In the following reaction, how many liters of oxygen will produce 15.67 liters of CO2 at STP? C2H4 (g) + 3O2 (g) 2CO2 (g) + 2H2O (g)

5.22 liters

7.84 liters

10.45 liters

23.50 liters

88.00 liters

We solve for the number of mols of CO2 given its volume, assuming that it is an ideal gas.

n = PV / RT

Substituting,

n = (1 atm) (15.67 L) / (0.082 L. atm/mol. K) (273.15 K) = 0.7 moles

From the balanced chemical reaction above, we determine the number of O2 moles needed to produce 0.7 moles CO2.

0.7 moles CO2 x (3 moles O2 / 2 moles CO2) = 1.05 moles O2

Then, we multiply this value by 22.4 L/mol

1.05 moles O2 x (22.4 L / mol) = 23.52 L O2

Thus, the answer is the fourth choice.