Write balanced chemical equation for the following reactions: Dic…

Question

Write balanced chemical equation for the following reactions:
Dichlorine heptaoxide ($Cl_2O_7$) in gaseous state combines with an aqueous solution of hydrogen peroxide in acidic medium to give chlorite ion ($ClO^–_2$) and oxygen gas.
(Balance by ion electron method)

✓

Answer

$\text{Cl}_2\text{O}_7(\text{g})+4\text{H}_2\text{O}_2(\text{aq})\xrightarrow{ \ \ \ \ \ \ \ }2\text{ClO}^-_2(\text{aq})+3\text{H}_2\text{O(l)}+4\text{O}_2(\text{g})+2\text{H}^+(\text{aq})$
Balancing by ion-electron method:
Oxidation half:
$\text{H}_2\text{O}_2\xrightarrow{ \ \ \ \ \ \ \ }\text{O}_2+2\text{e}^-$
Adding $2H^+$ on right side to balance H atoms and charge.
$\text{H}_2\text{O}_2\xrightarrow{ \ \ \ \ \ \ \ }\text{O}_2+2\text{H}^++2\text{e}^-$
Reduction half:
$\text{Cl}_2\text{O}_7+8\text{e}^-\xrightarrow{ \ \ \ \ \ \ \ }2\text{ClO}^-_2$
Adding $H_2O$ and $H^+$ to balance H and O atoms
$\text{Cl}_2\text{O}_7+8\text{e}^-+6\text{H}^+\xrightarrow{ \ \ \ \ \ \ \ \ }2\text{ClO}^-_2+3\text{H}_2\text{O}$
Adding oxidation and reduction half
$[\text{H}_2\text{O}_2\xrightarrow{ \ \ \ \ \ \ }\text{O}_2+2\text{e}^-+2\text{H}^+]\times4 \\ \text{Cl}_2\text{O}_7+8\text{e}^-+6\text{H}^+\xrightarrow{ \ \ \ \ \ \ \ }2\text{ClO}^-_2+3\text{H}_2\text{O} \\ \underline{ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ } \\ \text{Cl}_2\text{O}_7+4\text{H}_2\text{O}_2\xrightarrow{ \ \ \ \ \ \ \ }2\text{ClO}^-_2+3\text{H}_2\text{O}+4\text{O}_2+2\text{H}^+$

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