[cuckoo99]

(Original post by gmseahorse)
There is a bit in the syllabus on why they affect things, some limited stuff about more collisions or something, I would love to know in a bit more depth though.

ok i'll enlighten you then with my AS knowledge hahaha An equilibrium is made up of a forward and backward reactions that produce reactants and products at the same rate and the concentrations of these reactants and products remains constant. This is called a dynamic equilibrium. if the forward reaction is ENDOTHERMIC and the temperature is increased, the system will shift to the right and produce a higher yield of the species on the right. This is due a thing called Le Chateliers principle- If their is a disturbance in the system, the system will shift in the direction that tends to reduce the disturbance.

Now back to increasing temperature. if the forward reaction is endothermic (endothermic meaning more energy is taken in than given out when bonds are formed.) Then the system will shift to the side that is producing products endothermicaly so if the forward reaction is endothermic the equilibrium will shift to the right. This will reduce the temperature(Disturbance) of the system. Now using that knowledge you can deduce what will happen if you decrease the temperature. Decreasing the temperature would make the system take the exothermic route.


When it comes to pressure, an increase in pressure will course the equilibrium to shift to the side that has the fewest moles of gas, This is an attempt to reduce the pressure of the system as. i could go on for more but im kinda tirred so ye ;p

hope this helps your understanding of what AS chemistry has to offer

*starts doing A2 work*

[sherbetlily]

I am screwed for this exam, realising how little I actually know and understand my teacher is deaf so has speech problems and we just never learnt anything
Could someone please go over the equations we need to know?
thanks!

[No brainer1]

Can someone upload the january 2012 c4 c5 c6 higher tier chemistry gcse paper
When you have could you quote me thanks a million

[gideongaspard]

what did you guys get last year I got 100 ums in chem and physics?

[gideongaspard]

(Original post by cmab52)
I got an A* 100% - quite chuffed lol My teacher kept nagging everyone - YOU GOT TO GET FULL MARKS i was like "no waaaay" turns out I did.

I did too and physics as well nearly biology but only got 98

[gmseahorse]

(Original post by cuckoo99)
ok i'll enlighten you then with my AS knowledge hahaha An equilibrium is made up of a forward and backward reactions that produce reactants and products at the same rate and the concentrations of these reactants and products remains constant. This is called a dynamic equilibrium. if the forward reaction is ENDOTHERMIC and the temperature is increased, the system will shift to the right and produce a higher yield of the species on the right. This is due a thing called Le Chateliers principle- If their is a disturbance in the system, the system will shift in the direction that tends to reduce the disturbance.

Now back to increasing temperature. if the forward reaction is endothermic (endothermic meaning more energy is taken in than given out when bonds are formed.) Then the system will shift to the side that is producing products endothermicaly so if the forward reaction is endothermic the equilibrium will shift to the right. This will reduce the temperature(Disturbance) of the system. Now using that knowledge you can deduce what will happen if you decrease the temperature. Decreasing the temperature would make the system take the exothermic route.


When it comes to pressure, an increase in pressure will course the equilibrium to shift to the side that has the fewest moles of gas, This is an attempt to reduce the pressure of the system as. i could go on for more but im kinda tirred so ye ;p

hope this helps your understanding of what AS chemistry has to offer

*starts doing A2 work*

Amazingly that is only a very small amount more than we have to know, but I don't expect they'll test it.

[cuckoo99]

(Original post by gmseahorse)
Amazingly that is only a very small amount more than we have to know, but I don't expect they'll test it.

they teach le chateliers principle at gcse now ? equilibria is probly the easiest topic in AS unit 2 alongside redox though thats just me ;p

[meme0609]

Right, what did everyone get for the coulombs one?

[chocolate1996]

(Original post by meme0609)
Right, what did everyone get for the coulombs one?

24

[No brainer1]

I got so confused.

[meme0609]

(Original post by chocolate1996)
24

Yes!

[gmseahorse]

(Original post by cuckoo99)
they teach le chateliers principle at gcse now ? equilibria is probly the easiest topic in AS unit 2 alongside redox though thats just me ;p

Not the Chatliers priciple bit, but pretty much everything else you said.



In general I thought it was a nice paper, what does everybody else think.

[subjectman10]

I think it was quite easy, except the coulombs one.
The only thing I'm worried about is the grade boundaries- the paper was easy so they might make it harder to get A*

Also, will there be an unofficial mark scheme coming out soon?

[Simran Mars Foster]

I thought the paper was a really nice paper to!. We were given the jan 2012 paper at revision class and im not lying to you it was SO HARD!!!!. No where near as this paper!. Grade bounderies are going to rocket up though :/

[robynelisabeth]

(Original post by meme0609)
Yes!

same!

[zangorou]

I loved it so much my goodness!
The only one I wasn't certain about was the nano-tube one, but I made an educated guess, I hope.

[zangorou]

(Original post by chocolate1996)
24

The calculation one? I swear it was more than that!

[Simran Mars Foster]

I said that they can be joined to catalyst?

[Lilbixxie]

For the Columbs one I got 1440 because the table gave you the number in minutes so I thought you had to change it to seconds but I might be wrong

[Lilbixxie]

What did everyone put for the equation of h2?