Question

Consider the following reaction: How many moles of oxygen are required to produce 14.0 moles of water? Assume that there is excess C₃H₇SH present.

C₃H₇SH(D) + O₂(g) -> CO₂(g) + SO₂(g) + 4 H₂O(g)

Answer 1

To produce 14.0 moles of water, you would need 3.5 moles of oxygen.

Step-by-step explanation:

The balanced equation for the reaction is:

C₃H₇SH(D) + O₂(g) -> CO₂(g) + SO₂(g) + 4 H₂O(g)

From the equation, we can see that 1 mole of C₃H₇SH reacts with 1 mole of O₂ to produce 4 moles of H₂O. Therefore, to produce 14.0 moles of water, we would need 3.5 moles of oxygen (14.0 moles/4 = 3.5 moles).