideas ?

Answer 6

I found some answers to this question yet not sure which is correct one.

Answer 7

1) You can see that both concentrations of the products increased at (1) while the reagent NOCl decreased. Le Chatalier's Principle says that if you have a system at equilibrium, and a stress is applied to the system, then the system will react to relieve that stress. If the concentrations of the products increased then that means something happened to left side of the equation (reagents) which we can assume as heat was added to the mixture. The addition of heat puts stress on the balanced system toward the left side of the reaction, so the equilibrium shifts to the right to relieve the stress and produces more products.

2)The accumulation of excess product (due to the above addition of heat) on the right side of the equation will in turn mean that the equilibrium will shift back to the left side of the equation. This is what happens at point 2, as you can see both products peak then decline while the reagent concentration begins to increase.

3)The concentration of Cl2 increased thus the system will gradually decrease NOCL and gradually increase NO and Cl2
____________

OK stress one was adding NO - note how sharp it is compared to the other responses that take a while to respond.


Stress 2 affects all three at once and they ALL go up thus the volume was decreased and they all go up.


____________________________________________________________________________________________________
All these stresses follow Le Chatlier's principle which states that a stress applied on a reaction is relieved by producing and/or consuming the species in the reaction.

1) Heat was added. The resulted in the consumption of NOCl at a rate similar to the production of NO since they both have coefficients of 2. And Cl2 was produced at a slower rate.

2) Most likely the pressure was raised resulting in a decrease in volume.

3) Most likely NO was removed from the reaction resulting in it being replenished.

Answer 8

Alright, lets have a look at them, It looks like you collected from different sources, nvm... so how should i help you?

Answer 9

I need help in knowing which is correct one

Answer 10

I keep going back to my text and websites yet they don't help much

Answer 11

Hmm, well so what does the 1st option from the first part says ?

Answer 12

the first option saying that heat was added and system relieves the system

Answer 13

Exactly, The addition of heat puts stress on the balanced system toward the left side of the reaction, so the equilibrium shifts to the right to relieve the stress and produces more products. with which we can see that both concentrations of the products increased. Its what you find in the graph too.. \(You~are~brave~!\)

Answer 14

is it mean that NO and CI2 was produced due to heat, yet NO produced at a quick rate while CI2 produced at slow rate, NOCI the comsumption (relived)?

Answer 15

For 2: Is it because pressure was increased the volume was decreased?

Answer 16

\(Yeah\), When the equilibrium mixture is heated, more NO and Cl2 are produced. \(!!\)

You type so fast !!

Answer 17

yeah sorry I got use to typing fast. Learned computers when I was 16 now 36. Yet I'm slow compared to secretaries

Answer 18

Lol, \(You~talk~funny~too...~!!\) 2. Exactly as u said happens too !

Answer 19

\(\color{darkgreen}{~''Hello"}\) @cutepochacco ! Hope your doubts are cleared..!! \(\color{darkgreen}{~''ave~A~nice~Day~!"}\)