Which species in each of the following pairs is better reducing agent under standard state conditions. $E^{0}$ values are given. Give reasons for your ?

K (s) (- 2.93 V)

M g (s) (- 2.36 V)

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C o^{2 +} (a q) (1.81 V)

I n (s) (- 0.14 V)

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C e^{3 +} (a q) (1.61 V)

T i^{2 +} (- 0.37 V)

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H g (l) (0.86 V)

N i (s) (- 0.23 V)

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Solution

The correct option is B $K (s) (- 2.93 V)$ or $M g (s) (- 2.36 V)$
Reducing agent Based upon reduction potential higher negative value in electro chemical series in A option K and Mg has high negative values of reduction potential.so better reducing agent is K than Mg.

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Which species in each of the following pairs is better reducing agent under standard state conditions. E0 values are given. Give reasons for your ?

The correct option is B K(s)(−2.93 V) or Mg(s)(−2.36 V)Reducing agent Based upon reduction potential higher negative value in electro chemical series in A option K and Mg has high negative values of reduction potential.so better reducing agent is K than Mg.

Which species in each of the following pairs is better reducing agent under standard state conditions. $E^{0}$ values are given. Give reasons for your ?

The correct option is B $K (s) (- 2.93 V)$ or $M g (s) (- 2.36 V)$
Reducing agent Based upon reduction potential higher negative value in electro chemical series in A option K and Mg has high negative values of reduction potential.so better reducing agent is K than Mg.