A ball has a volume of 6.35 liters and is at a temperature of
27.0°C. A pressure gauge attached to the ball reads 0.45
atmosphere. The atmospheric pressure is 1.00 atmosphere.
Calculate the absolute pressure inside the ball and the
amount of moles of air it contains. (First, find the absolute
pressure and then use that to find the moles using the ideal
gas law. Remember to use the correct ideal gas constant and
to convert from celsius to kelvin.)

Explanation:

The gauge pressure inside the ball gives the absolute pressure inside the ball, relative to the atmospheric pressure outside the ball. In other words:

.

Rearrange to obtain:

.

Look up the ideal gas constant. This constant comes in a large number of unit combinations. Look for the one that takes for pressure and for volume.

.

Convert the temperature to absolute temperature:

.

Assume that the gas inside this ball acts like an ideal gas. Apply the ideal gas law (after rearranging) to find the number of moles of gas particles in this ball:

.

(Rounded to two significant figures, as in the pressure gauge reading.)

it's filtration, but this is an assumption so my apologies if i got this

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.