Find the G- of a galvanic cell with Ag and Al-Standard Reduction Potentials at 25-CHalf-Reaction E-V F2 - 2e- 2F- 2-87 Ag2 - e- Ag- 1-99 Co3- - e- Co2- 1-82 H2O2 - 2H- - 2e- 2H2O 1-78 MnO4- - 4H- - 3e- MnO2 - 2H2O 1-68 2e- - 2H- - IO4- IO3- - H2O 1-60 MnO4- - 8H- - 5e- Mn2- - 4H2O 1-51 Au3- - 3e- Au 1-50 Cl2 - 2e- 2Cl- 1-36 O2 - 4H- - 4e- 2H2O 1-23 MnO2 - 4H- -2e- Mn2- - 2H2O 1-21 Br2 - 2e- 2Br- 1-09 NO3- - 4H- - 3e- NO - 2H2O 0-96 ClO2 - e- ClO2 0-954 2Hg2- - 2e- Hg22- 0-91 Ag- - e- Ag 0-80 Hg22- - 2e- 2Hg 0-80 Fe3- - e- Fe2- 0-77 O2 - 2H- - 2e- H2O2 0-68 MnO4- - e- MnO42- 0-56 I2 - 2e- 2I- 0-54 Cu- - e- Cu 0-52 O2 - 2H2O - 4e- 4OH- 0-40 Cu2- - 2e- Cu 0-34 AgCl - e- Ag - Cl- 0-22 Cu2- - e- Cu- 0-16 2H- - 2e- H2 0-00 Fe3- - 3e- Fe -0-036 Pb2- - 2e- Pb -0-13 Ni2- - 2e- Ni -0-23 Cd2- - 2e- Cd -0-40 Fe2- - 2e- Fe -0-44 Cr3- - e- Cr2- -0-50 Cr3- - 3e- Cr -0-73 Zn2- - 2e- Zn -0-76 2H2O - 2e- H2 - 2OH- -0-83 Mn2- - 2e- Mn -1-18 Al3- 3e- Al -1-66 H2 - 2e- 2H- -2-23 Mg2- - 2e- Mg -2-37 Na- - e- Na -2-71 Ca2- - 2e- Ca -2-76 Ba2- - 2e- Ba -2-90 K- - e- K -2-92 Li- - e- Li -3-05

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Electrode Potential

Find the G∘...

