The combustion of liquid ethanol (c2h5oh) produces carbon dioxide and water. after 4.60 ml of ethanol (density=0.789g/ml) was allowed to burn in the presence of 15.50 g of oxygen gas, 3.70 ml of water (density=1.00g/ml) was collected.
a) determine the limiting reactant for the reaction. (hint: write a balanced equation for the combustion of ethanol.)
b) determine the theoretical yield of h2o for the reaction.
c) determine the percent yield of h2o for the reaction.

a. Ethanol.

b. 4.21 mL H2O.

c. 87.8%

Explanation:

Hello,

- For the limiting reactant, the available amount of ethanol is less than the ideal amount of ethanol that would react with the given amount of oxygen, that's why it is the limiting one.

- You will find the calculations in the attached picture; take into account that the molecular mass of water is 18 g/mol and ethanol 46 g/mol.

- The percent yield is allowed to be computed in terms of volume as well, because the relationships are conserved.

Best regards!

it takes on an electronical energy