Question

Read the following chemical equations.

Reaction 1: H2S+Cl->2HCl+S
Reaction 2: Fe+S->FeS

Which of the following statements if true for both the chemical equations?

A) Chlorine is reduced in reaction 1 and iron is reduced 2

B) chlorine is oxidized in reaction 1 and iron is oxidized in reaction 2

C) chlorine is oxidized in reaction 1 and iron is reduced in reaction 2

D) Chlorine is reduced in reaction 1 and iron is oxidized in reaction 2

Answer 1

D) Chlorine is reduced as hydrogen is added whereas Iron is oxidised as Joins with a non hydrogen compound.

Answer 2

In the given reactions, Chlorine has been reduced in the first reaction, while Iron has been oxidized in the second reaction. Thus, option D is correct.

The redox reaction has been termed the oxidation and reduction reaction. The reduction reaction can be given as the gain of electrons while the oxidation reaction can be given as the loss of electrons.

Since the first reaction, chlorine has been present in the free state with the ions having a negative charge. The bond formation between hydrogen and chlorine results in the gain of hydrogen electrons by chlorine. Thus, chlorine has been reduced in the first reaction.

The Iron has been the reducing agent in the reaction, thus with the loss of electrons, Iron reduces sulfur and gets oxidized itself. Thus, iron has been oxidized in the reaction.

In the given reactions, Chlorine has been reduced in the first reaction, while Iron has been oxidized in the second reaction. Thus, option D is correct.

For more information about oxidation and reduction, refer to the link:

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