2C14H30 (l) + 45O2 (g) -> 28CO2 (g) + 30H2O (g)
When zinc metal is dropped into a solution of copper (II) nitrate, a redox reaction occurs. Zinc metal is oxidized, losing electrons, while copper (II) ions are reduced, gaining electrons. The reaction can be represented as:
Zn (s) + Cu(NO3)2 (aq) -> Zn(NO3)2 (aq) + Cu (s)
In this reaction, zinc metal acts as a reducing agent, donating electrons to copper (II) ions, while copper (II) ions act as an oxidizing agent, accepting electrons from zinc metal.
