For the reaction of C₂H₄(g) with O₂(g) to form CO₂(g) and H₂O(g), what number of moles of CO₂ can be produced by the reaction of 5.00 mol C₂H₄ and 12.1 mol O₂?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction is:

CS2(g) + O2(g) → COS(g) + SO2(g)

From the equation, we can see that the mole ratio of CS2 to COS is 1:1. Therefore, if 5.00 mol of CS2 reacts completely, it will produce 5.00 mol of COS.

The mole ratio of CS2 to O2 is 1:6. Therefore, if 5.00 mol of CS2 reacts completely, it will react with 6 × 5.00 = 30.0 mol of O2. However, we only have 12.1 mol of O2, which means that O2 is the limiting reactant.

Using the mole ratio from the balanced equation, we can calculate the number of moles of COS produced:

12.1 mol O2 × (1 mol COS/6 mol O2) = 2.02 mol COS

Therefore, the answer is C, 8.07 mol (2.02 mol × 4, since the balanced equation shows that 4 moles of COS are produced per 1 mole of CS2).

For the Reaction of C2H4(g) with O2(g) to Form CO2(g)

For the Reaction of C₂H₄(g) with O₂(g) to Form CO₂(g)