Half ReactionEoI- Mg- Mg 2- -2 e -2-37VII- Mn- Mn 2- -2 e -1-03VIII- H 2 - 2 H - -2 e -0-00VIV- Cu- Cu 2- -2 e -0-16VFrom the above experimental data which of the following represents a spontaneous process-

The correct option is D Mg+ Mn ^ 2+ → E^0_A=(0.00 1.03)= 1.03 V E^0_B=(2.37 1.03)=1.34 V E^0_C=(1.03 2.37)= 1.34 V E^0_D=( 0.16 0.0 ...

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Byju's Answer

Standard XII

Chemistry

Redox Reactions and Couple

Half Reaction...

Question

Half Reaction Eo
I. $M g \to {M g}^{2 +} + 2 e^{-}$ 2.37V
II. $M n \to {M n}^{2 +} + 2 e^{-}$ 1.03V
III. $H_{2} \to 2 H^{+} + 2 e^{-}$ 0.00V
IV. $C u \to {C u}^{2 +} + 2 e^{-}$ -0.16V
From the above experimental data which of the following represents a spontaneous process?

{M n}^{2 +} + H_{2} \to

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M g + {M n}^{2 +} \to

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{M g}^{2 +} + M n \to

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C u + 2 H^{+} \to

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{M g}^{2 +} + C u \to

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Solution

The correct option is D $M g + {M n}^{2 +} \to$
$E_{A}^{0} = (0.00 - 1.03) = - 1.03 V$
$E_{B}^{0} = (2.37 - 1.03) = 1.34 V$
$E_{C}^{0} = (1.03 - 2.37) = - 1.34 V$
$E_{D}^{0} = (- 0.16 - 0.00) = - 0.16 V$
$E_{E}^{0} = (- 0.16 - 2.37) = - 2.53 V$

Reaction is feasible if $E^{0}$ is positive. Therefore, only reaction B is possible.

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Similar questions

Half Reaction	Eo
I. $M g \to {M g}^{2 +} + 2 e^{-}$	2.37V
II. $M n \to {M n}^{2 +} + 2 e^{-}$	1.03V
III. $H_{2} \to 2 H^{+} + 2 e^{-}$	0.00V
IV. $C u \to {C u}^{2 +} + 2 e^{-}$	-0.16V

From the above experimental data what will be the standard reduction potential which represents spontaneous process?

Q. Refer to the following experimental data.

Half Reaction	Eo
I. $M g \to {M g}^{2 +} + 2 e^{-}$	2.37V
II. $M n \to {M n}^{2 +} + 2 e^{-}$	1.03V
III. $H_{2} \to 2 H^{+} + 2 e^{-}$	0.00V
IV. $C u \to {C u}^{2 +} + 2 e^{-}$	-0.16V

What will be the standard reduction potential for the reaction:

M g + M n^{2 +} \to M g^{2 +} + M n

Q. Refer to the following experimental data.

Half Reaction	$E_{o}$
I. $M g \to {M g}^{2 +} + 2 e^{-}$	2.37V
II. $M n \to {M n}^{2 +} + 2 e^{-}$	1.03V
III. $H_{2} \to 2 H^{+} + 2 e^{-}$	0.00V
IV. $C u \to {C u}^{2 +} + 2 e^{-}$	-0.16V

Which of the following reactions is spontaneous?

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. Find the

△ G^{\circ}

of a galvanic cell with

A g

and

A l

Standard Reduction Potentials at

25^{\circ} C

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

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Half ReactionEoI. Mg→Mg2++2e−2.37VII. Mn→Mn2++2e−1.03VIII. H2→2H++2e−0.00VIV. Cu→Cu2++2e−-0.16VFrom the above experimental data which of the following represents a spontaneous process?

The correct option is D Mg+Mn2+→E0A=(0.00−1.03)=−1.03 VE0B=(2.37−1.03)=1.34 VE0C=(1.03−2.37)=−1.34 VE0D=(−0.16−0.00)=−0.16 VE0E=(−0.16−2.37)=−2.53 VReaction is feasible if E0 is positive. Therefore, only reaction B is possible.

Half Reaction Eo
I. $M g \to {M g}^{2 +} + 2 e^{-}$ 2.37V
II. $M n \to {M n}^{2 +} + 2 e^{-}$ 1.03V
III. $H_{2} \to 2 H^{+} + 2 e^{-}$ 0.00V
IV. $C u \to {C u}^{2 +} + 2 e^{-}$ -0.16V
From the above experimental data which of the following represents a spontaneous process?