How does Gas behave inside a closed container?

Answer 1

Boyle’s Law
It’s a little basic common sense: In a close container of gas as the volume of a container is increased the pressure is decreased and as the volume is decreased the pressure is increased. However, the relationship is directly proportional so you can easily use math to figure out what would happen.

According to Wikipedia: http://en.wikipedia.org/wiki/Boyle%27s_law
“Boyle's law (sometimes referred to as the Boyle-Mariotte law) is one of the gas laws and basis of derivation for the Ideal gas law, which describes the relationship between the product pressure and volume within a closed system as constant when temperature remains at a fixed measure; both entities remain inversely proportional.[1][2] The law was named for chemist and physicist, Robert Boyle who published the original law in 1662. The law itself can be defined succinctly as:
“For a fixed amount of gas kept at a fixed temperature, P and V are inversely proportional”

So as the pressure is varied the volume of the gas varies in the opposite direction.
If you increase the pressure the volume shrinks; but it does so in the exact relationship to the pressure. The laws get more complex when temperature is taken into account, because if you compress a gas you increase its temperature; however the temperature will remain proportional to the volume and pressure as well.

An example of Bolye’s Law in action is how we create liquid oxygen or nitrogen. We don’t have refrigerators that can get that cold so we have to trick the gas to decrease the temperature. First you compress the gas, which increases the temperature, and then you cool it off. After that you release the gas to a larger volume container and the temperature has to fall again so the gas can increase its volume and decrease its pressure. Do this enough times and you can turn atmospheric gases into liquids. You’re AC works in a similar fashion. A compressor compresses the coolant gas, and the heat is taken away from it, usually by evaporation of water, then the gas is allowed to expand; which will again reduce the temperature.

Answer 2

A gas will spread apart to equally fill the space of any container.

Answer 3

It expands to fill the container, regardless of volume.

Answer 4

It expands to fill the container.

Answer 5

Depends on what you do to it. If you cool it, the pressure it exerts on the container goes down. If you heat it, the pressure increases.

Answer 6

perfect gasoline regulation: PV = nRT Conservation of mass and potential: beginning mass (grams) equals ending mass (grams) question 2 is spoke back suitable off the bat by ability of the Conservation of Mass regulation. ending mass is 3.50 g. question a million calls so which you would be able to place in writing out and stability the reaction: 3H2 (g) + N2 (g) --> 2NH3 (g) Then convert the a lot to moles (do no longer ignore nitrogen and hydrogen are diatomic!): 0.500 g H2 / 2.02 g/mol = 0.248 mol H2 3.00 g N2 / 28.0 g/mol = 0.107 mol N2 Now do your stoichiometry and locate your proscribing reactant: for each a million mol of N2 fed on, you ought to devour 3 mol of H2 and convey 2 mol NH3. 0.248 mol H2 * (2/3) = 0.a hundred sixty five mol NH3 (assuming N2 in extra) 0.107 mol N2 * (2) = 0.214 mol NH3 (assuming H2 in extra) H2 is the proscribing reactant and could be totally fed on in this reaction, through fact 0.a hundred sixty five is decrease than 0.214. Your very final products would be 0.a hundred sixty five mol NH3, with some N2 in extra. 0.a hundred sixty five mol NH3 * (a million/2) = 0.0827 mol N2 fed on. 0.107 mol N2 available - 0.0827 mol N2 fed on = 0.0243 mol N2 left over. n = finished moles after reaction = 0.a hundred sixty five mol NH3 + 0.0243 mol N2 = 0.189 mol finished gasoline Conversions to make the math greater handy: R = 8.134 J/(ok*mol) = 8.134 (Pa*m^3)/(ok*mol) V = 20.0 L = 20000 mL = 20000 cm^3 = 0.02 m^3 P = nRT/V = 0.189 mol * 8.314 (Pa*m^3)/(ok*mol) * 308.15 ok / 0.02 m^3 All contraptions cancel yet Pa P = 2.40 two * 10^4 Pa = 24.2 kPa