Be sure to answer all parts.(a) Balance the skeleton reaction. Include the states of matter for each substance.(b) Calculate E(c) Determine whether the reaction is spontaneous.A table of standard electrode potentials is given below for reference.Cl₂(g) + Fe2+ (aq) → CI (aq) + Fe³+ (aq)(a)(b)(c)OStrength of oxidizing agentcellVnot spontaneousspontaneousSelected Standard Electrode Potentials (298 K)Half-ReactionF2(g) + 2e7Cl₂(g) + 2e7MnO₂(s) + 4H+ (aq) + 2e7NO3(aq) + 4H+ (aq) + 3e¯Ag+ (aq) + eFe³+ (aq) + eO₂(g) + 2H₂O() + 4eCu²+ (aq) + 2e72H+ (aq) + 2e7N₂(g) + 5H+ (aq) + 4e¯Fe2+ (aq) + 2e72+Zn²+ (aq) + 2e2H₂O() +2e7Na+ (aq) + e2F (aq)2C1 (aq)2+Mn²+ (aq) + 2H₂O(l)NO(g) + 2H₂O(l)Ag(s)Fe²+ (aq)4OH(aq)Cu(s)H₂(g)N₂Hs+ (aq)Fe(s)Zn(s)H₂(g) + 2OH(aq)Na(s)Strength of reducing agentE half-cell (V)+2.87+1.36+1.23+0.96+0.80+0.77+0.40+0.340.00-0.23-0.44-0.76-0.83-2.71

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Be sure to answer all parts. (a) Balance the skeleton reaction. Include the states of matter for each substance. (b) Calculate E (a) (c) Determine whether the reaction is spontaneous. A table of standard electrode potentials is given below for reference. Cl₂(g) + Fe2+ (aq) →→CI (aq) + Fe³+ (aq) (b) (c) 0 V cell not spontaneous spontaneous

Be sure to answer all parts. (a) Balance the skeleton reaction. Include the states of matter for each substance. (b) Calculate E (a) (c) Determine whether the reaction is spontaneous. A table of standard electrode potentials is given below for reference. Cl₂(g) + Fe2+ (aq) →→CI (aq) + Fe³+ (aq) (b) (c) 0 V cell not spontaneous spontaneous

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Chapter1: Chemical Foundations

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Be sure to answer all parts.
(a) Balance the skeleton reaction. Include the states of matter for each substance.
(b) Calculate E
(c) Determine whether the reaction is spontaneous.
A table of standard electrode potentials is given below for reference.
Cl₂(g) + Fe2+ (aq) → CI (aq) + Fe³+ (aq)
(a)
(b)
(c)
O
Strength of oxidizing agent
cell
V
not spontaneous
spontaneous
Selected Standard Electrode Potentials (298 K)
Half-Reaction
F2(g) + 2e7
Cl₂(g) + 2e7
MnO₂(s) + 4H+ (aq) + 2e7
NO3(aq) + 4H+ (aq) + 3e¯
Ag+ (aq) + e
Fe³+ (aq) + e
O₂(g) + 2H₂O() + 4e
Cu²+ (aq) + 2e7
2H+ (aq) + 2e7
N₂(g) + 5H+ (aq) + 4e¯
Fe2+ (aq) + 2e7
2+
Zn²+ (aq) + 2e
2H₂O() +2e7
Na+ (aq) + e
2F (aq)
2C1 (aq)
2+
Mn²+ (aq) + 2H₂O(l)
NO(g) + 2H₂O(l)
Ag(s)
Fe²+ (aq)
4OH(aq)
Cu(s)
H₂(g)
N₂Hs+ (aq)
Fe(s)
Zn(s)
H₂(g) + 2OH(aq)
Na(s)
Strength of reducing agent
E half-cell (V)
+2.87
+1.36
+1.23
+0.96
+0.80
+0.77
+0.40
+0.34
0.00
-0.23
-0.44
-0.76
-0.83
-2.71

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