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Can you represent the reduction of perchlorate to chloride by oxidation of #NO_2# to nitrate anion?

Answer 1

Ellie Andrews

Well, #"perchlorate ion"# is reduced from #Cl(VII+)# to #Cl(-I)#....

#ClO_4^(-) + 8H^(+) + 8e^(-) rarr Cl^(-) + 4H_2O(l)# #(i)#

And #NO_2# is oxidized, #N(IV+)# to #N(V+)#:

#NO_2(g) +H_2O rarr NO_3^(-) +2H^(+) +e^-# #(ii)#

And so to eliminate the electrons, we take #(i) + 8xx(ii)#:

#8NO_2(g) +4H_2O+ClO_4^(-) rarr 8NO_3^(-) +8H^(+) + Cl^(-)#

Is the mass to charge ratio of this balanced?

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Answer 2

Serenity Allen

Yes, the reduction of perchlorate to chloride can be represented by the oxidation of NO2 to nitrate anion. This reaction involves the transfer of electrons, where perchlorate (ClO4-) is reduced to chloride (Cl-) and NO2 is oxidized to nitrate (NO3-). The balanced equation for this reaction is:

[4ClO4^- + 6NO2 + 6H2O \rightarrow 4Cl^- + 6NO3^- + 12H^+]

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.