What mass of iron is needed to react with sulfer in order to produce 96 grand of Fe2S3 according to this equation: 2Fe + 3S = Fe2S3?

51.69g

Explanation:

2Fe + 3S —> Fe2S3

Molar Mass of Fe2S3 = (2x56) + (32x3) = 112 + 96 = 208g/mol

Molar Mass of Fe = 56g/mol

Mass conc. Of Fe = 2x56 = 112g

From the equation,

112g of Fe produced 208g of Fe2O3.

Therefore, Xg of Fe will produce 96g of Fe2O3 i.e

Xg of Fe = (112x96)/208 = 51.69g

"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."