Question

Find the $△ G^{\circ}$ of a galvanic cell with $A g$ and $A l$ .
Standard Reduction Potentials at $25^{\circ} C$
Half-Reaction $E^{\circ} (V)$
$F_{2} + 2 e^{-} \to 2 F^{-}$ $2.87$
$A g^{2} + e^{-} \to A g^{+}$ $1.99$
$C o^{3 +} + e^{-} \to C o^{2 +}$ $1.82$
$H_{2} O_{2} + 2 H^{+} + 2 e^{-} \to 2 H_{2} O$ $1.78$
$M n O_{4}^{-} + 4 H^{+} + 3 e^{-} \to M n O_{2} + 2 H_{2} O$ $1.68$
$2 e^{-} + 2 H^{+} + I O_{4}^{-} \to I O_{3}^{-} + H_{2} O$ $1.60$
$M n O_{4}^{-} + 8 H^{+} + 5 e^{-} \to M n^{2 +} + 4 H_{2} O$ $1.51$
$A u^{3 +} + 3 e^{-} \to A u$ $1.50$
$C l_{2} + 2 e^{-} \to 2 C l^{-}$ $1.36$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$ $1.23$
$M n O_{2} + 4 H^{+} + 2 e^{-} \to M n^{2 +} + 2 H_{2} O$ $1.21$
$B r_{2} + 2 e^{-} \to 2 B r^{-}$ $1.09$
$N O_{3}^{-} + 4 H^{+} + 3 e^{-} \to N O + 2 H_{2} O$ $0.96$
$C l O_{2} + e^{-} \to C l O_{2}$ $0.954$
$2 H g^{2 +} + 2 e^{-} \to H g_{2}^{2 +}$ $0.91$
$A g^{+} + e^{-} \to A g$ $0.80$
$H g_{2}^{2 +} + 2 e^{-} \to 2 H g$ $0.80$
$F e^{3 +} + e^{-} \to F e^{2 +}$ $0.77$
$O_{2} + 2 H^{+} + 2 e^{-} \to H_{2} O_{2}$ $0.68$
$M n O_{4}^{-} + e^{-} \to M n O_{4}^{2 -}$ $0.56$
$I_{2} + 2 e^{-} \to 2 I^{-}$ $0.54$
$C u^{+} + e^{-} \to C u$ $0.52$
$O_{2} + 2 H_{2} O + 4 e^{-} \to 4 O H^{-}$ $0.40$
$C u^{2 +} + 2 e^{-} \to C u$ $0.34$
$A g C l + e^{-} \to A g + C l^{-}$ $0.22$
$C u^{2 +} + e^{-} \to C u^{+}$ $0.16$
$2 H^{+} + 2 e^{-} \to H_{2}$ $0.00$
$F e^{3 +} + 3 e^{-} \to F e$ $- 0.036$
$P b^{2 +} + 2 e^{-} \to P b$ $- 0.13$
$N i^{2 +} + 2 e^{-} \to N i$ $- 0.23$
$C d^{2 +} + 2 e^{-} \to C d$ $- 0.40$
$F e^{2 +} + 2 e^{-} \to F e$ $- 0.44$
$C r^{3 +} + e^{-} \to C r^{2 +}$ $- 0.50$
$C r^{3 +} + 3 e^{-} \to C r$ $- 0.73$
$Z n^{2 +} + 2 e^{-} \to Z n$ $- 0.76$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$ $- 0.83$
$M n^{2 +} + 2 e^{-} \to M n$ $- 1.18$
$A l^{3 +} + 3 e^{-} \to A l$ $- 1.66$
$H_{2} + 2 e^{-} \to 2 H^{-}$ $- 2.23$
$M g^{2 +} + 2 e^{-} \to M g$ $- 2.37$
$N a^{+} + e^{-} \to N a$ $- 2.71$
$C a^{2 +} + 2 e^{-} \to C a$ $- 2.76$
$B a^{2 +} + 2 e^{-} \to B a$ $- 2.90$
$K^{+} + e^{-} \to K$ $- 2.92$
$L i^{+} + e^{-} \to L i$ $- 3.05$

- 712 k J

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- 240 k J

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250 k J

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730 k J

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Solution

The correct option is A $- 712 k J$
We have,
$E^{0}$ for $A l = - 1.66 V$ and $E^{0}$ for $A g = 0.80 V$

$E_{c e l l}^{0} = 0.8 - (- 1.66) = 2.46 V$

Now,
$Δ G^{0} = - n F E_{c e l l}^{0}$

$Δ G^{0} = - 3 \times 96500 \times 2.46$

$Δ G^{0} = - 712170 J = 712 k J$ .

