An iron ore samp;le contains Fe2O3 plus other impurities. A 752-g sample of impure iron ore is heated with excess carbon, producing 453 g of pure iron by the following reaction: Fe2O3 (s) + 3C(s) ----2Fe (s) + 3CO(g). what is the mass percent of Fe2O3 in the impure iron ore sample? Assume Fe2O3 is the only source of iron and that the reaction is 100% efficient.
Fe2O3 (s) + 3C(s) →2Fe (s) + 3CO(g) (2*55.847 + 3*15.999) g Fe2O3 → 2*55.847 g Fe 159.691 g Fe2O3 → 111.694 g Fe 1.429719 g Fe2O3 → 1.0 g Fe 647.6626 g Fe2O3 → 453 g Fe (647.6626)(100)/752 ≈ 86.125% ≈ 86.1%
Someone who wanted to torture all the wives of soccer playing, soccer watching, soccer coaching fanatical men!
Someone who wanted to torture all the wives of soccer playing, soccer watching, soccer coaching fanatical men!
Fe2O3 (s) + 3C(s) →2Fe (s) + 3CO(g) (2*55.847 + 3*15.999) g Fe2O3 → 2*55.847 g Fe 159.691 g Fe2O3 → 111.694 g Fe 1.429719 g Fe2O3 → 1.0 g Fe 647.6626 g Fe2O3 → 453 g Fe (647.6626)(100)/752 ≈ 86.125% ≈ 86.1%
