Question

If the percent yiled for the reaction 2CO + O2 = 2CO2 was 65.8% what mass of product in grams could be produced from a reactant mixture containing 35.0 grams of each reactant?

Answer 1

2CO + O2 ----> 2 CO2

Thus 2 moles of CO reacts with 1 mole of O2 gives 2 moles of CO2.

Moles = wt in g / mol. Wt. g/mol

35 g of CO = 35 g / 28.01 g/mol = 1.2496 mol.

And 35 g of O2 = 35 g / 16 g = 2.1875 mol.

Thus 1.2496 mol of CO reacts with 0.6248 mol of O2 to give 1.2496 mol of CO2.

Hence 1.2496 mol of CO2 = 1.2496 mol × 44.01 g/mol = 54.9949 g of CO2.

This is theoretical yield. Practical yield is 65.8% . Thus 65.8% of 54.9949 g CO2 is = 36.19 g of CO2.

Thus reaction produces 36.19 g of CO2.