Given a cylinder of fixed volume filled with 1 mol of argon gas, which of the following is correct? (Assume all gases obey the ideal gas law.) a) If the temperature of the cylinder is changed from 25 degree c to 50 degree c, the pressure inside the cylinder will double. b) A cylinder of identical volume filled with the same pressure of helium must contain more atoms of gas because He has a smaller atomic radius than argon. c) If a second mole of argon is added to the original cylinder, the pressure will be doubled. d) If the temperature of the cylinder is changed from 400K to 200 K, the pressure will be doubled. e) None of the above.

Given a cylinder of fixed volume filled with 1 mol of argon gas, assume all gases obey the ideal gas law, none of the statement are correct. (Option E)

The ideal gas law, also known as the general gas equation, refers to a state of a hypothetical ideal gas. It is a good behavioral approximation of many gases exhibit under many conditions, although it has several limitations. It was suggested 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. The ideal gas law is often written in an empirical form:

pV = nRT

where p, V and T are the pressure, volume, and temperature; n is the amount of substance; and R is the ideal gas constant.

Based on the relationship between pressure, volume, and temperature given by the equation, none of the statements are true.

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