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Similar questions

Q. Rank the following elements by increasing ease of oxidation with most easily oxidized LAST:

C d, C u, N i, F e

Standard Reduction Potentials at

25^{\circ} C

Half-Reaction	$E^{\circ} (V)$
$F_{2} + 2 e^{-} \to 2 F^{-}$	$2.87$
$A g^{2} + e^{-} \to A g^{+}$	$1.99$
$C o^{3 +} + e^{-} \to C o^{2 +}$	$1.82$
$H_{2} O_{2} + 2 H^{+} + 2 e^{-} \to 2 H_{2} O$	$1.78$
$M n O_{4}^{-} + 4 H^{+} + 3 e^{-} \to M n O_{2} + 2 H_{2} O$	$1.68$
$2 e^{-} + 2 H^{+} + I O_{4}^{-} \to I O_{3}^{-} + H_{2} O$	$1.60$
$M n O_{4}^{-} + 8 H^{+} + 5 e^{-} \to M n^{2 +} + 4 H_{2} O$	$1.51$
$A u^{3 +} + 3 e^{-} \to A u$	$1.50$
$C l_{2} + 2 e^{-} \to 2 C l^{-}$	$1.36$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$	$1.23$
$M n O_{2} + 4 H^{+} + 2 e^{-} \to M n^{2 +} + 2 H_{2} O$	$1.21$
$B r_{2} + 2 e^{-} \to 2 B r^{-}$	$1.09$
$N O_{3}^{-} + 4 H^{+} + 3 e^{-} \to N O + 2 H_{2} O$	$0.96$
$C l O_{2} + e^{-} \to C l O_{2}$	$0.954$
$2 H g^{2 +} + 2 e^{-} \to H g_{2}^{2 +}$	$0.91$
$A g^{+} + e^{-} \to A g$	$0.80$
$H g_{2}^{2 +} + 2 e^{-} \to 2 H g$	$0.80$
$F e^{3 +} + e^{-} \to F e^{2 +}$	$0.77$
$O_{2} + 2 H^{+} + 2 e^{-} \to H_{2} O_{2}$	$0.68$
$M n O_{4}^{-} + e^{-} \to M n O_{4}^{2 -}$	$0.56$
$I_{2} + 2 e^{-} \to 2 I^{-}$	$0.54$
$C u^{+} + e^{-} \to C u$	$0.52$
$O_{2} + 2 H_{2} O + 4 e^{-} \to 4 O H^{-}$	$0.40$
$C u^{2 +} + 2 e^{-} \to C u$	$0.34$
$A g C l + e^{-} \to A g + C l^{-}$	$0.22$
$C u^{2 +} + e^{-} \to C u^{+}$	$0.16$
$2 H^{+} + 2 e^{-} \to H_{2}$	$0.00$
$F e^{3 +} + 3 e^{-} \to F e$	$- 0.036$
$P b^{2 +} + 2 e^{-} \to P b$	$- 0.13$
$N i^{2 +} + 2 e^{-} \to N i$	$- 0.23$
$C d^{2 +} + 2 e^{-} \to C d$	$- 0.40$
$F e^{2 +} + 2 e^{-} \to F e$	$- 0.44$
$C r^{3 +} + e^{-} \to C r^{2 +}$	$- 0.50$
$C r^{3 +} + 3 e^{-} \to C r$	$- 0.73$
$Z n^{2 +} + 2 e^{-} \to Z n$	$- 0.76$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$	$- 0.83$
$M n^{2 +} + 2 e^{-} \to M n$	$- 1.18$
$A l^{3 +} + 3 e^{-} \to A l$	$- 1.66$
$H_{2} + 2 e^{-} \to 2 H^{-}$	$- 2.23$
$M g^{2 +} + 2 e^{-} \to M g$	$- 2.37$
$N a^{+} + e^{-} \to N a$	$- 2.71$
$C a^{2 +} + 2 e^{-} \to C a$	$- 2.76$
$B a^{2 +} + 2 e^{-} \to B a$	$- 2.90$
$K^{+} + e^{-} \to K$	$- 2.92$
$L i^{+} + e^{-} \to L i$	$- 3.05$

