Need chemistry help

Question

The volume of a driver-side air bag is 80.0 L. Calculate the number of moles of CO2 needed to fill the air bag and the grams of sodium bicarbonate and milliliters of vinegar needed for the reaction. 

Moles of CO2 required to inflate 80-L driver-side air bag at room temperature and pressure

Balanced equation for the reaction of NaHCO3 and CH3COOH to CO2

Mass of NaHCO3 needed for the reaction (84.0 g/mol)

Volume of vinegar required (0.833 M acetic acid)

Answer 1

First we need to use ideal gas law (PV=nRT) to find number of moles of CO2:

1 atm x 80L = n. x 0.082 L.atm/K x (273+25)K

Therefore: n = 80 / (0.082 x 298) = 3.27 moles

Now, to produce CO2, we need to react vinegar and baking soda as follows:

NaHCO3 + CH3COOH ---> NaCH3COO + CO2 + H2O (it is balanced already)

Every mole of CO2 needs one mole of baking soda, so we need 3.27 moles of it

3.27 x 84 = 274.7 g of baking soda needed.

Finally, the volume of vinegar needed is:

3.27 / 0.833 = 3.93 L of vinegar

:-)