Question

2Ag + H2S ? Ag2S + H2 Which statement is true about this chemical equation? A) Ag (silver) is oxidized and H (hydrogen) is reduced. B) Ag (silver) is reduced and H (hydrogen) is oxidized. C) S (sulfur) is reduced and H (hydrogen) is oxidized. D) S (sulfur) is oxidized and Ag (silver) is reduced.

Answer 1

Answer:

It is A).

Explanation:

Silver (Ag) goes from the  pure metal to Ag+ losing 1 electron so it is oxidised.

The hydrogen ion  gains electrons and is reduced.

Answer 2

Answer: The correct answer is Option A.

Explanation:

Oxidation reaction is defined as the chemical reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

$X\rightarrow X^{n+}+ne^-$

Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

$X^{n+}+ne^-\rightarrow X$

For the given chemical reaction:

$2Ag+H_2S\rightarrow Ag_2S+H_2$

The half cell reactions for the above reaction follows:

Oxidation half reaction:  $Ag\rightarrow Ag^{+}+e^-$

Reduction half reaction:  $2H^{+}+2e^-\rightarrow H_2$

As, silver is loosing 1 electron to form silver cation. Thus, it is getting oxidized. Hydrogen is gaining 2 electrons to form hydrogen atom. Thus, it is getting reduced.

Hence, the correct answer is Option A.