Question

Balance the following chemical equation under acidic conditions and provide the coefficients

Sb(s) +NO₃^-(aq) --> Sb₄O_{6 (s)} + NO (aq)

The coefficient for Sb is ________

The coefficient for NO₃^- is ____________

The coefficient for Sb₄O₆ is ______________

The coefficient for NO is ________

The coefficient for H₂O ____________ on the __________side (*type either: product or reactant)

The coefficient for H⁺ is __________on the ___________side (*type either: product or reactant)

Answer 1

This is a redox reaction. First balance the qxidation and reduction half reactions.

Oxidation half reaction

Sb is oxidized to Sb4O6(s). The oxidation no. of Sb is zero.To find the oxidation no. of Sb4O6, the following calculation is done.

Therfore, the half reaction for oxidation is as follows.

Now, we balance the oxygen atoms by adding water.

Then balance the hydrogen atoms by adding H+ (remeber that this happens in acidic conditions).

Now balance te charges by adding electrons.

Reduction half reaction

Similarly, balance the reduction half reaction.

Overall reaction

Now, all you have to do is combine the two reactions. REMEMBER to cancel out the electrons! The overall reaction can't have any electrons in it, so we have to multiply the reduction reaction by 4.

The overall reaction when these two are added;