Saved Bookmarks
| 1. |
Balance the following redox reactions by ion electon mehtod (a) MnO_(4)^(-)+I^(-)(aq)rarrMnO_(2)(s)+I_(2) (in basic medium) (brgt (b)MnO_(4)^(-)(aq)+SO_(2)(g)rarrMn^(2+)(aq)+HSO_(4)^(-)(in acidic solution ) (c ) H_(2)O_(2)(aq)+Fe^(32+)(aq)rarrFe^(3+)(aq)+H_(2)O(l) (in acidic solution) (d) Cr_(2)O_(7)^(2-)(aq)+SO_(2)(g)rarrCr^(3+)(aq)+SO_(4)^(2-)(aq) (ion acidic solution) |
|
Answer» Solution :(B) following the genal procedure for ion electron method detailed onthe BALANCED half reactionare oxidationhalf equation`SO_(2)(g)+2H_(2)O(l)rarrHSO_(4)^(-)(aq)+3H^(+)(aq)+2e^(-)` reductin half equation : `MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-)rarrMn^(2+)(aq)+4 H_(2)O(l)` (C ) oxidation half equation `Fe^(2+)(aq)rarrFe^(3+)(aq)+e^(-)` Multiply eq (i) by 2 and add it to eq (ii) we have `H_(2)O_(2)(aq)+2Fe^(2+)(aq)+2H^(+)(aq)rarr2Fe^(3+)(aq)+2H_(2)O(l)` (d) following the general procedurefor ion electron detailed on the balanced half reaction equation are Oxidation half equation`SO_(2)(g)+2H_(2)O(l)rarrSO_(4)^(2-)(aq)+4H^(+)(aq)+2e^(-)` multiply eq (i) by 3 and add it to eq (ii) we have `Cr_(2)O_(7)^(2)(aq)+3 SO_(2)(q)+2H^(+)(aq)+2H^(+)(aq)rarr2Cr^(3+)(aq)+3SO_(4)^(2-)(aq)+H_(2)O(l)` |
|