1. Prepare the reactant/product table shown below. Note that you can estimate the volume of
H2 and air by estimating the diameter of the balloon used and using the lab temperature
and pressure to determine the approximate number of moles of H2 and O2 in the balloons.
The ideal gas law ($PV = nRT$) is particularly useful for this calculation. For the purposes
of this exercise assume the balloons containing H2 and O2 are 15 cm in diameter (about
6"), the laboratory temperature is 23°C, and the laboratory pressure is 730 torr. It should
also be noted that the pressure in a balloon is about 50 torr higher than the external pressure.
R (the gas constant) in the ideal gas law is 62.36 L torr mol$^{-1}$ K$^{-1}$.
Material
Volume /L
Mass /g
Molecular weight
or molarity
Moles
H2
O2 (as air, 20% v/v)
NaOH
Laboratory conditions
Temperature (K)
Pressure (torr)
