COLLEGE CHEMISTRY 35 POINTS
Determine the percent yield when 12 g of CO2 are formed experimentally from the reaction of 0.5 moles of C8H18 reacting with excess oxygen according to the following balanced equation:

2 C8H18(l) + 25 O2(g)  16 CO2(g) + 18 H2O(l)

Please show your work.

6.81% is the percent yield when 12 g of CO2 are formed experimentally from the reaction of 0.5 moles of C8H18 reacting with excess oxygen.

Explanation:

Data given:

mass of carbon dioxide formed = 12 grams (actual yield)

atomic mass of CO2 = 44.01 grams/mole

moles of = 0.5

Balanced chemical reaction:

2 + 25 ⇒ 16 C + 18

number of moles of carbon dioxide given is

number of moles =

number of moles=

number of moles of carbon dioxide gas = 0.27 moles

from the reaction 2 moles of reacts to produce 16 moles of C

So, when 0.5 moles reacted it produces x moles

=

x = 4

4 moles of carbon dioxide formed, mass from it will give theoretical yield.

mass  = number of moles x molar mass

mass = 4 x 44.01

        = 176.04 grams

percent yield = x 100

percent yield = x 100

     percent yield  = 6.81 %