The correct option is B 10:3
+2.5S4O2−6(aq)+0Al(s)→H2−2S(aq)++3Al3+(aq)
S4O2−6 is oxidising agent.
Al is reducing agent.
nf=(|O.S.Product−O.S.Reactant|×number of atom
+2.5S4O2−6(aq)→H2−2S(aq) oxidation
nf=(|−2−2.5|×4=18
0Al(aq)→+3Al3+(aq) reduction
nf=(|3−0|×1=3
Ratio of nf for oxidation to reduction is 6:1
Cross mutiply the oxidising and reducing agents with ratio of n-factors.
S4O2−6(aq)+6 Al(s)→H2S(aq)+Al3+(aq)
Balancing elements except O and H
S4O2−6(aq)+6Al(s)→4H2S(aq)+6Al3+(aq)
Balance atoms oxygen by adding H2O.
S4O2−6(aq)+6Al(s)→4H2S(aq)+6Al3+(aq)+6H2O(l)
Balance hydrogen by adding H+
S4O2−6(aq)+6Al(s)+20H+→4H2S(aq)+6Al3+(aq)+6H2O(l)
Balancing charge:
charge in reactant side = -2+20=+18
charge in product side = +18
so the balanced equation is:
S4O2−6(aq)+6Al(s)+20H+→4H2S(aq)+6Al3+(aq)+6H2O(l)
The coefficient of H+ is 20 and coefficient of H2O is 6.
Desired ratio:
20:6⇒10:3