In the following reaction, Zn is Zn(s) H2SO4(aq) --> ZnSO4(aq) H2(g) A. Reduced B. Oxidized C. This is not a redox reaction D. An oxidizing agent

The correct option is B) oxidized

Explanation:

Redox reaction is defined as the reaction in which oxidation and reduction take place simultaneously.

The oxidation reaction is defined as the reaction in which a chemical species loses electrons in a chemical reaction. It occurs when the oxidation number of a species increases.

A reduction reaction is defined as the reaction in which a chemical species gains electrons in a chemical reaction. It occurs when the oxidation number of a species decreases.

For the given chemical reaction:

On the reactant side:

Oxidation number of H = +1

Oxidation number of Zn = 0

Oxidation number of S = +6

Oxidation number of O = -2

On the product side:

Oxidation number of H = 0

Oxidation number of Zn = +2

Oxidation number of S = +6

Oxidation number of O = -2

As the oxidation number of Zn is increasing from 0 to +2. Thus, it is getting oxidized. Similarly, the oxidation number of H is decreasing from +1 to 0. Thus, it is getting reduced.

Hence, the correct option is B) oxidized

d.) the average kinetic energy of the gas particles is greater in container b because its particles move faster.