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# Current Year 13 Thread (2013/14) - Mark I Watch

1. Nooooooooooooooooooooooooooo

2. ffs

wai
3. (Original post by Pandora.)
Nooooooooooooooooooooooooooo

Haha!

4. (Original post by Felix Felicis)
ffs

wai
What a shame
5. (Original post by Felix Felicis)
ffs

wai
Life's tough man...

(Original post by usycool1)
Haha!

I hope you're pleased with yourself

My brother think Nadal won't win tomorrow.

6. Rafa.

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7. Was hoping for an all swiss final :/

Can only hope Djokovic/ Wawrinka take it now

8. I was so excited for a moment there, thinking that I could go to uni in London just to stalk a certain GOAT.

Alas, I think it's too late..
9. Dear Chemists!

So I got rate equation:
Rate=k[ClO2]^2[OH-]

And my question is:
How does it provide evidence that the reaction takes place by more than one step?
10. (Original post by purplemind)
Dear Chemists!

So I got rate equation:
Rate=k[ClO2]^2[OH-]

And my question is:
How does it provide evidence that the reaction takes place by more than one step?
Second order? No idea, just felt like saying something because it looks so good
11. (Original post by L'Evil Fish)
Second order? No idea, just felt like saying something because it looks so good
I had to work out orders in a previous part so I'm afraid stating that the order is second wouldn't be enough.
12. (Original post by purplemind)
Dear Chemists!

So I got rate equation:
Rate=k[ClO2]^2[OH-]

And my question is:
How does it provide evidence that the reaction takes place by more than one step?
Were you given the "actual" equation for the reaction?
13. (Original post by purplemind)
Dear Chemists!

So I got rate equation:
Rate=k[ClO2]^2[OH-]

And my question is:
How does it provide evidence that the reaction takes place by more than one step?
Have they given you any other information?
14. (Original post by purplemind)
I had to work out orders in a previous part so I'm afraid stating that the order is second wouldn't be enough.
Oh, there actually are orders? I'm just saying random stuff. Can't wait for A2
15. (Original post by usycool1)
Were you given the "actual" equation for the reaction?
(Original post by mynameisntbobk)
Have they given you any other information?
So from previous parts I know that:
Rate=k[ClO2]^2[OH-]
and k=200.

Later they tell me that 'In the overall equation, 2 mol ClO2 reacts with 2 mol OH- to form an aqueous solution containing chlorate (III) and chlorate (V) ions.

I found the overall equation: 2ClO2 + 2OH- -> ClO2- + ClO3- + H2O

(I thought this information isn't important because they asked how the rate equation provides evidence that reaction takes place by more than 1 step).

(Original post by L'Evil Fish)
Oh, there actually are orders? I'm just saying random stuff. Can't wait for A2
I'm doing OCR Chemistry A but I guess syllabus is similiar for all exam boards. But I don't find it too interesting (maybe that's because Chemistry isn't my favourite subject. )
16. (Original post by mynameisntbobk)
Congrats dude some hefty grades though I'm sure you'll manage it

(Original post by furryface12)
Well done! Good luck with those grades though

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(Original post by Lucy96)

Yay congratulations!
(Original post by Prinz655)
well done
Thanks guys
Thanks guys
Ooh, I've just seen - well done!
18. (Original post by purplemind)
So from previous parts I know that:
Rate=k[ClO2]^2[OH-]
and k=200.

Later they tell me that 'In the obverall equation, 2 mol ClO2 reacts with 2 mol OH- to form an aqueous solution containing chlorate (III) and chlorate (V) ions.

I found the overall equation: 2ClO2 + 2OH- -> ClO2- + ClO3- + H2O

(I thought this information isn't important because they asked how the rate equation provides evidence that reaction takes place by more than 1 step).
I'm not actually sure. I'd probably guess it has something to do with the fact that the orders of the reactant are different (?)
19. (Original post by purplemind)
So from previous parts I know that:
Rate=k[ClO2]^2[OH-]
and k=200.

Later they tell me that 'In the overall equation, 2 mol ClO2 reacts with 2 mol OH- to form an aqueous solution containing chlorate (III) and chlorate (V) ions.

I found the overall equation: 2ClO2 + 2OH- -> ClO2- + ClO3- + H2O

(I thought this information isn't important because they asked how the rate equation provides evidence that reaction takes place by more than 1 step).
Hmm...not 100% sure. If you're asked to just use the rate equation, all I can think of is that the rate equation shows only the rate-determining step (i.e. the slowest step in the reaction) and so there must be more than one step. Not 100% sure though tbh
Thanks guys
Congrats!!

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