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What? They are definitely not behaving according to the ideal gas law: PV = nRT, that law only work for low pressures and totally inert gasses like helium, argon and so on, and then not even that accurate.
The ideal gas law makes several assumptions.
The particles collide completely elastically (no energy is transfered at collision)
The particles does not in anyway react with one or other
The particles don't affect each other besides from "ideal collisions" (=no attraction/repulsion because of charge and so on)
And in fact ALL those assumptions are false for normal air at 1 atm.
The equation that accurately describes real gasses and mixtures of different real gasses is extremely complicated and not completely accurate either and it uses a lot of gas-specific constant and is very unwieldy. Which is why the ideal gas equation of state is so often used at lower level courses..
Another way of modelling real gasses iw to run a simulation; simply have the gas molecules bounce around in a computer model with all their properties built into the model as accurately as possible. A simple problem could probably be run fairly quickly by a normal desktop PC, but more complex scenarios would need a supercomputer/cluster to come up with a quick answer. The supercomputer doing weather forecasting (can't remembers its name, Earth Simulator) has such a gas model built into its larger climate model.
So that is what I got from your question.
What else can I help you with?
What happens to the temperature increase the number of particles what happens to the pressure?
Increasing the temperature the number of particles remain constant and the pressure increase.
Comparison between normal temperature pressure and standard temperature pressure?
Normal temperature pressure refers to conditions at 0°C (273K) and 1 atm pressure, while standard temperature pressure refers to conditions at 25°C (298K) and 1 atm pressure. These conditions are used as reference points for certain calculations and measurements in chemistry and physics. The main difference is the temperature at which they are defined, with standard temperature pressure being at a slightly higher temperature than normal temperature pressure.
What causes the particles of a substance to condense?
Particles of a substance condense due to a decrease in temperature or an increase in pressure, which reduces the kinetic energy of the particles. As temperature drops, particles move slower and lose energy, allowing intermolecular forces to pull them closer together. This leads to a transition from a gas to a liquid or from a liquid to a solid, depending on the substance and conditions.
A sample of hydrogen gas will behave most like an ideal gas under the conditions of?
High temperature and low pressure. High temperature because this speeds up the rate of the molecules so there is less intermolecular forces of attraction between particles. Low pressure because the greater the distance of the particles and the less molecular forces of attraction between particles.
How does the number of particles affect the pressure of a gas?
Increased density and temperature.
What is chlorine's state at solid room temperature?
Chlorine is a gas at room temperature and pressure, not a solid.
Which gas can be liquefied under pressure at ordinary temperature?
Carbon dioxide (CO2) can be liquefied under pressure at ordinary temperature.
What are two conditions that determine the mass of solute that will dissolve in a given mass of solvent?
The temperature: Increasing temperature makes the particles move faster. Heat energy is transferred by the movement of the particles. Because the solvent particles are moving faster, they bump into the solute.Stirring: Moves all the particles around do the solvent particles bump into the solute particles.
Under ordinary conditions of temperature and pressure how are the particles of a gas arranged?
The particles are far apart and moving randomly. Due to something called thermal equilibrium, an object, if left for a certain amount of time, will reach the same temperature as its surroundings. When a gas is placed in an environment that has, let's say, 1 atmosphere of pressure, it will equalize to 1 atmosphere of pressure, going from high pressure to low pressure. And the same will happen with temperature, so leave a gas in an environment for long enough and it will reach the same temperature and pressure as its environment.
What happens to the temperature increase the number of particles what happens to the pressure?
Increasing the temperature the number of particles remain constant and the pressure increase.
Why can scientist ignore the forces of attraction among particles in a gas undr ordinary conditions?
Scientists can sometimes ignore the forces of attraction among particles in a gas under ordinary conditions because the kinetic energy of gas particles is much greater than the attractive forces between them. This means that the particles move around freely and independently of each other, resulting in the ideal gas behavior that doesn't consider intermolecular forces. This simplification allows for easier mathematical modeling and analysis of gas behavior.
Comparison between normal temperature pressure and standard temperature pressure?
Normal temperature pressure refers to conditions at 0°C (273K) and 1 atm pressure, while standard temperature pressure refers to conditions at 25°C (298K) and 1 atm pressure. These conditions are used as reference points for certain calculations and measurements in chemistry and physics. The main difference is the temperature at which they are defined, with standard temperature pressure being at a slightly higher temperature than normal temperature pressure.
How are conditions of pressure and temperature?
Temperature is particles moving really fast and bumping in to each other (in a sense, but nothing really "touches" other things atomically or else they fuse), unless of course, they are at 0 D. kelvin, and pressure is just density in the air or in another sense it's compression.
What does the volume of gas depend on?
The volume of gas depends on the temperature, pressure, and number of gas particles present. These factors affect the amount of space the gas particles occupy.
A sample of hydrogen gas will behave most like an ideal gas under the conditions of?
High temperature and low pressure. High temperature because this speeds up the rate of the molecules so there is less intermolecular forces of attraction between particles. Low pressure because the greater the distance of the particles and the less molecular forces of attraction between particles.
Which term is defined as a measure of the average kinetic energy of particles in a sample?
temperature
How does pressure temperature and the number of particles affect the behavior of a gas?
The combined gas equation is used to calculate the behaviour of gas under different temperature, pressure and number of particles. PV = nRT Where P is pressure V is volume n is the number of moles T is the temperature in Kelvin and R is the Ideal Gas Constant. If P is in kPa and V is in dm3 then R = 8.31.
