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What quantities is zero on an average for the molecules of an ideal gas in equilibrium?
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Do particles in a liquid move at the same pace?
No, but if the system is at equilibrium the speeds of all the molecules (assuming an ideal liquid) will be characterized by a Boltzman distribution.
Type of equilibrium that occurs when allel frequencies do not change?
the type of equilibrium that occurs when an allele frequencies do not change is dynamic equilibrium :)
Explain what is the difference between real gas molecules and ideal gas molecules by kinetic theory?
In an ideal gas, molecules don't take up space, and don't have long-range interactions.
When can you safely assume any gas is ideal?
Characteristics of an ideal gas:- an extremely low concentration- molecules are in a permanent motion- Newton laws can be applied- all collisions are elastic- molecules are spherical- molecules are not compressible
What is the molecules of an ideal gas?
Perfectly elastic collisions, point masses (no volume of individual molecules), no intermolecular attractions.
Do particles in a liquid move at the same pace?
No, but if the system is at equilibrium the speeds of all the molecules (assuming an ideal liquid) will be characterized by a Boltzman distribution.
Type of equilibrium that occurs when allel frequencies do not change?
the type of equilibrium that occurs when an allele frequencies do not change is dynamic equilibrium :)
For ideal gas force of attraction between molecules?
In an ideal gas there is no attarcation between molecules. There is no such thing as an ideal gas it is a model that approximates the behaviour of real gases.
The molecules of all samples of ideal gases have the same average kinetic energies at the same?
Temperature and pressure.KEavg = (3/2)RT
Why real gases deaviat from ideal behaviou?
It is assumed that Ideal Gases have negligible intermolecular forces and that the molecules' actualphysical volume is negligible. Real Gases have the molecules closer together so that intermolecular forces and molecules' physical volumes are no longer negligible. High pressures and low temperatures tend to produce deviation from Ideal Gas Law and Ideal Gas behavior.
Explain what is the difference between real gas molecules and ideal gas molecules by kinetic theory?
In an ideal gas, molecules don't take up space, and don't have long-range interactions.
When an ideal gas does positive work on its surroundings which of the gas's quantities increases?
Volume
What chemical is in a cell?
Chemical equilibrium in a cell is when the chemical concentration, that is all of the various ions, molecules, and minerals, within the cell (cytoplasm mainly) is in a state of stasis or equality with its external concentration. Wherein there is no concentration gradient or osmotic pressure under which molecules would need to diffuse across the cell membrane. This ideal (which never truly comes to pass) would imply that the molecules within and external to the cell membrane would cease to flow continually in and out, as the cell and its exterior would be of equal concentrations/ at equilibrium.
When can you safely assume any gas is ideal?
Characteristics of an ideal gas:- an extremely low concentration- molecules are in a permanent motion- Newton laws can be applied- all collisions are elastic- molecules are spherical- molecules are not compressible
Diff between real gas and ideal gas?
In an ideal gas molecules interact only elastically.
What is the average kinetic energy of all the molecules in an object?
Average KE for molecules is defined by (3/2)RT: where R is the ideal gas constant (8.314 J K-1 mol-1 ) and T is the absolute temperature of the fluid (gas/liquid) in Kelvin. The reason for 3/2 is based on the x,y, and z planes that the gas molecules could be moving (vibrating, translating, rotating). For just a single plane it would be 1/2RT. The KE derived from the equation is the average KE for a mole of gas molecules and not the energy of every, or any of the molecules. A single gas molecules chosen at random may have any KE associated with it, but this equation gives the average of all molecules
Why ammonia doesnt behave as an ideal gas?
NH3, as in Ammonia, like all real gases, are not ideal. Ideal gases follow the ideal gas laws, but ammonia does not adhere to a few of them. First of all, the volume of its molecules in a container is not negliggible. Next, NH3 molecules have intermolecular hydrogen bonding, which is a strong intermolecular bond. Thus, the forces of attaction between molecules is not neglible. All real gases have a certain degree of an ideal gas, but no real gas is actually ideal, with H2 being the closest to ideal.
