Question

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

$2\mathrm{Mg}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{x}\right)\to 2\mathrm{MgO}\left(\mathrm{y}\right)$

Answer 1

Step 1: Balanced chemical equations

Chemical equations that obey the law of conservation of mass are called balanced chemical equations. The number of atoms of all the elements on the reactant side will be equal to that on the product side for a balanced equation. Equations are balanced using the trial and error method.

The states of all the reactants and products are also mentioned in a balanced chemical equation.

Step 2: Finding x and y

The reaction represents the burning of Magnesium $\left(\mathrm{Mg}\right)$. In this reaction, Magnesium is heated in the presence of Oxygen gas $\left({\mathrm{O}}_2\right)$. Therefore, Oxygen is in the gaseous state represented by the alphabet g.

Therefore, x = g.

The product formed from burning Magnesium is Magnesium oxide $\left(\mathrm{MgO}\right)$. Magnesium oxide is formed by the oxidation of Magnesium and is in the solid-state.

Therefore, y = g.

Then, the balanced equation for the burning of magnesium is given below:

$$\begin{gathered} 2\mathrm{Mg}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to 2\mathrm{MgO}\left(\mathrm{s}\right) \\ \left(\mathrm{Magnesium}\right)\left(\mathrm{Oxygen}\right)(\mathrm{Magnesium}\mathrm{oxide}) \end{gathered}$$