In alkaline medium ClO2 oxidises H2O2 to O2 and itself gets reduced to Cl-, X moles of H2O2 are oxidised by 1 mole of ClO2 . Calculate 2X ?

Question

In alkaline medium ClO2 oxidises H2O2 to O2 and itself gets reduced to Cl-, X moles of H2O2 are oxidised by 1 mole of ClO2 . Calculate 2X ? (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

The balanced chemical equation is 2ClO2​+5H2O2​+2OH- arrow 2Cl-+5O2​+6H2O 2molClO2​=5molH2O2​ 1molClO2 ​=2.5molH2O2​2X=2× 2.5=5

Q. In alkaline medium $Cl O_{2}$ oxidises $H_{2} O_{2}$ to $O_{2}$ and itself gets reduced to $C l^{-},$ $X$ moles of $H_{2} O_{2}$ are oxidised by $1$ mole of $Cl O_{2}$ . Calculate $2 X$ ?

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

Q. In alkaline medium ClO2​ oxidises H2​O2​ to O2​ and itself gets reduced to Cl−, X moles of H2​O2​ are oxidised by 1 mole of ClO2​ . Calculate 2X ?

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

Q. In alkaline medium $Cl O_{2}$ oxidises $H_{2} O_{2}$ to $O_{2}$ and itself gets reduced to $C l^{-},$ $X$ moles of $H_{2} O_{2}$ are oxidised by $1$ mole of $Cl O_{2}$ . Calculate $2 X$ ?

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