Question

You have an evacuated container of fixed volume and known mass and introduce a known mass of a gas sample. Measuring the pressure at constant temperature over time, you are surprised to see it slowly dropping. You measure the mass of the gas- filled container and find that the mass is what it should be--gas plus container--and the mass does not change over time, so you do not have a leak.A. Suggest an explanation for your observations.B. At constant pressure, the mean free path () of a gas molecule is directly proportional to temperature (T). At constant temperature, 1 is inversely proportional to pressure (P). If you compare two different gas molecules at the same temperature and pressure, ) is inversely proportional to the square of the diameter (d) of the gas molecules. Put these facts together to create a formula for the mean free path of a gas molecule with a proportionality constant (call it Rmfp, like the ideal-gas constant).C. Define units for Rmtp

Answer 1

The gas goes through a chemical reaction where the products have fewer gas particles than reactants. Since the number of particles directly relates to pressure, the pressure dropped.

PV = nRT is the ideal gas law.

Pressure also reduced as drug amount did.

PV = nRT is the equation for an ideal gas. In this equation, P stands for the ideal gas's pressure, V for the ideal gas' volume, n for the total amount of the ideal gas expressed in moles, R for the universal gas constant, and T for temperature.

PV = nRT

The macroscopic characteristics of ideal gases are related by the ideal gas law (PV = nRT). A gas is considered to be perfect if its particles (a) do not interact with one another and (b) occupy no space (have no volume).

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