24Q1 edited [1]
Q3 u r rite ...thx[1]
Q1 Which can not reduce acidified soln of MnO4 -
a)H2C2O4
b)H2
c)H
d)Fe2+
Q2 which oxidising agent is not used for oxidn of mangantae to permanagante
a)CO2
b)H2O2
Q3 which of the following cannpt be oxidised by acidified KMnO4
a)sodium oxalate
b)potassium iodide
c)ferrous sulfate
c)sodium sulfate
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14 Answers
106Q1. acidified KMnO4 is oxidising agent naa? how can it reduce something ??
Q3. (d) all others can be oxidised. oxalate to CO2 iodide to I2 and ferrous to ferric
106yeah if it is H+ then option (c) becz it cant be oxidised further.. but what is H ? (maybe [H] ??) (nascent H)
1Q.1) its 'b' - H2
a) 8 H+(aq) + MnO4.-(aq) + 5 e- → Mn2+(aq) + 4 H2O.
this reaction is becoz of the presence of H+ ions in oxalic acid.
c) ' H ' is certainly reducing, as nascent state is most reactive and in most reactions, [H] only facilitates reduction.
d) Fe2+ + MnO4.- + H2O → Fe3+ + Mn2+ + OH-
this reaction takes place readily.
thus, its 'b'
106abhi what happens with H2(how does it reduce)
as far as i know [H] reduces things.. (not act as catalyst)
1sorry, i didn't mean dat. i meant facilitates. its the cause of occurence.
sorry, my english is a bit weak
1sorry, i linked it wrong.
Q.2) Actually the reaction wid H2O2 , if possible will take place this way :
H2O2 + MnO42- → MnO4- + H2O.
but the reaction doesn't go to completion . becoz MnO4- ion again oxidises water to O2 gas and itself gets reduced to MnO42- (manganate ion ).thus this reaction doesn't take place.
And with CO2 ,
CO2 + MnO42- → MnO4- + C2O32-.
Q.4) d) as here Na and S atoms are at maximum oxidation states.
24kk thx....
btw in reaction with CO2 is C2O3 the only possiblity ????
I mean any explaination for that ??
1any other possible is CO , C3O2 . Carbon suboxide ( C3O2) is unstable. and CO is stable , but i think it too exists in the state of oxalate ion.