In alkaline medium ClO2 , oxidizes H2O2 to O2 and itself gets reduced to Cl- , How many moles of H2O2 are oxidised by 2 mole of ClO2?

Question

In alkaline medium ClO2 , oxidizes H2O2 to O2 and itself gets reduced to Cl- , How many moles of H2O2 are oxidised by 2 mole of ClO2? (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

The balanced chemical equation is: 2ClO2+5H2O2+2OH- overset arrow 2Cl-+5O2+6H2O 1molClO2=2.5molH2O22molClO2=5molH2O2

Q. In alkaline medium $Cl O_{2}$ , oxidizes $H_{2} O_{2}$ to $O_{2}$ and itself gets reduced to $C l^{-}$ , How many moles of $H_{2} O_{2}$ are oxidised by $2$ mole of $Cl O_{2} ?$

The balanced chemical equation is:
$2 Cl O_{2} + 5 H_{2} O_{2} + 2 O H^{-} \to 2 C l^{-} + 5 O_{2} + 6 H_{2} O$
$1 m o lCl O_{2} = 2.5 m o l H_{2} O_{2} 2 m o lCl O_{2} = 5 m o l H_{2} O_{2}$

Q. In alkaline medium ClO2​ , oxidizes H2​O2​ to O2​ and itself gets reduced to Cl− , How many moles of H2​O2​ are oxidised by 2 mole of ClO2​?

The balanced chemical equation is: 2ClO2​+5H2​O2​+2OH−→2Cl−+5O2​+6H2​O 1molClO2​=2.5molH2​O2​2molClO2​=5molH2​O2​

Q. In alkaline medium $Cl O_{2}$ , oxidizes $H_{2} O_{2}$ to $O_{2}$ and itself gets reduced to $C l^{-}$ , How many moles of $H_{2} O_{2}$ are oxidised by $2$ mole of $Cl O_{2} ?$

The balanced chemical equation is:
$2 Cl O_{2} + 5 H_{2} O_{2} + 2 O H^{-} \to 2 C l^{-} + 5 O_{2} + 6 H_{2} O$
$1 m o lCl O_{2} = 2.5 m o l H_{2} O_{2} 2 m o lCl O_{2} = 5 m o l H_{2} O_{2}$