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But violet isn't in the optionIsn't it 400 for D ?
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But violet isn't in the optionIsn't it 400 for D ?
Thanks.Here you go. It would be a really crowded structure in a space fill model.
how about this question ?But violet isn't in the option
Why will u do that?how about this question ?
Value in c(i) is 7 x 10^-7 . in the mark scheme it's written concentration of product if 0.1 but shouldn't it be 0.1 - (7 x 10^-7 )?
You made ur equation of Kc.how about this question ?
Value in c(i) is 7 x 10^-7 . in the mark scheme it's written concentration of product if 0.1 but shouldn't it be 0.1 - (7 x 10^-7 )?
Yes but we need to use the concentration of Ag(NH3)2 not of silver nitrateYou made ur equation of Kc.
Just substitute the values and find [NH3(aq)]
o.1 is conc of silver nitrate soln and (7 x 10^-7 ) is conc of Ag.
= (Mass no x Relative Abundance) / (Relative Abundance)View attachment 59644 Can anyone plz explain me why the answer for chemistry may june 2007 v1 p1 first answer is C?
From part (a) you can see that there is no effect of Cl- ion on production of O2 where as if u see the reaction of chlorine the equilibrium shifts to form more chlorine and moves in direction of electrons thus the E value will be less positive that is it will decrease.
I believe the CD has been uploaded here before, so you could find it by using the search bar in xtremepapers. If not, here is a torrent link for the CD.
The tricky thing involved in the 11 question is the balancing of the redox reaction equation. You're given this reaction:http://papers.xtremepapers.com/CIE/Cambridge International A and AS Level/Chemistry (9701)/9701_s13_qp_11.pdf
Can anyone please explain question 11 and 12?
Your cycle is correct, but you don't need to make any cycles here. Do this question with bond energies. Find the energy absorbed for bond-breaking, and the energy released when bonds were formed. Then simply subtract the energy released from energy absorbed to get the enthalpy change.View attachment 59660
Is my enthalpy cycle for Q12 correct? View attachment 59661
If it is, how do I calculate the enthalpy change of combustion now?
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