More active metals will cause the reduction of less active metals. Less active metals will cause no reaction (N. R.) in more active metals. What is the complete and balanced reaction of solid iron with aqueous zinc(II)? Use the following activity series to arrive at your

Activity of metals with most active and less active metals are given below.

Explanation:

1. Activity of metals -Divide metals Based on the activity.

2. The primary difference between metals is the ability with which they undergo chemical reactions. The elements toward the bottom left corner of the periodic table are the metals that are the most active in the sense of being the most reactive. Lithium, sodium, and potassium all react with water, for example. The rate of this reaction increases as we go down this column, however, because these elements become more active as they become more metallic.

3. Common Metals Divided into Classes on the Basis of Their Activity

4. The most active metals are so reactive that they readily combine with the O2 and H2O vapor in the atmosphere and are therefore stored under an inert liquid, such as mineral oil. These metals are found exclusively in Groups IA and IIA of the periodic table.

5. Metals in the second class are slightly less active. They don't react with water at room temperature, but they react rapidly with acids.

6.The third class contains metals such as chromium, iron, tin, and lead, which react only with strong acids. It also contains even less active metals such as copper, which only dissolves when treated with acids that can oxidize the metal.

7. Metals in the fourth class are so unreactive they are essentially inert at room temperature. These metals are ideal for making jewelry or coins because they do not react with the vast majority of the substances with which they come into daily contact. As a result, they are often called the "coinage metals."

Fe⁺² (aq)+Zn(s)=>Zn⁺² (aq)+Fe(s)

i believe the answer is true.