blazeuofa said:Homework Statement
Determine the number density of particles in a gas at STP (T=273, p=1atm)
Homework Equations
Answer is 2.68x1025
The Attempt at a Solution
pV=nRT
I don't really understand what the "number density of particles" means please help!
blazeuofa said:hmm I can't quite get the right answer. V=22.4L and avagadros # is the molecules in one mole. How do I piece this together?
A simple ideal gas is a theoretical model of a gas that is composed of particles that have negligible volume and do not interact with each other. This model is often used in scientific calculations and experiments as it simplifies the behavior of gases.
The assumptions made in a Simple Ideal Gas problem include: 1) particles have negligible volume, 2) particles do not interact with each other, 3) particles move in random straight-line motion, and 4) the average kinetic energy of the particles is directly proportional to temperature.
The pressure of a Simple Ideal Gas can be calculated using the ideal gas law, which states that pressure (P) is equal to the number of moles (n) of gas multiplied by the gas constant (R) and the temperature (T) in Kelvin, divided by the volume (V) of the gas. This can be expressed as the equation: P = (nRT)/V.
According to the ideal gas law, as temperature increases, the pressure of a Simple Ideal Gas will also increase if the volume and number of moles remain constant. This is because an increase in temperature means an increase in the average kinetic energy of the particles, causing them to collide with the walls of their container with greater force, thus increasing the pressure.
A Simple Ideal Gas problem assumes that the gas particles have no volume and do not interact with each other, while real gases exhibit some volume and do interact with each other. This can cause deviations from the ideal behavior predicted by the ideal gas law, especially at high pressures and low temperatures. Real gases also have specific gas constants, whereas the ideal gas law uses a universal gas constant that applies to all ideal gases.