Answer:
2Ag (s) + 2HNO₃ (aq) 2AgNO₃ (aq) + H₂ (g)
Explanation:
2Ag (s) + 2HNO₃ (aq) 2AgNO₃ (aq) + H₂ (g)
Ag is below H₂ in reactivity series. Therefore Ag does not spontaneously replace H₂ from any compound.
Answer:
The answer to the question is
2Ag (s) +2HNO₃ (aq) →2AgNO₃ (aq)+ H₂ (g)
Explanation:
The position of a cell on the reduction potential table determines if a reduction reaction will be spontaneous
The higher the positive reduction potential the higher the spontaneity of the reduction reaction. that is if the E⁰ cell is positive the cell is a spontaneous voltaic cell, however if the E⁰ cell is negative the cell is a electrolytic non-spontaneous cell
On the standard potential table silver has a low positive potential of
Ag⁺ + e⁻ → Ag = 0.799
It is an oxidizing agent tending to scarcely release electrons, therefore for the reaction to take place, there has to be some external supply of electromotive force.
