# Fe2O3(s) + 3CO(g)  2Fe(s) + 3CO2(g), a)The reaction is started with 40.0 g of Fe2O3 and 60.0 g of CO. Indicate the limiting reagent.?

4. Iron ore containing Fe2O3 is converted into iron according to the following reaction: Fe2O3(s) + 3CO(g)  2Fe(s) + 3CO2(g) a) The reaction is started with 40.0 g of Fe2O3 and 60.0 g of CO. Indicate the limiting reagent. b) What is the theoretical yield of Fe? c) If the actual yield of Fe was 20.0 g, calculate the percent yield of the reaction. Atomic weights Fe: 55.9; O: 16.0; C; 12.0
Answers

pisgahchemist

Smelting of iron ore ..... To cover (a) and (b), calculate the amount of Fe using each reactant. The lesser of the two is the theoretical yield and tells the limiting reactant. Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g) 40.0g ......... 60.0g ........?g 40.0g Fe2O3 x (1 mol Fe2O3 / 159.6g Fe2O3) x (2 mol Fe / 1 mol Fe2O3) x (55.8g Fe / 1 mol Fe) = 28.0g Fe 60.0g CO x (1 mol CO / 28.0g CO) x (2 mol Fe / 3 mol CO) x (55.8g Fe / 1 mol Fe) = 79.7g Fe The theoretical yield is 28.0g Fe, and Fe2O3 is the limiting reactant. Percent yield = 20.0g / 28.0g x 100 = 71.4%