1. Stoichiometry and the combustion of fuels 2
Calculations involving gases and fuels

2. Combined gas equation
This combines the relationships between pressure, volume, moles and temperature when ‘something has changed’. If a quantity has remained constant it can be simply removed from the equation.
Example - A balloon contains a 1.80 mol sample of gas and has a volume of mL at 1.00 atmosphere pressure and 27C. Some of the gas is removed from the balloon and new measurements are taken. The new volume is 60.0 mL and the pressure and temperature are 800 mm Hg and 17C respectively? What is the amount (in mol) of the gas now in the balloon?

3. Universal gas equation
This equation has been determined from the combined gas equation where a value has been determined for the constant, k, in the equation.
The constant of proportionality is referred to as the Gas Constant and is given the symbol R.
Hence the General Gas Equation can be written as:
PV = nRT

4. Units for the Universal gas equation
The units of the Gas Constant depend on the units of P, V, n and T.
n is always in moles (mol)
T is measured in Kelvin (K)
P is measured in kilopascals (kPa) PV = nRT
V is measured in L
When all the variables are measured in SI (System International) units R = 8.31 J K–1mol–1

5. Using the universal gas equation
If mol of a gas occupies 2000 mL at atm, what is its temperature in oC?
Try q 5-8 on p80 of your text

6. Combining all of the equations

7. Mass-Mass stoichiometric problems
Calculate the mass of carbon dioxide produced when 3.60kg of butane (C4H10) is burned completely in oxygen
Write the equation and balance it
Determine the moles of the known quantity
Use the molar ratio in the equation to determine the moles of the unknown quantity
Use the moles of the unknown substance to determine the mass
P84 – complete q 1-5

8. Mass – Volume stoichiometric problems
Connecting mass and volume again involves moles but this time temperature is important as it will determine whether Vm or PV = nRT is used.
Example 1 (mass volume – standard)
Calculate the volume of CO2, in L, produced when 300g of butane is burned completely in oxygen. The gas is measured at SLC.

9. Example 2 – mass volume (non standard)
Calculate the volume of CO2, in L, produced when 5.00kg of butane is burned completely in oxygen. The gas is measured at 40˚C and 400kPa.

10. Example 3 – Volume-volume
If all reactants are gases then the volumes can act as the molar ratios
Methane gas (CH4) is burned un a gas stove according to the following equation
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)
If 50mL of methane is burned in air, calculate the volume of CO2 gas produced under constant temperature and pressure
P90 – complete q 1-5