Given the balanced combustion reaction: 2C2H6 + 7O2 --> 4CO2 + 6H2O What is the total mass of C2H6 that will react to produce 72 grams of H2O

2C2H6(g) + 7O2(g) ==> 4CO2(g) + 6H2O(g)

One way to find the limiting reactant is to divide the moles of reactant by the corresponding coefficient in the balanced equation and whichever is less is limiting.

For C2H6 we have 2 moles / 2 = 1

For O2 we have 8 moles / 7 = 1.14

Explanation:

If a reaction mixture contains 8 moles of O2(g) with 2 moles of C2H6(g),which reactant is the limiting reactqnt and what is the mass (in grams) remaining of the reactant in excess?

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