26. Complete and balance the following equation:

2. $\mathrm{Fe}+\hspace{0.17em}{\mathrm{H}}_2{\mathrm{SO}}_4$

Step 1: Write the skeletal chemical equation

Iron (Fe), an active metal reacts with Sulphuric acid $\left({\mathrm{H}}_2{\mathrm{SO}}_4\right)$ to form Iron (II) sulphate $\left({\mathrm{FeSO}}_4\right)$, a metallic salt and Hydrogen gas $\left({\mathrm{H}}_2\right)$. The skeletal chemical equation for the reaction is as follows:

$\underset{\mathrm{Iron}}{\mathrm{Fe}\left(\mathrm{s}\right)}+\hspace{0.17em}\underset{\mathrm{Sulphuric}\mathrm{acid}}{{\mathrm{H}}_2{\mathrm{SO}}_4\left(\mathrm{aq}\right)}\to \underset{\mathrm{Iron}\left(\mathrm{II}\right)\hspace{0.17em}\mathrm{sulphate}}{{\mathrm{FeSO}}_4\left(\mathrm{aq}\right)}+\underset{\mathrm{Hydrogen}}{{\mathrm{H}}_2\left(\mathrm{g}\right)}$

Step 2: Determine the number of atoms of each element on both sides of the equation

For balancing the equation, both reactants and products should be balanced on both the sides.

Reactant	Product
$\mathrm{Fe}=1$	$\mathrm{Fe}=1$
$\mathrm{H}=2$	$\mathrm{H}=2$
$\mathrm{S}=1$	$\mathrm{S}=1$
$\mathrm{O}=4$	$\mathrm{O}=4$

Since the number of atoms of each element are equal on both sides of the equation thus, it is said to be balanced.

Conclusion:

Therefore, the balanced chemical equation for the given reaction is as follows:

$\underset{\mathrm{Iron}}{\mathrm{Fe}\left(\mathrm{s}\right)}+\hspace{0.17em}\underset{\mathrm{Sulphuric}\mathrm{acid}}{{\mathrm{H}}_2{\mathrm{SO}}_4\left(\mathrm{aq}\right)}\to \underset{\mathrm{Iron}\left(\mathrm{II}\right)\hspace{0.17em}\mathrm{sulphate}}{{\mathrm{FeSO}}_4\left(\mathrm{aq}\right)}+\underset{\mathrm{Hydrogen}}{{\mathrm{H}}_2\left(\mathrm{g}\right)}$