Question

If 4.50 moles of C2H6 undergoes combustion, how many moles of oxygen would it combust with?

Answer 1

To combust 4.50 moles of C2H6, you would need 15.75 moles of O2.

Step-by-step explanation:

In the combustion of C2H6, the balanced equation is:

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

From the balanced equation, we can see that for every 2 moles of C2H6 combusted, we need 7 moles of O2. Therefore, if we have 4.50 moles of C2H6, we would need:

(7 moles O2 / 2 moles C2H6)(4.50 moles C2H6) = 15.75 moles of O2

Answer 2

First balance the equation

C2H6 + 7/2O2 2CO2 +3H2O

for one mole of C2H6 there are 7/2 mole of O2 required. so for4.50 moles you require 4.50 x 7/2 = 15.75 moles of O2.

Step-by-step explanation: