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Under ordinary conditions of temperature and pressure, the particles in a gas are?
Wiki User
∙ 8y ago
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.
Wiki User
∙ 8y ago
Wiki User
∙ 12y agoI had this question on a test and i got it right. Under ordinary conditions of temperature and pressure the particles in a gas are very far from on another
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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.
If you wanted to predict how temperature will effect the volume of a gas what factors must be held constant?
If temperature increases, then pressure increases. Temperature measures the average speed of particles, so if the temperature is high, then the particles are moving quickly and are colliding with other particles more forcefully. Pressure is defined as the force and number of collisions the particles have with the wall of its container. So if the high temperature causes the particles to move quickly, they are going to collide more often with the container, increasing the pressure. This remains true as long as the number of moles (n) remains constant.
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.
What are the best conditions for dissolving a gas in a liquid?
high pressure to force the gas into the liquid and low temperature so that the moving gas particles have less resistance to being dissolved
How does the number of particles affect the pressure of a gas?
Increased density and temperature.
Why can scientist ignore the forces of attraction among particles in a gas undr ordinary conditions?
ordinaroly these forces do not effect the changes in pressure , volume, or temperature to an extent where they are important.
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 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.
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.
Which term is defined as a measure of the average kinetic energy of particles in a sample?
temperature
Can ammonia be liquefied under pressure at ordinary temperature?
No you can't do that. There is a very low temperature to do that.
Which gas can be liquefied under pressure at ordinary temperature?
LPG gas
If you wanted to predict how temperature will effect the volume of a gas what factors must be held constant?
If temperature increases, then pressure increases. Temperature measures the average speed of particles, so if the temperature is high, then the particles are moving quickly and are colliding with other particles more forcefully. Pressure is defined as the force and number of collisions the particles have with the wall of its container. So if the high temperature causes the particles to move quickly, they are going to collide more often with the container, increasing the pressure. This remains true as long as the number of moles (n) remains constant.
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.
What is an ordinary condition of temperature and pressure?
15 Degrees C, and 29.92 inHg
Which conditions of pressure and temperature would give the most accurate value of Mr?
Its high temperature and low pressure
What conditions represent Stp?
Standard Temperature and Pressure
