2 C8H18(l) + 25 O2(g) #-># 16 CO2(g) + 18 H2O(g) If you burned one gallon of gas (C8H18) (approximately 4000 grams), how many liters of carbon dioxide would be produced at a temperature of 21.0°C and a pressure of 1.00 atm?
One gallon of octane produces approximately 7000 L of carbon dioxide.
Since the temperature in the problem is
Step1. You must first determine the number of moles that are in 4000 g of octane, using the molar mass of octane. Step 2. Then you must determine the number of moles of carbon dioxide that can be produced by that number of moles of octane, based on the mole ratio between octane and carbon dioxide in the balanced equation. Step 3. Then use the ideal gas law to determine the volume in liters of carbon dioxide that can be formed.
mass of octane = approximately 4000 g
pressure = 1.00 atm
molar mass of octane,
mole/mole ratio for
Balanced Chemical Equation:
Ideal Gas Law:
Step 1. Determine Moles of Octane in One Gallon
Step 2. Moles of Carbon Dioxide Produced by One Gallon of Octane
Multiply moles of octane times the mole/mole ratio between octane and carbon dioxide, so that carbon dioxide is in the numerator.
Step 3. Calculate Volume of
P = 1.00 atm
n = 280.1312 mol