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WJEC Chemistry CH5 Summer 2012 Exam Tweet

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1. Re: WJEC Chemistry CH5 Summer 2012 Exam
(Original post by nikhil.shah)
I got 15.5, but can someone explain why this was correct??? I just kind of multiplied some numbers and got it lol...
Asking because my friend put quite a logical argument to me after that basically said because the pack was smaller (only 0.5 moles in 200g) than the 1 mol in 1kg the temp change should be smaller than 6.3 degrees
because this is 2.5 times more concentrated than 1 mol in 1 kg,
if it was as simple as your friends logic, we could just halve their given change, as we have half a mole
6.2 x 2.5 = 15.5
Last edited by kobrakaai; 19-06-2012 at 22:53.
2. Re: WJEC Chemistry CH5 Summer 2012 Exam
did anyone get a molar ratio of 1:2 NH3NO3 because the reaction only began when ten cm^3 of NH3 was added to 20cm^3 of HNO3?
3. Re: WJEC Chemistry CH5 Summer 2012 Exam
(Original post by TSRuser1234)
did anyone get a molar ratio of 1:2 NH3NO3 because the reaction only began when ten cm^3 of NH3 was added to 20cm^3 of HNO3?
it was 1:1
4. Re: WJEC Chemistry CH5 Summer 2012 Exam
It was the same concentration of NH3 and HNO3 and both had 20cm^2 at equilibrium so I said it was 1:1 ?
5. Re: WJEC Chemistry CH5 Summer 2012 Exam
(Original post by Bland New Eyes)
It was the same concentration of NH3 and HNO3 and both had 20cm^2 at equilibrium so I said it was 1:1 ?
That is correct.
6. Re: WJEC Chemistry CH5 Summer 2012 Exam
What did everyone do for the Le Chateliers principle question to reduce the amount of Iodine present? I wasn't sure so said add sodium thiosulphate to remove the iodine, but don't think that's right.
7. (Original post by biolchem)
What did everyone do for the Le Chateliers principle question to reduce the amount of Iodine present? I wasn't sure so said add sodium thiosulphate to remove the iodine, but don't think that's right.
You had to add NaOH, the OH- ions react and remove the H+ ions from solution so equilibrium would shift to the left to counteract the change

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