Three samples of three different gases are listed in the table below. All the samples contain exactly 1 mole of gas and are at a temperature of 0.0°C.For each sample, decide whether the gas can be reasonably described as an ideal gas. If the gas isn't ideal, decide the most important reason why it isn't.sample pressure volume ideal? If not ideal, the most(atm) (L) important reason why not:A 1.3 20.0 yesThere are attractions between the particles.noThe particles don't have zero volume.B 0.75 30.0 yesThere are attractions between the particles.noThe particles don't have zero volume.C 0.50 40.0 yesThere are attractions between the particles.noThe particles don't have zero volume.

The question seems to be asking for an analysis of whether each gas sample can be considered an ideal gas, and if not, why not. An ideal gas is a theoretical gas composed of a set of randomly moving, non-interacting point particles. The ideal gas concept is useful because it obeys the ideal gas law, a simplified equation of state, and is amenable to analysis under statistical mechanics.

Here's how you might approach this:

Sample A: Pressure = 1.3 atm, Volume = 20.0 L The ideal gas law is PV=nRT, where P is pressure, V is volume, n is number of moles, R is the gas constant, and T is temperature in Kelvin. If we plug in the given values (converting temperature to Kelvin by adding 273 to the Celsius temperature), we get (1.3 atm)(20.0 L) = (1 mole)(0.0821 L·atm/K·mol)(273 K). The left side of the equation equals 26, and the right side equals 22.4. Since these are not equal, the gas does not behave ideally. The most likely reason is that the particles do not have zero volume.

Sample B: Pressure = 0.75 atm, Volume = 30.0 L Using the same process, we get (0.75 atm)(30.0 L) = (1 mole)(0.0821 L·atm/K·mol)(273 K). The left side of the equation equals 22.5, and the right side equals 22.4. These values are very close, so we can say that the gas behaves almost ideally.

Sample C: Pressure = 0.50 atm, Volume = 40.0 L Again using the ideal gas law, we get (0.50 atm)(40.0 L) = (1 mole)(0.0821 L·atm/K·mol)(273 K). The left side of the equation equals 20, and the right side equals 22.4. Since these are not equal, the gas does not behave ideally. The most likely reason is that there are attractions between the particles.

Please note that this analysis assumes that the deviations from ideality are due to either attractions between particles or non-zero particle volumes. Other factors could also cause deviations from ideal behavior.