Question

Write proper symbols for x and y in the following chemical equations:

$\mathrm{Fe}\left(\mathrm{x}\right)+{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)\to {\mathrm{Fe}}^{2+}+\mathrm{Zn}\left(\mathrm{y}\right)$

Answer 1

Balanced chemical equations

Chemical equations that have the same number of atoms of all the elements on the reactant side and product side and thus obey the law of conservation of mass are called balanced chemical equations. These equations are used to determine the relative amount of reactants required for a complete reaction.

The states of the reactants and products are represented in a balanced chemical equation using symbols s, l, and g for solids, liquids, and gases respectively. The aqueous state is represented as ‘aq’.

Finding x and y

In the given reaction, Iron $\left(\mathrm{Fe}\right)$ reacts with Zinc ions $\left({\mathrm{Zn}}^{2+}\right)$ to form Zinc $\left(\mathrm{Zn}\right)$ and Ferrous ions $\left({\mathrm{Fe}}^{2+}\right)$. The reaction is an example of a redox reaction in which Iron is oxidized and Zinc ions are reduced.

Iron is solid metal. Therefore, it is represented using the symbol ‘s’.

Therefore, x = s.

When Zinc ions are reduced into Zinc, it is displaced from the solution and deposited in their metallic state. Zinc metal is solid and is represented by symbol ‘s’.

Therefore, y = s.

Therefore, the balanced chemical equation can be given as:

$$\begin{gathered} \mathrm{Fe}\left(\mathrm{s}\right)+{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)\to {\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)+\mathrm{Zn}\left(\mathrm{s}\right) \\ \left(\mathrm{Iron}\right)(\mathrm{Zinc}\mathrm{ion})(\mathrm{Ferrous}\mathrm{ion})\left(\mathrm{Zinc}\right) \end{gathered}$$