Fe₃o₄ reacts with co according to the equation
fe₃o₄ + co --> fe + co₂ (unbalanced)
if 478.9 g fe₃o₄ is reacted with excess co, what mass of co₂ will be produced assuming 100% yield?
1. 91.02 g co₂
2. 182.05 g co₂
3. 364.1 g co₂
4. none of these
5. 273.1 g co₂

Option 3.

364.1 g of CO₂ are produced by the reaction

Explanation:

Let's verify the balance equation for this reaction:

Fe₃O₄  +   4 CO  →  3 Fe   +   4CO₂

Let's convert the mass of Fe₃O₄ to moles (mass / molar mass)

478.9 g / 231.55 g/mol  = 2.07 moles

Ratio is 1:4, so let's make a rule of three to determine the moles of CO₂ produced and then its mass.

1 mol of Fe₃O₄ is needed to produce 4 moles of CO₂

Then, 2.07 moles of Fe₃O₄ will produce (2.07  .4) /1 = 8.27 moles of CO₂.

Molar mass . moles = mass

44 g/mol . 8.27 mol = 364 g of CO₂

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."