Liquid hexane
CH3CH24CH3
will react with gaseous oxygen
O2
to produce gaseous carbon dioxide
CO2
and gaseous water
H2O
. Suppose 6.0 g of hexane is mixed with 32.3 g of oxygen.
Calculate the minimum mass of hexane that could be left over by the
chemical reaction. Be sure your answer has the correct number of
significant digits.
Balanced equation is
2CH3(CH2)4CH3 + 19O2 --------> 12CO2 + 14H2O
Number of moles of hexane = 6.0g / 86.18 g/mol = 0.0696 mole
Number of moles of O2 = 32.3 g / 32.0 g/mol = 1.009 mole
from the balanced equation we can say that
2 mole of hexane requires 19 mole of O2 so
0.0696 mole of hexane will require
= 0.0696 mole of hexane *(19 mole of O2 / 2 mole of hexane)
= 0.6612 mole of O2
but we have 1.009 mole of O2 which is in excess so O2 is excess reactant
and hexane is the limiting reactant so no amount of hexane will be left over in this reaction.
Get Answers For Free
Most questions answered within 1 hours.