What mass of iron must react to produce
3600 kJ of energy? 3Fe+2O2 →Fe3O4 ∆H=-1120kJ
the mass is 537.9 g youre welcome
-1120KJ/3 mols of Fe= 3600 KJ/x mol
= 538g
To find the mass of iron required to produce a certain amount of energy, we need to use the balanced chemical equation and the enthalpy change (∆H) value provided.
The given equation is: 3Fe + 2O2 → Fe3O4
The enthalpy change (∆H) for this reaction is -1120 kJ. This means that the reaction releases 1120 kJ of energy.
We are given that the reaction will release 3600 kJ of energy.
Now, we can set up a proportion to find the mass of iron required:
(Change in energy)/(∆H) = (Change in mass)/(molar mass of Fe)
Since the ratio of the energy released is 3600 kJ and -1120 kJ, and the molar mass of Fe is 55.85 g/mol, we can set up the proportion as follows:
(3600 kJ)/(-1120 kJ) = (Change in mass)/(55.85 g)
Simplifying the equation:
(3600 kJ) * (55.85 g) = (-1120 kJ) * (Change in mass)
199,260 kJ · g = -1,254,400 kJ · mol
Now, we can multiply both sides of the equation by -1 to get a positive value for the mass:
-199,260 kJ · g = 1,254,400 kJ · mol
Dividing both sides of the equation by 1,254,400 kJ · mol:
-199,260 kJ · g / 1,254,400 kJ · mol = 1 mol
Now, we have the molar mass of iron:
-0.159 g/mol = 1 mol
To find the mass of iron required, we can multiply the molar mass by the number of moles required, which is 1:
-0.159 g/mol × 1 mol = -0.159 g
Therefore, the mass of iron required to produce 3600 kJ of energy is approximately 0.159 grams.