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Standard Electrode Potentials

Which of the ...

Question

Which of the following is/are true about the given shorthand notation of electrode potential?
$E_{C d (s) / C d^{2 +} (a q)}^{o} = 0.40 V$

Standard oxidation potential is

0.40 V

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Standard reduction potential is

0.40 V

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Electrode reaction is

C d^{2 +} (a q) + 2 e^{-} \to C d (s)

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None of the above

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Solution

The correct option is A Standard oxidation potential is $0.40 V$
Electrode potential for oxidation half cell reaction is called oxidation potential. The corresponding electrode is termed as negative electrode.

From the shorthand notation, it is clear that $C d (s)$ is oxidised to $C d^{2 +} (a q)$ at standard condition.
So, the oxidation half cell reaction is
$C d (s) \to C d^{2 +} (a q) + 2 e^{-}$

Hence, it is the standard oxidation potential of the electrode.

Suggest Corrections

Similar questions

(a) H g_{2}^{2 +} (a q) + 2 e^{-} ⇌ 2 H g (l)

(b) F e^{3 +} (a q) + e^{-} ⇌ F e^{2 +} (a q)

(a) C H_{3} C O O^{-} (a q) + 4 H_{2} O (a q) ⇌ 2 H C O_{3}^{-} (a q) + 9 H^{+} (a q) + 8 e^{-}

(b) C (s) + 2 H_{2} O (a q) ⇌ C O_{2} (a q) + 4 H^{+} (a q) + 4 e^{-}

F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = + 0.77 V

A l^{3 +} (a q) + 3 e^{-} \to A l (s); E^{0} = - 1.66 V

B r_{2} (g) + 2 e^{-} \to 2 B r^{-} (a q); E^{0} = + 1.08 V

F e_{(a q)}^{3 +} + e^{-} \to F e_{(a q)}^{2 +}

E^{o} = + 0.77

A l_{(a q)}^{3 +} + 3 e^{-} \to A l_{s}; E^{o} = - 1.66

B r_{2 (a q)} + 2 e^{-} \to 2 B r_{(a q)}^{-}; E^{o} = + 1.66

C d (N O_{3})_{2}

A g N O_{3}

E_{A g^{+} / A g}^{0} = 0.77 V a n d E_{C d^{2 +} / C d}^{0} = - 0.40

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