Liquid hexane CH3CH24CH3 reacts with gaseous oxygen gas O2 t

Liquid hexane (CH3CH24CH3) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide CO2 and gaseous water (H2O. If 104.g of water is produced from the reaction of 79.28g of hexane and 559.3g of oxygen gas, calculate the percent yield of water. Be sure your answer has the correct number of significant digits in it.

Solution

The balanced reaction will be

C6H14 + 9.5O2 -------- 6CO2 + 7H2O

Number of moles of water produced = Mass/molar mass = 104./18 = 5.77777778 moles

1 mole of C6H14 gives 7 moles of water

Molar mass of Hexane (C6H14) = 6 * 12 + 14 * 1 = 86 gm/mol

Number of moles of Hexane = Mass/molar mass = 79.28/86 = 0.92186 moles

Percentage Yield = actual Yield/ Theoritical Yield

=> 5.7777778/(0.92186 * 7)

=> 89.53%