what is real gases?
Answers
Answer:
The term ‘real gas’ usually refers to a gas that does not behave like an ideal gas. Their behaviour can be explained by the interactions between the gaseous molecules. These intermolecular interactions between the gas particles is the reason why real gases do not adhere to the ideal gas law. Therefore, real gases can be defined as non ideal gases whose molecules occupy a given amount of space and have the ability to interact with each other.
Answer:
Real gases are nonideal gases whose molecules occupy space and have interactions; consequently, they do not adhere to the ideal gas law.
Explanation:
ideal gas law
The ideal gas law, also called the general gas equation, is the equation of state of a hypothetical ideal gas. It is a good approximation of the behavior of many gases under many conditions, although it has several limitations. It was first stated by Benoît Paul Émile Clapeyron in 1834 as a combination of the empirical Boyle's law, Charles's law, Avogadro's law, and Gay-Lussac's law.[1] The ideal gas law is often written in an empirical form:
{\displaystyle PV=nRT}PV=nRT
where {\displaystyle P}P, {\displaystyle V}V and {\displaystyle T}T are the pressure, volume and temperature; {\displaystyle n}n is the amount of substance; and {\displaystyle R}R is the ideal gas constant. It is the same for all gases. It can also be derived from the microscopic kinetic theory, as was achieved (apparently independently) by August Krönig in 1856[2] and Rudolf Clausius in 1857.[3]
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