How many liters of CO2 at STP are produced from the complete combustion of 2.00 moles of C7H16?

Answer 1

Balanced equation.

C7H16 + 11O2 >> 7CO2 + 8H2O

2.00 moles C7H16 (7moles CO2/1mole C7H16) = 14 moles CO2

( I forget STP standard, so will use PV = nRT )

(1atm)(V) = (14moles CO2)(0.08206 Latm/molK)(273.15K)

Volume CO2 = 14 *0.08206*273.15/1

= 314 Liters CO2

Answer 2

Heptane is C7H12. Hydrocarbons burn to form CO2 and water. If we balance the equation we get

C7H12 + 10 O2 -> 7 CO2 + 6 H2O

We see that for every mole of heptane burned we get 7 moles of CO2. Therefore 2 moles of heptane would get us 14 moles of CO2.

1 mole of any gas at standard temperature and pressure (STP) is equal to 22.4 liters. Multiply 22.4 liters by 14 moles to get 313.6 liters of carbon dioxide.