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Application of Electrolysis

Consider the ...

Question

Consider the following reduction processes:

$Z n^{2 +} + 2 e^{-} \to Z n (s); E^{o} = - 0.76 V$
$C a^{2 +} + 2 e^{-} \to C a (s); E^{o} = - 2.87 V$
$M g^{2 +} + 2 e^{-} \to M g (s); E^{o} = - 2.36 V$
$N i^{2 +} + 2 e^{-} \to N i (s); E^{o} = - 0.25 V$

The reducing power of the metals increases in the order:

A

C a < Z n < M g < N i

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B

N i < Z n < M g < C a

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C

Z n < M g < N i < C a

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D

C a < M g < Z n < N i

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Solution

The correct option is B $N i < Z n < M g < C a$
Lower the reduction potential , higher is the tendency of the species to get oxidised and hence better will be reducing power. So, according to the given data correct order will be:
$N i < Z n < M g < C a$

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Similar questions

Q. Consider the follwoing reduction processes :

Z n^{2 +} + 2 e^{-} \to Z n (s); E^{0} = - 0.76 V

C a^{2 +} + 2 e^{-} \to C a (s); E^{0} = - 2.87 V

M g^{2 +} + 2 e^{-} \to M g (s); E^{0} = - 2.36 V

N i^{2 +} + 2 e^{-} \to N i (s); E^{0} = - 0.25 V

The reducing power of the metals increases in the order :

Q. Consider the following processes:

Z n^{2 +} + 2 e^{-} \to Z n (s); E^{o} = - 0.76 V

C a^{2 +} + 2 e^{-} \to C a (s); E^{o} = - 2.87 V

M g^{2 +} + 2 e^{-} \to M g (s); E^{o} = - 2.36 V

N i^{2 +} + 2 e^{-} \to N i (s); E^{o} = - 0.25 V

The reducing power of the metals increases in the order:

Q. Consider the follwoing reduction processes :

Z n^{2 +} + 2 e^{-} \to Z n (s); E^{0} = - 0.76 V

C a^{2 +} + 2 e^{-} \to C a (s); E^{0} = - 2.87 V

M g^{2 +} + 2 e^{-} \to M g (s); E^{0} = - 2.36 V

N i^{2 +} + 2 e^{-} \to N i (s); E^{0} = - 0.25 V

The reducing power of the metals increases in the order :
(JEE MAIN 2019)

Q. The standard reduction potential of the half cells at

298 K

N i^{2 +} (a q) + 2 e^{-} \to N i (s); E^{o} = - 0.28 V

M g^{2 +} (a q) + 2 e^{-} \to M g (s); E^{o} = - 2.37 V

The standard cell potential for a voltaic cell constructed using the two half reaction is

Q. Standard reduction potentials of the half reactions are given below

F_{2 (g)} + 2 e^{-} \to 2 F_{(a q)}^{-}

E^{o} = + 2.85 V

C l_{2 (g)} + 2 e^{-} \to 2 C l_{(a q)}^{-}

E^{o} = + 1.36 V

B r_{2 (l)} + 2 e^{-} \to 2 B r_{(a q)}^{-}

E^{o} = + 1.06 V

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

E^{o} = + 0.53 V

The strongest oxidising and reducing agents respectively are:

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