In the reaction, $C_{2} O_{4}^{2 -}$ $\to$ $C O_{2}$ , the total number of electrons lost per mole of $C_{2} O_{4}^{- 2}$ is

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Solution

The correct option is B
2N

Oxidation state of ‘C’ in $C_{2} O_{4}^{2 -} = + 3$ & Oxidation state of ‘C’ in $C O_{2} = + 4$

Change in oxidation state of ‘C’ = 4 – 3 = 1

Since there are two ‘C’ atoms in $C_{2} O_{4}^{2 -}$ ; Number of electrons transferred = 2 x 1 = 2 e

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Similar questions

In the reaction, $C_{2} O_{4}^{2 -}$ $\to$ $C O_{2}$ , the total number of electrons lost per mole of $C_{2} O_{4}^{- 2}$ is

For the redox reaction
$M n O_{4}^{-} + C_{2} O_{4}^{- 2} + H^{+} ⟶ M n^{2 +} + C O_{2} + H_{2} O$
the correct coefficients of the reactants $M n O_{4}^{-}, C_{2} O_{4}^{2 -} a n d H^{+}$ for the balanced reaction are

Q. For the redox reaction,

M n O_{4,}^{-} + C_{2} O_{4}^{2 -} + H^{+} \to M n^{2 +} + C O_{2} + H_{2} O

the correct coefficients of the reactants for the balanced reaction are respectively

M n O_{4,}^{-} + C_{2} O_{4}^{-} + H^{+} :

Q. The total number of moles of

C O_{2}

evolved in following reaction per mole of compounds' is?

For the redox reaction
MnO−4+C2O−24+H+⟶Mn2++CO2+H2O
the correct coefficients of the reactants MnO−4, C2O2−4 and H+ for the balanced reaction are

2, 5, 16

16, 5, 2

5, 16, 2

2, 16, 5

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In the reaction, C2O2−4 → CO2 , the total number of electrons lost per mole of C2O−24 is

The correct option is B 2N Oxidation state of ‘C’ in C2O2−4=+3 & Oxidation state of ‘C’ in CO2=+4 Change in oxidation state of ‘C’ = 4 – 3 = 1 Since there are two ‘C’ atoms in C2O2–4 ; Number of electrons transferred = 2 x 1 = 2 e

In the reaction, $C_{2} O_{4}^{2 -}$ $\to$ $C O_{2}$ , the total number of electrons lost per mole of $C_{2} O_{4}^{- 2}$ is

The correct option is B
2N

Oxidation state of ‘C’ in $C_{2} O_{4}^{2 -} = + 3$ & Oxidation state of ‘C’ in $C O_{2} = + 4$

Change in oxidation state of ‘C’ = 4 – 3 = 1

Since there are two ‘C’ atoms in $C_{2} O_{4}^{2 -}$ ; Number of electrons transferred = 2 x 1 = 2 e