How do I do this? please help?

Question

calculate how many moles of the second reactant would be required to react completely with 5.00 mol of the first reactant

C2H6(g) + O2(g)-->CO2(g) + H2O(g)

all numbers are supposed to be subscripts.

Please explain how to get the answer if you can! cuz i don't understand it at all! thanks

Answer 1

balance the equation
2C2H6 + 7O2 -> 4CO2 + 6H2O

Then do
5 mol / 2 * 7 = 17.5 mol

2 is the coefficient of C2H6 and 7 is coefficient of O2

Answer 2

I suppose 5.00 mole of the first reactant would be C2H6.

2C2H6 + 7O2 ===> 4CO2 + 6H2O

5.00molC2H6 x 7molO2/2molC2H6 = 17.5 moles O2

First, you must balance the equation. Beginning wigh 5.00 C2H6, the first factor cancels the moles C2H6, giving the moles O2.

Answer 3

FIRST OF ALL BALANCE THE EQUATION

2C2H6 + 7O2 -> 4CO2 + 6H2O

From the above equation:
5 mol / 2 * 7 = 17.5 mol