Question

The reduction of iron(III) oxide to iron metal is an endothermic process: Fe2O3(s) + 2 CO(g) → 2 Fe(s) + 3 CO2(g) ΔH = +26.3 kJ How many kilojoules of energy are required to produce 1.00 kilogram of iron metal?

Answer 1

Answer: Thus 234 kJ of energy are required to produce 1.00 kilogram of iron metal

Explanation:

To calculate the number of moles , we use the equation:

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$  

Putting values , we get:

$\text{Moles of iron}=\frac{1000g}{56g/mol}=17.8moles$    (1.00kg=1000g)

The balanced chemical reaction is:

$Fe_2O_3(s)+2CO(g)\rightarrow 2Fe(s)+3CO_2(g)$   $\Delta H=+26.3kJ$

Given :

Energy released when 2 moles of $Fe$ is produced = 26.3 kJ

Thus Energy released when 17.8 moles of $Fe$ is produced =

= $\frac{26.3kJ}{2}\times 17.8=234kJ$

Thus 234 kJ of energy are required to produce 1.00 kilogram of iron metal