Question

Iron metal is made from iron ore in a blast furnace, were this chemical reaction occurs: Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) (a) Is this a redox equation? State why it is or why it is not. (b) If 175 kg of iron ore (Fe2O3) is reacted with excess carbon monoxide (CO), what is the theoretical yield (amount in kg) of iron metal (Fe)? (c) If the actual yield of iron metal is 109 kg, what is the percent yield?

Answer 1

Ans. Pego z 39 + 3 Cog 2 Fe (s) + 360, (g) @ indicatina gidation number Oz + 3 co2 pe t3co +3 -2 + 2-2 O so +3 sen Reduction +2 14 3 Co 3002 oxidation this redox reaction As both half reaction of reduction and exidation is to be written 175 kg of reg, so Pe o mols = 175 Kg 159.69 gm/mol z1095.87 mol from balanced reaction male of Pe produced zgx mold reg

= 2 x (1095.87) mol 2191-746 mol Theonetied mass of Fe 219 6. Tub Bobaly 55.847 gh mol 2 122.402 Kg Actual 2 Log Kg of Iron yield percent yield log Kg 122.402 xloo y z lang 0.8908oxlos y z 0 2 89.05./.