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

Step-by-step 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}=(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 =

=
`(26.3kJ)/(2)* 17.8=234kJ`

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