Can someone please please please help me in this ALEVEL CHEM pp question ?
Q14 part b ii
https://qualifications.pearson.com/content/dam/pdf/International%20Advanced%20Level/Chemistry/2013/Exam%20materials/WCH05_01_que_20180119.pdf
https://qualifications.pearson.com/content/dam/pdf/International%20Advanced%20Level/Chemistry/2013/Exam%20materials/WCH05_01_rms_20180308.pdf
I got the ratio 1:4 which is correct according to the MS but I don't understand how we should know that the product is SO4 2-
I wrote the equation with S4O6 2- as the product because that was the product in part i , the ratio turned out to be 1:2 in my equation, which didn't match the calculation I made but how do I know whether my calculation is incorrect or my equation is incorrect in an exam ? Most importantly, how do I know what the products are when there are so many possibilities ?
https://qualifications.pearson.com/content/dam/pdf/International%20Advanced%20Level/Chemistry/2013/Exam%20materials/WCH05_01_que_20180119.pdf
https://qualifications.pearson.com/content/dam/pdf/International%20Advanced%20Level/Chemistry/2013/Exam%20materials/WCH05_01_rms_20180308.pdf
I got the ratio 1:4 which is correct according to the MS but I don't understand how we should know that the product is SO4 2-
I wrote the equation with S4O6 2- as the product because that was the product in part i , the ratio turned out to be 1:2 in my equation, which didn't match the calculation I made but how do I know whether my calculation is incorrect or my equation is incorrect in an exam ? Most importantly, how do I know what the products are when there are so many possibilities ?
Br2 is a stronger oxidant than I2 so you might expect S to be oxidised more than +2 to +2.5
mole ratio of S2O32-:Br2 = 1:4
8 electrons are gained by the 4 Br2 molecules
this must be lost by 1 S2O32- molecule
each S atom must lose 4 electrons
Oxidation number of S must go from +2 to +6, so SO42- ion is formed
mole ratio of S2O32-:Br2 = 1:4
8 electrons are gained by the 4 Br2 molecules
this must be lost by 1 S2O32- molecule
each S atom must lose 4 electrons
Oxidation number of S must go from +2 to +6, so SO42- ion is formed
Original post by BobbJo
Br2 is a stronger oxidant than I2 so you might expect S to be oxidised more than +2 to +2.5
mole ratio of S2O32-:Br2 = 1:4
8 electrons are gained by the 4 Br2 molecules
this must be lost by 1 S2O32- molecule
each S atom must lose 4 electrons
Oxidation number of S must go from +2 to +6, so SO42- ion is formed
mole ratio of S2O32-:Br2 = 1:4
8 electrons are gained by the 4 Br2 molecules
this must be lost by 1 S2O32- molecule
each S atom must lose 4 electrons
Oxidation number of S must go from +2 to +6, so SO42- ion is formed
Oh, that makes sense.
1 more thing please, if a molecule had a C=C and an OH + a COOH
so
it was able to from both addition and condensation polymerisation, which one is more likely ?
Original post by Leah.J
Oh, that makes sense.
1 more thing please, if a molecule had a C=C and an OH + a COOH
so
it was able to from both addition and condensation polymerisation, which one is more likely ?
1 more thing please, if a molecule had a C=C and an OH + a COOH
so
it was able to from both addition and condensation polymerisation, which one is more likely ?
Is it a past paper question? Any source?
Probably condensation polymerisation since small molecules are eliminated, hence giving a larger increase in entropy than the corresponding addition polymer of similar length
Original post by BobbJo
Is it a past paper question? Any source?
Probably condensation polymerisation since small molecules are eliminated, hence giving a larger increase in entropy than the corresponding addition polymer of similar length
Probably condensation polymerisation since small molecules are eliminated, hence giving a larger increase in entropy than the corresponding addition polymer of similar length
No, I just saw the polymer polypropenamide and I got the question. It can't form condensation polymers I know
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