Perform the following calculations for the unbalanced reaction S40 (aq) + 21 (aq) →→ 1₂(s) + S₂0₂² (aq) (a) Identify the oxidizing and reducing agents. Oxidizing agent: O S40,² (aq) I (aq) 1₂(s) $₂0,² (aq) 0 (b) Calculate the E -0.45 and calculate E 2- SO +2e S in S40: 2.5 S in S₂0₂²": 0 E Oxidation numbers: 0:-2✔ cell half-cell half-cell (c) For the reduction half-reaction, write a balanced equation, give the oxidation number of each element, 0 --0.45 2- -25₂03 Reducing agent: ⒸS40,² (aq) Or(aq) 1₂(s) S₂03² (aq) AG 0 E -87.8 kJ/mol anode =0.53 V

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Perform the following calculations for the unbalanced reaction
S40 (aq) + 21 (aq) →→ 1₂(s) + S₂0₂² (aq)
(a) Identify the oxidizing and reducing agents.
Oxidizing agent:
O S40,² (aq)
I (aq)
1₂(s)
$₂0,² (aq)
0
(b) Calculate the E
-0.45
and calculate E
2-
0
E
+2e
S in S40: 2.5
S in $₂0,²":
Oxidation numbers:
0:-2✔
half-cell
cell
(c) For the reduction half-reaction, write a balanced equation, give the oxidation number of each element,
0
half-cell
--0.45
2-
-25₂03
Reducing agent:
ⒸS40,² (aq)
O I (aq)
1₂(s)
S₂03² (aq)
AG-87.8 kJ/mol
0
E
anode
=0.53 V
Transcribed Image Text:Perform the following calculations for the unbalanced reaction S40 (aq) + 21 (aq) →→ 1₂(s) + S₂0₂² (aq) (a) Identify the oxidizing and reducing agents. Oxidizing agent: O S40,² (aq) I (aq) 1₂(s) $₂0,² (aq) 0 (b) Calculate the E -0.45 and calculate E 2- 0 E +2e S in S40: 2.5 S in $₂0,²": Oxidation numbers: 0:-2✔ half-cell cell (c) For the reduction half-reaction, write a balanced equation, give the oxidation number of each element, 0 half-cell --0.45 2- -25₂03 Reducing agent: ⒸS40,² (aq) O I (aq) 1₂(s) S₂03² (aq) AG-87.8 kJ/mol 0 E anode =0.53 V
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