Given is the unbalanced redox reaction: CrO2−4+SO2−3→CrO−2+SO2−4+OH− The balanced half reaction among the following is :
A
2CrO2−4+8H2O+6e−→2CrO−2+4H2O+8OH−
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B
2CrO2−4+8H2O→CrO−2+4H2O+8OH−
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C
CrO2−4+H2O→CrO−2+H2O+OH−
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D
3CrO2−4+4H2O+6e−→2CrO−2+8OH−
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Solution
The correct option is B2CrO2−4+8H2O+6e−→2CrO−2+4H2O+8OH− 2CrO2−4+8H2O+6e−→2CrO−2+4H2O+8OH− Here, the number of atoms of each type and charges on both sides (left
and right of the equation) are same so this is the balanced half reaction.