Which balanced redox reaction is occurring in the voltaic cell represented by the notation of \(\mathrm{Al}(\mathrm{s})\left|\mathrm{Al}^{3+}(\mathrm{aq}) \| \mathrm{Pb}^{2+}(\mathrm{aq})\right| \mathrm{Pb}(\mathrm{s}) ?\)
Select one:
Q \(\mathrm{Al}(\mathrm{s})+\mathrm{Pb}^{2+}(\mathrm{aq}) \longrightarrow \mathrm{Al}^{3+}(\mathrm{aq})+\mathrm{Pb}(\mathrm{s})\)
\bigcirc \(2 \mathrm{Al}^{3+}(\mathrm{aq})+3 \mathrm{~Pb}(\mathrm{~s}) \longrightarrow 2 \mathrm{Al}(\mathrm{s})+3 \mathrm{~Pb}^{2+}\) (aq)
Q \(\mathrm{Al}^{3+}(\mathrm{aq})+\mathrm{Pb}(\mathrm{s}) \longrightarrow \mathrm{Al}(\mathrm{s})+\mathrm{Pb}^{2+}(\mathrm{aq})\)
\(2 \mathrm{Al}(\mathrm{s})+3 \mathrm{~Pb}^{2+}(\mathrm{aq}) \longrightarrow 2 \mathrm{Al}^{3+}(\mathrm{aq})+3 \mathrm{~Pb}(\mathrm{~s})\)
Given cell notation is, \(\mathrm{Al}(\mathrm{s})\left|\mathrm{Al}^{3+}(\mathrm{aq}) \| \mathrm{Pb}^{2+}(\mathrm{aq})\right| \mathrm{Pb}(\mathrm{s})\)
In this notation, \(\|\) represents salt bridge. The half-cell present on the left side of salt bridge represents oxidation half reaction. The half-cell present on the right side of salt bridge represents reduction half reaction. Oxidation half reaction: \(\mathrm{Al}(\mathrm{s}) \longrightarrow \mathrm{Al}^{3+}(a q)+3 \mathrm{e}^{-}\)
Reduction half reaction \(: \mathrm{Pb}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow \mathrm{Pb}(\mathrm{s})\)
The number of electrons lost is not equal to number of electrons gained. Thus, to get balanced redox reaction multiply the oxidation half reaction with 2 and the reduction reaction with 3 . Add the resultant reactions.
\(2 \mathrm{Al}(\mathrm{s}) \longrightarrow 2 \mathrm{Al}^{3+}(\mathrm{aq})+6 \mathrm{e}^{-}\)
\(3 \mathrm{~Pb}^{2+}(\mathrm{aq})+6 \mathrm{e}^{-} \longrightarrow 3 \mathrm{~Pb}(\mathrm{~s})\)
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\(2 \mathrm{Al}(\mathrm{s})+3 \mathrm{~Pb}^{2+}(\mathrm{aq}) \longrightarrow 2 \mathrm{Al}^{3+}(\mathrm{aq})+3 \mathrm{~Pb}(\mathrm{~s})\)
Which balanced redox reaction is occurring in the voltaic cell represented by the notation of \(\mathrm{Al}(\mathrm{s})\left|\mathrm{Al}^{3+}(\mathrm{aq})...
Consider a voltaic cell that uses the reaction$$ 2 \mathrm{Al}(\mathrm{s})+3 \mathrm{Fe}^{2+}(\mathrm{aq}) \rightarrow 2 \mathrm{Al}^{3+}(\mathrm{aq})+3 \mathrm{Fe}(\mathrm{s}) $$What is the potential of the cell at \(25^{\circ} \mathrm{C}\). given the following ion concentrations?$$ \begin{aligned} &{\left[\mathrm{Al}^{3+}\right]=0.10 \mathrm{M}} \\ &{\left[\mathrm{Fe}^{2+}\right]=0.020 \mathrm{M}} \end{aligned} $$ 1.20 V 1.17 V 1.03 V 1.19 V
for a cell Zn-Al, write a balanced redox reaction that is occurring in the cell. include phase labels for each substance.
tion 3 of 40 ) A voltaic cell employs the redox reaction: Zn (s) + Pb2+ (aq) — Zn2+ (aq) + Pb () where Pb2+ (aq) + 2e Zn2+(aq) + 2e Pb(s) E = -0.1262 V Zn(s) E = -0.7618 V The cell potential (Ecell) of this voltaic cell when [Pb2+1 = 1.10 M and [Zn2+) = 0.00110 Mis:
What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) | Pb2+(aq) | | H+(aq) H2 | (g) | Pt A. Pb(s) B. Pt C. Pb2+(aq) D. H2(g) E. H+(aq) We were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this image
A voltaic cell is constructed using silver and aluminum. The following is the unbalanced redox reaction: Ag+ (aq) + Al(s) Ag (s) + A13+ (aq) What is the correct, balanced redox reaction that occurs in the cell? O A 5 Ag+ (aq) + 3 AI (5) - 5 Ag (s) + 3 A13+ (aq) O B. Ag* (aq) + 4 AI (5) ► Ag (s) + 4 A13+ (aq) OC 3 Ag* (aq) + Al(s) — 3 Ag (s) +...
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3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s) + Mn2+ (aq) a) Make a sketch of the cell. Label the cathode, anode, Sn2+, Mn, Sn, Mn?, and salt bridge. Indicate the direction of electron flow and the direction of ion flow from the salt bridge. b) Use line notation to represent the cell. c) What is the cell potential at 25°C when [Sn?] is 0.002 M and [Mn2+] is 0.050 M?
4. The following balanced redox reaction occurs in voltaic cell at 25°C H2 (g) + 2Ag+ (aq) → 2H* (aq) + 2 Ag (s) 2H+ + 2e → H2 (g) EⓇ = 0.00V Ag (aq) + le → Ag(s) E = +0.80V a. Write the two half-reactions (oxidation and reduction) occurring in the cell. Clearly indicate which reaction shows oxidation and which shows reduction. Clearly indicate which reaction occurs at the anode and which reaction occurs at the cathode. (4...
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