Hydrogen-atom transfer
Hydrazine, losing hydrogen, is oxidized to molecular nitrogen, while oxygen, gaining hydrogen, is reduced to water.
When an oxidation number of an atom is increased in the course of a redox reaction, that atom is being oxidized. When an oxidation number of an atom is decreased in the course of a redox reaction, that atom is being reduced.
So, hearing this information, how will you solve your problem?
Identify all the species that got oxidized and reduced in the reactions below.
a. NaOH (aq) + HCl (aq) ----→ NaCl (aq) + H2O (l)
b. Fe (s) + CuCl2 (aq) -------→ FeCl2 (aq) + Cu (s)
c. Cr2O7 2- (aq) + Cl- (aq) -----→ Cr3+ (aq) + Cl2(g)
4 answers
a. I don't see any increase or decrease in atoms for this one. Is this a non-redox reaction?
b. Fe is the reduced and Cu is oxidized?
c. Cr is oxidized and Cl is reduced?
b. Fe is the reduced and Cu is oxidized?
c. Cr is oxidized and Cl is reduced?
I'm confused about hydrazine and N2. Don't see any in the problem.
There is no oxidation/reduction in a.
In b Fe is oxidized and Cu^2+ is reduced. Note the Fe INCREASES oxidation number from zero to 2+ and Cu DECREASES from 2+ to zero. In c, Cr is reduced (EACH Cr goes from oxidation state of 6+ to 3+ so it DECREASES while Cl goes from 1- to zero so it INCREASES.
In b Fe is oxidized and Cu^2+ is reduced. Note the Fe INCREASES oxidation number from zero to 2+ and Cu DECREASES from 2+ to zero. In c, Cr is reduced (EACH Cr goes from oxidation state of 6+ to 3+ so it DECREASES while Cl goes from 1- to zero so it INCREASES.
1 answer