Question

In alkaline medium ClO2 oxidized H2O2 toO2 and itself gets reduce Cl-.how many mole of H2O2 are oxidized by 1mole ClO2.

Answer 1

Answer on Question #48578 - Chemistry – Inorganic Chemistry

Question

In alkaline medium $\mathrm{ClO}_2$ oxidized $\mathrm{H}_2\mathrm{O}_2$ to $\mathrm{O}_2$ and itself gets reduce $\mathrm{Cl}^-$, how many mole of $\mathrm{H}_2\mathrm{O}_2$ are oxidized by 1 mole $\mathrm{ClO}_2$.

Answer:

Ionic equation for this redox reaction is:

$$\mathrm{ClO}_2 + \mathrm{H}_2\mathrm{O}_2 + \mathrm{OH}^- \rightarrow \mathrm{O}_2 + \mathrm{Cl}^- + \mathrm{H}_2\mathrm{O}$$

Half-reaction of reduction and oxidizing processes are:

$$\mathrm{Cl}^{+4} + 5\mathrm{e} = \mathrm{Cl}^- \quad 2$$ $$2\mathrm{O}^- - 2\mathrm{e} = \mathrm{O}_2^{0} \quad 5$$

Then we put this coefficients to the reaction equation and balance it:

$$2\mathrm{ClO}_2 + 5\mathrm{H}_2\mathrm{O}_2 + 2\mathrm{OH}^- = 5\mathrm{O}_2 + 2\mathrm{Cl}^- + 6\mathrm{H}_2\mathrm{O}$$

According to the balanced reaction, 2 moles of $\mathrm{ClO}_2$ oxidize 5 moles of $\mathrm{H}_2\mathrm{O}_2$, or 1 mole of $\mathrm{ClO}_2$ oxidizes 2.5 moles of $\mathrm{H}_2\mathrm{O}_2$.

Answer: 2.5 moles of $\mathrm{H}_2\mathrm{O}_2$

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