Which of the following equations depict the oxidising nature of H2O2?

Question

Which of the following equations depict the oxidising nature of H2O2? (A) 2MnO4- + 6H+ + 5H2O2 → 2Mn2+ + 8H2O + 5O2 (B) 2Fe3+ + 2H+ + H2O2 → 2Fe2+ + 2H2O + O2 (C) 2I- + 2H+ + H2O2 → I2 + 2H2O (D) KIO4 + H2O2 → KIO3 + H2O + O2

Tardigrade Admin · Accepted Answer

Oxidising nature of H2O2 means it oxidises other substance and itself gets reduced. In such reactions O2 is not evolved. In (a), MnO4- gets reduced from Mn7+ to Mn2+. In (b), Fe3+ gets reduced to Fe2+. In (c), I- gets oxidised to I2. In (d), KIO4 gets reduced from I7+ to I5+ .

Q. Which of the following equations depict the oxidising nature of $H_{2} O_{2}$ ?

$2 M n O_{4}^{-} + 6 H^{+} + 5 H_{2} O_{2} \to 2 M n^{2 +} + 8 H_{2} O + 5 O_{2}$

$2 F e^{3 +} + 2 H^{+} + H_{2} O_{2} \to 2 F e^{2 +} + 2 H_{2} O + O_{2}$

$2 I^{-} + 2 H^{+} + H_{2} O_{2} \to I_{2} + 2 H_{2} O$

$K I O_{4} + H_{2} O_{2} \to K I O_{3} + H_{2} O + O_{2}$

Q. Which of the following equations depict the oxidising nature of H2​O2​?

2MnO4−​+6H++5H2​O2​→2Mn2++8H2​O+5O2​

2Fe3++2H++H2​O2​→2Fe2++2H2​O+O2​

2I−+2H++H2​O2​→I2​+2H2​O

KIO4​+H2​O2​→KIO3​+H2​O+O2​

Oxidising nature of H2​O2​ means it oxidises other substance and itself gets reduced. In such reactions O2​ is not evolved. In (a), MnO4−​ gets reduced from Mn7+ to Mn2+. In (b), Fe3+ gets reduced to Fe2+. In (c), I− gets oxidised to I2​. In (d), KIO4​ gets reduced from I7+ to I5+ .

Q. Which of the following equations depict the oxidising nature of $H_{2} O_{2}$ ?

$2 M n O_{4}^{-} + 6 H^{+} + 5 H_{2} O_{2} \to 2 M n^{2 +} + 8 H_{2} O + 5 O_{2}$

$2 F e^{3 +} + 2 H^{+} + H_{2} O_{2} \to 2 F e^{2 +} + 2 H_{2} O + O_{2}$

$2 I^{-} + 2 H^{+} + H_{2} O_{2} \to I_{2} + 2 H_{2} O$

$K I O_{4} + H_{2} O_{2} \to K I O_{3} + H_{2} O + O_{2}$