Avogadro's
Posted: Tue May 13, 2014 12:20 am
Hello!
I've always come by this statement in my dealings with chemistry; ''under conditions of same temperature and pressure, equal volumes of different gasses contain the same number of particles.'' I may neither have done an intensive study nor an experiment to thoroughly understand and confirm that ('cause i don't have access to either good study or a good lab), but i also came across something that explained to a great extent that statement, thus; ''when the distance between the particles in a gas are very great compared with the sizes of the particles, Avogadro's hypothesis works well for such...under these conditions, the volume of a gas is determined by the number of molecules present, not by the size of the individual particles.'' Here's what crossed my mind; at tempeture 'x' and pressure 'y', different gasses possess different sizes, masses and amounts of kinetic energy. Getting two gasses each saturated in a unit volume of space, under conditions of same temp. and pressure and different masses, sizes and kinetic energies, there would be a different number of particles in each space, because the interaction; motion rate and collision effects affecting motion, between individual gas particles would be determined by particle mass, size and amount of kinetic energy. In this sense the volume and other factors determine the number of particles, not the number of particles determining the volume.
Those're just my thoughts drawn from limited access to good educationing. Please, help correct any misconceptions 'cause you're better experienced than I.
I've always come by this statement in my dealings with chemistry; ''under conditions of same temperature and pressure, equal volumes of different gasses contain the same number of particles.'' I may neither have done an intensive study nor an experiment to thoroughly understand and confirm that ('cause i don't have access to either good study or a good lab), but i also came across something that explained to a great extent that statement, thus; ''when the distance between the particles in a gas are very great compared with the sizes of the particles, Avogadro's hypothesis works well for such...under these conditions, the volume of a gas is determined by the number of molecules present, not by the size of the individual particles.'' Here's what crossed my mind; at tempeture 'x' and pressure 'y', different gasses possess different sizes, masses and amounts of kinetic energy. Getting two gasses each saturated in a unit volume of space, under conditions of same temp. and pressure and different masses, sizes and kinetic energies, there would be a different number of particles in each space, because the interaction; motion rate and collision effects affecting motion, between individual gas particles would be determined by particle mass, size and amount of kinetic energy. In this sense the volume and other factors determine the number of particles, not the number of particles determining the volume.
Those're just my thoughts drawn from limited access to good educationing. Please, help correct any misconceptions 'cause you're better experienced than I.