2C2H6+7O2=4CO2+6H2O

how many moles of H2O are produced when a mixture of 0.427 moles of O2 and 0.150 moles of C2H6 is burned, iv already found moles of H2O for them separately.

To find the number of moles of H2O produced when a mixture of 0.427 moles of O2 and 0.150 moles of C2H6 is burned, you need to determine the limiting reactant first.

To determine the limiting reactant, you compare the ratio of moles of the reactants to the stoichiometric coefficients in the balanced equation.

The balanced equation is:
2C2H6 + 7O2 → 4CO2 + 6H2O

From the balanced equation, you can see that the stoichiometric ratio between O2 and H2O is 7:6, while the stoichiometric ratio between C2H6 and H2O is 2:6.

Firstly, let's find the moles of H2O produced from 0.427 moles of O2:
Using the ratio 7:6 from the balanced equation,
(0.427 moles O2) * (6 moles H2O / 7 moles O2) = 0.3674 moles H2O

Secondly, let's find the moles of H2O produced from 0.150 moles of C2H6:
Using the ratio 2:6 from the balanced equation,
(0.150 moles C2H6) * (6 moles H2O / 2 moles C2H6) = 0.450 moles H2O

Since 0.3674 moles of H2O is produced from the O2 and 0.450 moles of H2O is produced from the C2H6, the limiting reactant is O2 because it produces a lesser amount of H2O.

Therefore, when the mixture of 0.427 moles of O2 and 0.150 moles of C2H6 is burned, the number of moles of H2O produced is 0.3674 moles.