How many electrons are involved in the following redox reaction ?
\(\mathrm{Cr_2O_7^{2-}+Fe^{2+}+C_2O_4^{2-}}\)
\(\rightarrow \mathrm{Cr^{3+}+Fe^{3+}+CO_2}\) (Unbalanced)
\(\mathrm{Cr_2O_7^{2-}+Fe^{2+}+C_2O_4^{2-}}\)
\(\rightarrow \mathrm{Cr^{3+}+Fe^{3+}+CO_2}\) (Unbalanced)
Show Hint
- 3
- 4
- 6
- 5
The Correct Option is C
Solution and Explanation
Oxidation: \(\mathrm{Fe^{2+}\rightarrow Fe^{3+}+e^-}\) and \(\mathrm{C_2O_4^{2-}\rightarrow 2CO_2+2e^-}\).
Balanced: \(\mathrm{Cr_2O_7^{2-}+2Fe^{2+}+2C_2O_4^{2-}+14H^+\rightarrow2Cr^{3+}+2Fe^{3+}+4CO_2+7H_2O}\), where \(2\times1+2\times2=6\) electrons are lost.
Electrons involved = 6.
Answer: (3) 6
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