1 mol of ferric oxalate is oxidised by xmol of {MnO_4}^- in . . . - Toppr In acidic medium, two moles of permanganate oxidizes 5 moles of oxalic acid Also, 1 mole of permanganate oxidizes 5 moles of Fe (II) ions 1 mole of ferrous oxalate gives 1 mole of Fe (II) ions and 1 mole of oxalate ions It will require 1 5 moles of permanganate for the oxidation of Fe (II) ions and 2 5 moles of permanganate for the oxidation of oxalate ions Total permanganate required is 1
The initial concentration of { N }_ { 2 } { O }_ { 5 } in the first . . . The initial concentration of N 2O5 in the first order reaction N 2O5(g) 2N O2(g) + 1 2O2(g) was 1 1 24×10−2 mol L−1 at 318 K The concentration of N 2O5 after 60 minutes was 0 20×10−2molL−1 Calculate the rate constant of the reaction at 318 K