The number of "OH" - ions in the balanced equation of \(MnO_{4}(aq) + I^{-}(aq) \rightarrow MnO_{2}(s)+I_{2}(s)\)

The number of Fe^(2+) ion oxidised by one mole of MnO_(4)^(-) ions is:

Balancing the following redox reactions by ion-electron method. \(MnO_{4}^{-1}+SO_{2} (g) \rightarrow Mn^{2+}+HSO_{4}^{-}\) ( in Acid medium )

In acidic medium, potassium manganate undergoes disproportionation according to equation.\(3MnO_{4}^{2-}+4H^{+}\rightarrow 2MnO_{4}^{-}+MnO_{2}+2H_{2}O\) Equivalent weight of \(K_{2}MnO_{4}\) will be (Mol.wt.of \(K_{2}MnO_{4}\)=M)

Balance the following rebox reactions by ion electron method: a. MnO_(4)^(Θ)(aq)+I^(Θ)(aq) rarr MnO_(2)(s)+I_(2)(s) (in basic medium) b. MnO_(4)^(Θ)(aq)+SO_(2)(g) rarr Mn^(2+)(aq)+HSO_(4)^(Θ)(aq) (in acidic solution) c. H_(2)O_(2)(aq)+Fe^(2+)(aq) rarr Fe^(3+)(aq)+H_(2)O(l) (in acidic solution) d. Cr_(2)O_(7)^(2-)+SO_(2)(g) rarr Cr^(3+)(aq)+SO_(4)^(2-)(aq) (in acidic solution)

Use the given standard reduction potentials to determine the reduction potential for this half-reactions. MnO_(4)^(-)(aq) + 3e^(-) + 4H^(+) rightarrow MnO_(2)(S) + 2H_(2)O(l)

Complete the chemical equations : MnO_4^(-) (aq) + S_2O_3^(2-)(aq) + H_2O (l) to

Complete the chemical equations : MnO_4^(-) (aq) + H_2O_2(aq) + H^(+)(aq) to