Answer :
Answer:
1. 10 e⁻
Oxidation numbers
I₂O₅(s): I (5+); O(2-)
CO(g): C(2+); O(2-)
I₂(s): I(0)
CO₂(g): C(4+); O(2-)
2. 4 e⁻
Oxidation numbers
Hg²⁺(aq): Hg(2+)
N₂H₄(aq): N(2-); H(1+)
Hg(l): Hg(0)
N₂(g): N(0)
H⁺(aq): H(1+)
3. 6 e⁻
Oxidation numbers
H₂S(aq): H(1+); S(2-)
H⁺(aq): H(1+)
NO₃⁻(aq): N(5+); O(2-)
S(s): S(0)
NO(g): N(2+); O(2-)
H₂O(l): H(1+); O(2-)
Explanation:
In order to state the total number of electrons transferred we have to identify both half-reactions for each redox reaction.
1. I₂O₅(s) + 5 CO(g) → I₂(s) + 5 CO₂(g)
Oxidation: 10 e⁻ + 10 H⁺(aq) + I₂O₅(s) → I₂(s) + 5 H₂O(l)
Reduction: 5 H₂O(l) + 5 CO(g) → 5 CO₂(g) + 10 H⁺(aq) + 10 e⁻
2. 2 Hg²⁺(aq) + N₂H₄(aq) → 2 Hg(l) + N₂(g) + 4 H⁺(aq)
Oxidation: N₂H₄(aq) → N₂(g) + 4 H⁺(aq) + 4 e⁻
Reduction: 2 Hg²⁺(aq) + 4 e⁻ → 2 Hg(l)
3. 3 H₂S(aq) + 2H⁺(aq) + 2 NO₃⁻(aq) → 3 S(s) + 2 NO(g) + 4H₂O(l)
Oxidation: 3 H₂S(aq) → 3 S(s) + 6 H⁺(aq) + 6 e⁻
Reduction: 8 H⁺(aq) + 2 NO₃⁻(aq) + 6 e⁻ → 2 NO(g) + 4 H₂O
Answer:
The total number of electrons transferred in 1st reaction are 10, 2nd reactions are 4 and [tex]\rm 6\;e^-[/tex] are transferred in 3rd reaction.
Explanation:
Oxidation-reduction reactions are also known as Redox reactions. In these reactions one element is getting oxidized and other is getting reduced. To calculate the number of electrons transferred and oxidation number of each element in the reaction, the half reactions of Reduction and Oxidation are considered.
1. [tex]\rm I_2O_5\;+\;5\;CO\;+\;\rightarrow\;I_2\;+\;5\;CO_2\;[/tex]
Oxidation number:
[tex]\rm I_2O_5[/tex]: I : +5
O: -2
[tex]\rm CO[/tex]: C : +2
O : -2
[tex]\rm I_2[/tex]: I : 0
[tex]\rm CO_2[/tex] : C : +4
O : -2
The number of electron transferred :
Oxidation reaction: [tex]\rm 10^e^-\;+\;10^H^+\;+\;I_2O_5\;\rightarrow\;I_2\;+\;5\;H_2O[/tex]
Reduction reaction: [tex]\rm 5\;H_2O\;+\;5\;CO\;\rightarrow\;5\;CO_2+\;10\;H^+\;+\;10^e^-[/tex]
Total 10 electrons are transferred in balancing the reaction.
2. [tex]\rm 2\;Hg_2\;+\;N_2H_4\;\rightarrow\;2\;Hg\;+N_2\;+\;4\;H^+[/tex]
Oxidation number:
[tex]\rm Hg_2[/tex] : +2
[tex]\rm N_2_H_4[/tex] : N : -2
H : +1
Hg : 0
[tex]\rm N_2[/tex] : N : 0
[tex]\rm H^+[/tex] : H: +1
Total electrons transferred:
Oxidation reaction : [tex]\rm N_2H_4\;\rightarrow\;N_2\;+\;4\;H^+\;+\;4\;e^-[/tex]
Reduction reaction : [tex]\rm 2\;Hg^+\;+\;4\;e^-\;\rightarrow\;2\;Hg[/tex]
Total electrons transferred are 4 in the given reaction.
3. [tex]\rm 3\;H_2S\;+\;2\;H^+\;+\;2\;NO_3\;\rightarrow\;3\;S\;+\;2\;NO\;+4\;H_2O[/tex]
Oxidation number:
[tex]\rm H_2S[/tex] ; H : +1
S : -2
[tex]\RM H^+[/tex]: H: +1
[tex]\rm NO_3[/tex] : N : +5
O : -2
S : 0
NO : N : +2
O : -2
[tex]\rm H_2O[/tex] : H : +1
O : -2
Total number of electrons transferred :
Oxidation reaction : [tex]\rm 3\; H_2S\;\rightarrow\;3\;S\;+\;6\;H^+\;+\;6\;e^-[/tex]
Reduction reaction : [tex]\rm 8\;H^+\;+2\;NO_3^-\;+\;6\;e^-\;\rightarrow\;2\;NO\;+\;4\;H_2O[/tex]
Total electrons transferred in the reactions are 6 in number.
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