Which of the following factors does not explain why measurements of real gases deviate from
ideal values ?
(A) The volume of the gas particles themselves
(B) The volume between the gas particles
(C) Intermolecular forces
(D) All of these factors will cause deviation from ideal values
Answers
Answer:
b is a correct answer
Explanation:
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Answer:
a) Gases consist of very large numbers of tiny spherical particles that are far apart from one another compared to their size . The particles of a gas may be either atoms or molecules. The distance between the particles of a gas is much, much greater than the distances between the particles of a liquid or a solid.
b) Because most of the volume occupied by a gas is empty space, a gas has a low density and can expand or contract under the appropriate influence. The fact that gas particles are in constant motion means that two or more gases will always mix as the particles from the individual gases move and collide with each other.
c) Intermolecular forces are the forces which mediate interaction between atoms, including forces of attraction or repulsion which act between atoms and other types of neighboring particles, e.g. atoms or ions. Intermolecular forces are weak relative to intramolecular forces – the forces which hold a molecule together.
d) The causes of deviations from ideal behaviour may be due to the following two assumptions of kinetic theory of gases.
The volume occupied by gas molecules is negligibly small as compared to the volume occupied by the gas.The forces of attraction between gas molecules are negligible.