Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C3H7SH present.

The reaction between C3H7SH and oxygen can be illustrated using the following balanced equation:

C3H7SH (l) + 6O2 (g) - - > 3 CO2 (g) + SO2 (g) + 4 H2O (g)

From the balanced equation above, 6 moles of oxygen are required to produce 4 moles of water.

Therefore, to know the number of oxygen moles needed to produce 2.33 moles of water, all you have to do is cross multiplication as follows:

number of oxygen moles = (2.33*6) / 4 = 3.495 moles

Assuming that there is excess C3H7SH present, 6.21 moles of oxygen are required to produce 2.33 moles of water.