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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?
Real gas molecules have volume and experience intermolecular forces, while ideal gas molecules are treated as point particles with negligible volume and no intermolecular forces. In real gases, molecules have varying speeds and collision effects due to their volume and interactions, while ideal gases follow the assumptions of the kinetic theory perfectly due to their simplified behavior.
Why does strong repulsion between molecules not represent an ideal gas behavior?
The ideal gas laws are based on a model in which the ideal gas is composed of molecules which neither attract nor repel each other. The pressure that the ideal gas exerts on its container is simply the result of the random thermal motion of the molecules and the continual collisions which result from that random thermal motion. If the molecules also repelled each other, then they would produce a gas with even higher pressure, and the pressure would also increase more rapidly, if the gas was compressed, than it does in the absence of such repulsion. The observed behavior of real gases is much closer to that of an ideal gas that does not include repulsion between molecules. No such repulsion has been observed.
What would make gas non ideal?
The gas molecules interact with one another
What is the molecules of an ideal gas?
The molecules of an ideal gas have negligible volume and no intermolecular forces acting between them. They are in constant, random motion and collide elastically with each other and the walls of the container. The behavior of an ideal gas is described by the ideal gas law, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature.
What is the average volume per molecule in an ideal gas?
The average volume per molecule in an ideal gas is equal to the total volume of the gas divided by the total number of gas molecules present. This value is constant for all ideal gases at a given temperature and pressure.
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 :)
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.
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 avogadros principle be applied?
Avogadro's principle can be applied to ideal gases at constant temperature and pressure. It states that equal volumes of gases at the same temperature and pressure contain the same number of molecules, allowing for calculations involving quantities of gases.
For ideal gas force of attraction between molecules?
For an ideal gas, there is assumed to be no force of attraction between molecules. This assumption allows for simplification of the gas behavior under certain conditions, such as low pressure and high temperature. In reality, real gases do experience weak forces of attraction between molecules, but these are considered negligible in the ideal gas model.
Diff between real gas and ideal gas?
In an ideal gas molecules interact only elastically.
What is ideal average in statistics?
The term ideal refers to the one that is exactly right or perfect. Average refers to anything that isn't ideal, but also is not an outlier. Average is somewhere in the middle of the two.
The molecules of all samples of ideal gases have the same average kinetic energies at the same?
temperature. This is known as the kinetic theory of gases, which states that the average kinetic energy of gas molecules is directly proportional to the temperature of the gas, regardless of the type of gas.
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
Explain what is the difference between real gas molecules and ideal gas molecules by kinetic theory?
Real gas molecules have volume and experience intermolecular forces, while ideal gas molecules are treated as point particles with negligible volume and no intermolecular forces. In real gases, molecules have varying speeds and collision effects due to their volume and interactions, while ideal gases follow the assumptions of the kinetic theory perfectly due to their simplified behavior.
What is the different molecules that make up the air in the room have on average the same kinetic?
In a room, the different molecules making up the air have, on average, the same kinetic energy. This is governed by the ideal gas law and the distribution of kinetic energies within a gas at a particular temperature. Despite differences in mass and speed, the average kinetic energy remains constant for a given temperature.
