Question

The reaction of Fe3O4(s) with hydrogen(g) to form iron(s) and water(g) proceeds as follows: Fe3O4(s) + 4 H2(g) 3 Fe(s) + 4 H2O(g) When 61.8 grams of Fe3O4(s) react with sufficient H2(g) , 40.3 kJ of energy are absorbed . What is the value of H for the chemical equation given?

Answer 1

Answer: 151 kJ

Step-by-step explanation:

To calculate the moles :

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

`\text{Moles of} Fe_3O_4=(61.8g)/(231.5g/mol)=0.267moles`

`Fe_3O_4(s)+4H_2(g)\rightarrow 3Fe(s)+4H_2O(g)`

It is given that:

0.267 moles of
`Fe_3O_4` absorb energy = 40.3 kJ

Thus 1 mole of
`Fe_3O_4` absorb energy =
`(40.3)/(0.267)* 1=151kJ`

Thus the value of
`\Delta H` for the chemical equation given is 151 kJ