Question

The following reaction does not proceed to a product: H2O + Ag --> no reaction. Why is that?

A) The reaction proceeds too slowly too create products.


B) The reaction cannot occur because water is reactant.


C) Silver has a higher activity than hydrogen and cannot replace it.


D) Silver has a lower activity than hydrogen and cannot replace it.

Answer 1

Silver has lower reactivity than hydrogen and cannot replace it

Step-by-step explanation:

took test

Answer 2

D - Silver has lower reactivity than hydrogen and cannot replace it

Step-by-step explanation:

If we assume , Ag also reacts just like other metals as

Metal + H₂O ---> Metal Hydroxide + H₂

then Ag forms as

Ag + H2O ----->AgOH +
`(1)/(2)`H2

here Ag is converting into Ag⁺ and 2H⁺ are converting into H₂

for reaction Ag --->Ag⁺ + e⁻ E° = -0.799 V

for reaction H⁺ + e⁻ ---->
`(1)/(2)`H₂ E° = 0 V

by Adding those 2 above equations net E° will be -0.799 which is negative.As per Faradays Law

ΔG° = -nFE°

here we got E° as negative then ΔG° will be positive

As per thermodynamics if ΔG° is +ve then reaction is not feasible

so, then given reaction does not occur.....