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I'm not getting any of the optionsI asked this question already, but just thought I post it again since we're on a new page.
An aqueous solution was prepared containing 1.0mol of AgNO3 and 1.0mol of FeSO4 in 1.00 dm3
of water. When equilibrium was established, there was 0.44mol of Ag+(aq) in the mixture.
Ag+(aq) + Fe2+(aq) --> Ag(s) + Fe3+(aq)
What is Kc?
A. 0.35 B. 0.62 C. 1.62 D. 2.89
I got C as my answer but the correct one is D, can anyone explain how to get D?
even i am getting option C. Can you tell me which year paper is it ?I asked this question already, but just thought I post it again since we're on a new page.
An aqueous solution was prepared containing 1.0mol of AgNO3 and 1.0mol of FeSO4 in 1.00 dm3
of water. When equilibrium was established, there was 0.44mol of Ag+(aq) in the mixture.
Ag+(aq) + Fe2+(aq) --> Ag(s) + Fe3+(aq)
What is Kc?
A. 0.35 B. 0.62 C. 1.62 D. 2.89
I got C as my answer but the correct one is D, can anyone explain how to get D?
me neither trying frm long!!I'm not getting any of the options
wat method r u using please?
2. Total Flask Volume=5+10= 15dm3=15/1000 m3HELP Please :/
View attachment 8856
same hereme neither trying frm long!!
its winter 2011 variant 13 question 12. No examiners report out yet unfortunatelyeven i am getting option C. Can you tell me which year paper is it ?
I answered your first question, here is the next one:HELP Please :/
View attachment 8856
No point telling you my method, i got the wrong answer toome neither trying frm long!!
In Kc we do not take the concentration of the solid. So in this case we will not include the concentration of Ag(s)its winter 2011 variant 13 question 12. No examiners report out yet unfortunately
http://www.xtremepapers.com/papers/CIE/Cambridge International A and AS Level/Chemistry (9701)/9701_w11_qp_13.pdf
Thanks! That was a tough oneIn Kc we do not take the concentration of the solid. So in this case we will not include the concentration of Ag(s)
So it will be as follows:
Kc= (0.56) / (0.44^2)
= 2.89
That's option D
thanks a lot! i was trying the same thing of excluding Ag(s) but.... i thought we need to claculate its number of moles too ryt? then wat do we do wid da number of moles of Ag(s)?In Kc we do not take the concentration of the solid. So in this case we will not include the concentration of Ag(s)
So it will be as follows:
Kc= (0.56) / (0.44^2)
= 2.89
That's option D
You just ignore it the formula would be Kc=[Fe 3+]/[Ag +][Fe 2+]=.56/.44*.44thanks a lot! i was trying the same thing of excluding Ag(s) but.... i thought we need to claculate its number of moles too ryt? then wat do we do wid da number of moles of Ag(s)?
the ansewer is C you have to keep in mind that bond making is exothermic and bond breaking is endothermic.......
alright! so we dont need the moles of Ag den... THANKS A LOTYou just ignore it the formula would be Kc=[Fe 3+]/[Ag +][Fe 2+]=.56/.44*.44
Remember this: Bond breaking is endothermic(positive) and Bond making is exothermic(negative)
thanks..could you please solve 21 of the same paper?the ansewer is C you have to keep in mind that bond making is exothermic and bond breaking is endothermic.......
In P Br2 is broken to 2Br thus energy is given so ∆H=+193
In Q 2cl are converted into Cl2 thus energy is released so ∆H=-244
In R CH3+Cl a bind is made b/w C and Cl so ∆H=-340
In S CH4-----> CH3+H thus a bind b/w C and H is broken ∆H=+410
if we arrange ∆H in increasing order it is:-340,-244,+193,+410
thus R,Q,P,S
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