Complete the half-reactions that occur at each electrode in the cell shown. Then, write the line notation for the cell. Pb -PbCl₂(s) KCl(aq) Anode half-reaction: Pb(s) + 2Cl(aq) = Cathode half-reaction: 2 AgCl(s) Pb(s) Line notation: +2e= V CI (aq) KCl(aq) Ag -AgCl(s) PbCl₂ (s) +2e¯ PbCl₂ (s) 2 Ag(s) + 2Cl(aq) AgCl(s) Ag(s) AgCl(s) CI (aq) CI (aq) Answer Bank 2 AgCl(s) PbCl₂(s) 2 Ag(s) Ag(s) Pb(s) < Feedback The aqueous chloride ion is shown in the line notation in contact with the salt bridge.

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Chapter1: Chemical Foundations
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Complete the half-reactions that occur at each electrode in the cell shown. Then, write the line notation for the cell.
Pb
-PbCl₂(s)
KCl(aq)
Anode half-reaction:
Pb(s) + 2Cl(aq) =
Cathode half-reaction:
2 AgCl(s) +2e=
Pb(s)
Line notation:
V
Cl(aq)
KCl(aq)
Ag
PbCl₂ (s)
PbCl₂(s)
-AgCl(s)
+ 2e
2 Ag(s) + 2Cl(aq)
AgCl(s)
Ag(s)
AgCl(s)
CI (aq)
CI (aq)
Answer Bank
2 AgCl(s)
PbCl₂ (s)
2 Ag(s)
Ag(s)
Pb(s)
< Feedback
The aqueous chloride ion is shown in
the line notation in contact with the
salt bridge.
Transcribed Image Text:Complete the half-reactions that occur at each electrode in the cell shown. Then, write the line notation for the cell. Pb -PbCl₂(s) KCl(aq) Anode half-reaction: Pb(s) + 2Cl(aq) = Cathode half-reaction: 2 AgCl(s) +2e= Pb(s) Line notation: V Cl(aq) KCl(aq) Ag PbCl₂ (s) PbCl₂(s) -AgCl(s) + 2e 2 Ag(s) + 2Cl(aq) AgCl(s) Ag(s) AgCl(s) CI (aq) CI (aq) Answer Bank 2 AgCl(s) PbCl₂ (s) 2 Ag(s) Ag(s) Pb(s) < Feedback The aqueous chloride ion is shown in the line notation in contact with the salt bridge.
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