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Number of moles of H+ ions required by 1 mole of MnO4- to oxidise oxalate ion to CO2 is .
8
2MnO4- + 5C2O42- + 16H+ 2Mn2+ + 10CO2 + 8H2O
∵ Mn: +7 → +2 (gains 5e-); C2O42- 2CO2 (loses 2e-)
⇒ MnO4- : C2O42- = 2 : 5
2 mol MnO4- need 16 mol H+ ⇒ 1 mol needs 8 mol
Answer: 8
2MnO4- + bI- + cH2O xI2 + yMnO2 + zOH- If the above equation is balanced with integer coefficients, the value of z is .
Total number of species from the following which can undergo disproportionation reaction is . H2O2, ClO3-, P4, Cl2, Ag, Cu+1, F2, NO2, K+
Chlorine undergoes disproportionation in alkaline medium as shown below : aCl2(g) + bOH-(aq) cClO-(aq) + dCl-(aq) + eH2O(l) The values of a, b, c and d in a balanced redox reaction are respectively :
From the given list, the number of compounds with +4 oxidation state of Sulphur . SO3, H2SO3, SOCl2, SF4, BaSO4, H2S2O7
Which of the following cannot function as an oxidising agent?