Balance the following reaction- Cr2O2-7 - C2H4O - H- - C2H4O2 - Cr3-

The correct option is C Cr_2O^2 _7 + 3C_2H_4O + 8H^+ → 3C_2H_4O_2 + 2Cr^3+ + 4H_2O The unbalanced redox equation is as follows: Cr_2O^2 _7 + C_2H_4O + ...

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Byju's Answer

Standard XII

Chemistry

Introduction to Oxidation and Reduction

Balance the f...

Question

Balance the following reaction.

$C r_{2} O_{7}^{2 -} + C_{2} H_{4} O + H^{+} \to C_{2} H_{4} O_{2} + C r^{3 +}$

C r_{2} O_{7}^{2 -} + 3 C_{2} H_{4} O + 8 H^{+} \to 3 C_{2} H_{4} O_{2} + 2 C r^{3 +} + 4 H_{2} O

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C r_{2} O_{7}^{2 -} + C_{2} H_{4} O + 8 H^{+} \to 3 C_{2} H_{4} O_{2} + 5 C r^{3 +} + H_{2} O

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C r_{2} O_{7}^{2 -} + 4 C_{2} H_{4} O + 4 H^{+} \to C_{2} H_{4} O_{2} + 2 C r^{3 +} + 4 H_{2} O

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Solution

The correct option is C $C r_{2} O_{7}^{2 -} + 3 C_{2} H_{4} O + 8 H^{+} \to 3 C_{2} H_{4} O_{2} + 2 C r^{3 +} + 4 H_{2} O$
The unbalanced redox equation is as follows:
$C r_{2} O_{7}^{2 -} + C_{2} H_{4} O + H^{+} \to C_{2} H_{4} O_{2} + C r^{3 +}$
Balance all atoms other than H and O.
$C r_{2} O_{7}^{2 -} + C_{2} H_{4} O + H^{+} \to C_{2} H_{4} O_{2} + 2 C r^{3 +}$
The oxidation number of Cr changes from 6 to 3. So the change in oxidation number of one Cr atom is 3.
For 2 Cr atoms, the oxidation number changes by 6.
The oxidation number of C changes from -1 to 0. So the change in oxidation number of 1 C atom is 1.
For 2 C atoms, the oxidation number changes by 2.
The increase in the oxidation number is balanced with decrease in the oxidation number by multiplying
$C_{2} H_{4} O$ and $C_{2} H_{4} O_{2}$ with 3.
$C r_{2} O_{7}^{2 -} + 3 C_{2} H_{4} O + H^{+} \to 3 C_{2} H_{4} O_{2} + 2 C r^{3 +}$

O atoms are balanced by adding 4 water molecules on RHS.
$C r_{2} O_{7}^{2 -} + 3 C_{2} H_{4} O + H^{+} \to 3 C_{2} H_{4} O_{2} + 2 C r^{3 +} + 4 H_{2} O$
Hydrogen atoms are balanced by adding 7 $H^{+}$ atoms on RHS.
$C r_{2} O_{7}^{2 -} + 3 C_{2} H_{4} O + 8 H^{+} \to 3 C_{2} H_{4} O_{2} + 2 C r^{3 +} + 4 H_{2} O$
This is the balanced chemical equation.

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Similar questions

Q. Balance the following equation by ion electron method:

C r_{2} O_{7}^{2 -} + C_{2} H_{4} O + H^{+} \to 2 C r^{3 +} + C_{2} H_{4} O_{2} + H_{2} O

Balance the following equations:

C r_{2} O_{7}^{2 -} + I^{-} + H^{+} \to C r^{3 +} + I_{2} + H_{2} O

Q. Calculate the electrode potential at

25^{\circ} C

C r^{+ 3}, C r_{2} O_{7}^{2 -}

electrode at

p O H = 11

in a solution of

0.01 M

both in

C r^{3 +}

and

C r_{2} O_{7}^{2 -}

C r_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{-} \to 2 C r^{3 +} + 7 H_{2} O

E^{\circ} = 1.33 V

Q. Which of the following does not/do not represent the correct equivalent mass of

C r_{2} O_{7}^{2 -}

in the reaction

C r_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{-} 2 C r^{3 +} + 7 H_{2} O

Q. Balance the following equation by ion electron method:

C r_{2} O_{7}^{2 -} + C_{2} H_{4} O + H^{+} \to 2 C r^{3 +} + C_{2} H_{4} O_{2} + H_{2} O

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Balance the following reaction.Cr2O2−7+C2H4O+H+→C2H4O2+Cr3+

Balance the following reaction.

$C r_{2} O_{7}^{2 -} + C_{2} H_{4} O + H^{+} \to C_{2} H_{4} O_{2} + C r^{3 +}$