Question

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.

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

	6.21 moles O2
	3.50 moles O2
	4.14 moles O2
	2.33 moles O2
	1.55 moles O2

Answer 1

Ans :- Option (b) is the correct answer i.e.  Moles of oxygen required = 3.50 mol

Explanation :-

Given balanced chemical reaction is :

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

1 mol...........................6 mol...............3 mol................1 mol..........................4 mol (Reacting moles)

From the balanced chemical equation, it is cleared that

4 moles of water are formed from = 6 moles of oxygen

So,

1 moles of Water are formed from = 6/4 moles of Oxygen

and

2.33 moles of Water are formed from = 6 x 2.33 / 4 moles of Oxygen = 3.495 moles of Oxygen = 3.50 moles

Hence, Moles of oxygen required = 3.50 mol