Question

14. (1 point per blank) Iron ore, Fe2O3 (s), reacts with C (s) in a blast furnace to form Fe (s) and CO (g) The balanced reaction for the process is: The substance being oxidized is The substance reduced is In order to make 1510 grams of Fe (s) with 100% yield, one needs to grams of Fe2O3 (s) and use grams of C (s).

Answer 1

22 WALL solution (14) The Fe₂O₂ and can be written as reaction reaction between be Fe₂O₃ + c Fe +co +2 Balance reaction Fe₂O₃ +30 - 2Fe +300 +3 c. get oxidized and RezOg get reduced, Fe From equation ③ we see that moles of of Fe2O₃ produce a Since I mole and imple of Fe₂O3 Ž 3nd of c Therefore Mol of Fe produced by I mol of Fe2O3 and 3 mol of No. of mol of Fe = mass of fe Modlar mas of Fe - 1510g - 26.96 mol 56 g/mol 1. No.of mot of Fe2O3 required = 26.96 a 13:48 mel. mass of PegO3 = 13.48 mol x 159.69 g/mol molar mass of Fea 22152.62 ~ 2153 g #

And No. of mol. of c required - 3 mol of Fe 23 22 x 26.96 mot. 2 uo.u4 mol. . mars of c required a 4o.uumol x 12 Jmol. 2485.28 g ~ 4 85.3 g # Thus. reaction for the The balanced process is +30 2Fe +3co. The substance being oxidized is Ciss The substance being reduced is Fez 03 (8) In order to make 1510 grams a Fels) with 100%. Yield one needs to use 2153 grams of Fez 03 (8) and 485.3 grams. f CCs).