Q. Consider a galvanic cell using solid

C u

and

F e

metals with their corresponding solutions.
What is the

E_{c e l l}^{\circ}

Standard Potential (V)	Reduction Half-Reaction
$2.87$	$F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q)$
$1.51$	$M n O_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \to M n^{2 +} (a q) + 4 H_{2} O (l)$
$1.36$	$C l_{2} (a q) + 3 e^{-} \to 2 C l^{-} (a q)$
$1.33$	$C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q) + 7 H_{2} O (l)$
$1.23$	$O_{2} (g) + 4 H^{+} (a q) + 4 e^{-} \to 2 H_{2} O (l)$
$1.06$	$B r_{2} (l) + 2 e^{-} \to 2 B r^{-} (a q)$
$0.96$	$N O_{3}^{-} (a q) + 4 H^{+} (a q) + 3 e^{-} \to N O (g) + H_{2} O (l)$
$0.80$	$A g^{+} (a q) + e^{-} \to A g (s)$ $
$0.77$	$F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q)$
$0.68$	$O_{2} (g) + 2 H^{+} (a q) + 2 e^{-} \to H_{2} O_{2} (a q)$
$0.59$	$M n O_{4}^{-} (a q) + 2 H_{2} O (l) + 3 e^{-} \to M n O_{2} (s) + 4 O H^{-} (a q)$
$0.54$	$I_{2} (s) + 2 e^{-} \to 2 I^{-} (a q)$
$0.40$	$O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)$
$0.34$	$C u^{2 +} (a q) + 2 e^{-} \to C u (s)$
$0$	$2 H^{+} (a q) + 2 e^{-} \to H_{2} (g)$
$- 0.28$	$N i^{2 +} (a q) + 2 e^{-} \to N i (s)$
$- 0.44$	$F e^{2 +} (a q) + 2 e^{-} \to F e (s)$
$- 0.76$	$Z n^{2 +} (a q) + 2 e^{-} \to Z n (s)$
$- 0.83$	$2 H_{2} O (l) + 2 e^{-} \to H_{2} (g) + 2 O H^{-} (a q)$
$1.66$	$A l^{3 +} (a q) + 3 e^{-} \to A l (s)$
$- 2.71$	$N a^{+} (a q) + e^{-} \to N a (s)$
$- 3.05$	$L i^{+} (a q) + e^{-} \to L i (s)$

Q. Consider a spontaneous electrochemical cell between

C u

and

A l

. Predict what would happen if excess concentrated

N a O H

were added to the cell with copper ions and a precipitate forms.

Standard Potential (V)	Reduction Half-Reaction
$2.87$	$F_{2} (g) + 2 e^{-} \to 2 F^{-} (a q)$
$1.51$	$M n O_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \to M n^{2 +} (a q) + 4 H_{2} O (l)$
$1.36$	$C l_{2} (a q) + 3 e^{-} \to 2 C l^{-} (a q)$
$1.33$	$C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q) + 7 H_{2} O (l)$
$1.23$	$O_{2} (g) + 4 H^{+} (a q) + 4 e^{-} \to 2 H_{2} O (l)$
$1.06$	$B r_{2} (l) + 2 e^{-} \to 2 B r^{-} (a q)$
$0.96$	$N O_{3}^{-} (a q) + 4 H^{+} (a q) + 3 e^{-} \to N O (g) + H_{2} O (l)$
$0.80$	$A g^{+} (a q) + e^{-} \to A g (s)$ $
$0.77$	$F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q)$
$0.68$	$O_{2} (g) + 2 H^{+} (a q) + 2 e^{-} \to H_{2} O_{2} (a q)$
$0.59$	$M n O_{4}^{-} (a q) + 2 H_{2} O (l) + 3 e^{-} \to M n O_{2} (s) + 4 O H^{-} (a q)$
$0.54$	$I_{2} (s) + 2 e^{-} \to 2 I^{-} (a q)$
$0.40$	$O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)$
$0.34$	$C u^{2 +} (a q) + 2 e^{-} \to C u (s)$
$0$	$2 H^{+} (a q) + 2 e^{-} \to H_{2} (g)$
$- 0.28$	$N i^{2 +} (a q) + 2 e^{-} \to N i (s)$
$- 0.44$	$F e^{2 +} (a q) + 2 e^{-} \to F e (s)$
$- 0.76$	$Z n^{2 +} (a q) + 2 e^{-} \to Z n (s)$
$- 0.83$	$2 H_{2} O (l) + 2 e^{-} \to H_{2} (g) + 2 O H^{-} (a q)$
$1.66$	$A l^{3 +} (a q) + 3 e^{-} \to A l (s)$
$- 2.71$	$N a^{+} (a q) + e^{-} \to N a (s)$
$- 3.05$	$L i^{+} (a q) + e^{-} \to L i (s)$