Question

Mno4_so2 mn2+ +hso4 in acidic reaction

Answer 1

Answer:

Well the reduction is relatively easy, and it proceeds with a dramatic colour change from purple to colourless…

$Mn(+VII)→Mn(+II) …$

$MnO−4+8H++5e−→Mn2++4H2O$

And sulfur dioxide is OXIDIZED to bisulfate, i.e

$S(+IV)→S(+VI) …</p><p></p><p>SO2+2H2O→HSO−4+3H++2e−$

We take TWO of the former and FIVE of the latter…

$2MnO−4+16H++5SO2+10H2O+10e−→2Mn2++8H2O+5HSO−4+15H++10e−$

And we cancel away….

$2MnO−4+H++5SO2+2H2O→2Mn2++5HSO−4$

Which I think is balanced with respect to mass and charge…but it is your problem mate…. And what would we observe in the reaction? The deep purple-red colour of permanganate dissipates to give colourless

$Mn2+ ion…$