IGCSE/GCSE/O & A Level/IB/University Student Forum
Qualification => Subject Doubts => GCE AS & A2 Level => Sciences => Topic started by: Ghost Of Highbury on September 06, 2009, 03:31:15 pm
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okk..a doubt in reduction and oxidation
1) C4H8 + 6O2 --> 4CO2 + 4H2O
is this reduction, oxidation or reduction and why?
i strongly think that it is oxidation as oxygen is added...however, the oxidation state of "oxygen" decreases from -4 to -6
so its redox...
plzz..helpp!!
2.) 2KNO3=2KNO2+O2
this equation is so messed up for oxidation states
there are three elements in 1 compund ...how do u determine the oxidation states for them
plzz help!! is it oxidation reduction or redox..(plz explain the reason too!
thanks a lot!!
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I'll break it up and explain
1) In C4H8
H has ox.state +1 on each...so +1
the overall charge on the compound is 0
so C has ox.state -2
In 602
the ox.state is 0
Products
In 4CO2
C goes on to become +4 and O2 becomes -2
and H remains as +1 and O -2
it is redox becuz Cs ox.state has increased and that of oxygen has decreased
You do take into account the ox.state of oxygen
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I'll break it up and explain
1) In C4H8
H has ox.state +1 on each...so +1
the overall charge on the compound is 0
so C has ox.state -2
In 602
the ox.state is 0
Products
In 4CO2
C goes on to become +4 and O2 becomes -2
and H remains as +1 and O -2
it is redox becuz Cs ox.state has increased and that of oxygen has decreased
You do take into account the ox.state of oxygen
understood everything...
only..H becomes +2 na as its H2O
and...O2 becomes -4 na as it is O2
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second one
in KNO3
NO3 is ionic
so overall charge is -1
K is +1 and O3 is -6
so N is +5....+5-6=-1..overall charge becomes zero with K as +1
ok so
their states change to
NO2 again ionic with -1 charge
N becomes +3 since it is O2 and O2 is -4 overall
K remains as +1
and ox.state of O2 becomes 0
so Oxygen's ox.state increased but that of N decreased
so it's redox again
I've tried my best to explain
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I'll break it up and explain
1) In C4H8
H has ox.state +1 on each...so +1
the overall charge on the compound is 0
so C has ox.state -2
In 602
the ox.state is 0
Products
In 4CO2
C goes on to become +4 and O2 becomes -2
and H remains as +1 and O -2
it is redox becuz Cs ox.state has increased and that of oxygen has decreased
You do take into account the ox.state of oxygen
understood everything...
only..H becomes +2 na as its H2O
and...O2 becomes -4 na as it is O2
yaa if u mean the overall charge
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second one
in KNO3
NO3 is ionic
so overall charge is -1
K is +1 and O3 is -6
so N is +5....+5-6=-1..overall charge becomes zero with K as +1
ok so
their states change to
NO2 again ionic with -1 charge
N becomes +3 since it is O2 and O2 is -4 overall
K remains as +1
and ox.state of O2 becomes 0
so Oxygen's ox.state increased but that of N decreased
so it's redox again
I've tried my best to explain
thanks a lot~
just 1 qestion...is the charge of the NO3 and NO2 --> -1
if so ...how did u get that?...
soo..if its SO4...is the oxidation state overall -2??
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second one
in KNO3
NO3 is ionic
so overall charge is -1
K is +1 and O3 is -6
so N is +5....+5-6=-1..overall charge becomes zero with K as +1
ok so
their states change to
NO2 again ionic with -1 charge
N becomes +3 since it is O2 and O2 is -4 overall
K remains as +1
and ox.state of O2 becomes 0
so Oxygen's ox.state increased but that of N decreased
so it's redox again
I've tried my best to explain
thanks a lot~
just 1 qestion...is the charge of the NO3 and NO2 --> -1
if so ...how did u get that?...
soo..if its SO4...is the oxidation state overall -2??
this is a general rule
In an ion, the sum equals the overall charge
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thought so..
tks a lot!!
u sure both r redox..
because astar told me that the 1st one is oxidation and the 2nd one is reduction...??@?@?@?
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thought so..
tks a lot!!
u sure both r redox..
because astar told me that the 1st one is oxidation and the 2nd one is reduction...??@?@?@?
i just did redox yesterday...so according to my AS textbook..it's redox
but i'll ask my teacher tom and let you know if it's 200% redox or not..