Question

For the given reaction,

$3Fe\left(s\right)+x{H}_{2}O\left(l\right)\to F{e}_3{O}_4\left(s\right)+4H_2\left(l\right)$

What should be the value of x so that it is balanced?

Answer 1

A balanced chemical equation has an equal number of atoms of each element in reactants and products. [0.5 mark]

Consider the coefficients of Fe as 'A', ${\text{H}}_2\text{O}$ as 'B', ${\text{Fe}}_3{\text{O}}_4$ as 'C' and ${\text{H}}_2$ as 'D'.

Given, A = 3, C = 1 and D = 4
On comparining the number of each element in both sides we get, 2B = 2D
2B = 2$\times$4
$⟹$B = 4 [1 mark]
Since, B = $x$ Therefore, $x$ = 4 [0.5 mark]