Calculate the pressure exerted by 1.0 mol of c6h6behaving as a)a perfect gas and b) a van der waals gas when it is confined under the following conditions: i)373.15 k in 22.414 dm3ii)1000 k in 22.414 dm3iii)1000 k in 150.000 dm3at which one of these conditions does the real gas be?

The detailed calculation is shown in the attached file.

last condition (1000 K in 150.000 dm3) will have the least deviations and it is the condition where real gas will behave as ideal gases

Explanation:

Real gas behave more ideally or they tend towards ideality when there is the least deviation, or their inter-molecular forces between their molecules are mainly responsible for their deviations as such gases with the strongest intermolecular forces shows the strongest deviations. As such, when their is an increase in temperature and volume and a decrease in pressure, real gas tends towards ideal gas in this case.

From the three conditions given, it is obvious that the last condition(1000 K in 150.000 dm3)  will have the least deviations.

because u need two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei to form isotopes.

so since they all have the same shape? i mean maybe because m& m and reeses are both chocolates

c) should be the answer.