Quickly !
part 1. determine the molar mass of a 0.458-gram sample of gas having a volume of 1.20 l at 287 k and 0.980 atm. show your work. part 2. if this sample was placed under extreme pressure, describe how the actual volume would compare to the predicted volume. explain your answer.

The answers are:

Part 1

Part 2

The volume of the gas will decrease, the compresibility will decrease and the density will increase.

Since we are given the mass of the sample, first, we need to find the number of mole of the sample.

Part 1

We cand find the number of moles using the following formula:

Where,

So, isolating "n" we have:

Then, substituting we have:

Now, since we have the number of moles and the mass of the sample, we can calculate the molar mass using the following equation:

Part 2.

Now, if the gas is placed under extreme pressure, the volume will decrease but there will be always a certain volume since the molecules will always be occupying space, also, the compressibility of the gas will decrease.

If we are talking about ideal gases, the compressibility factor (z)will be equal to 1, but if the gas is placed under extreme pressure, I will not behave like an ideal gas, meaning that the compressibility factor will not be equal to 1, also the density of the gas will increase since there will be the same mass in a smaller volume. The compressibility factor is used to determinate the Boyle's Law deviation and it can be calculated by using the following equation:

We need to remember that the gas will behave like an ideal gas only with lower temperatures and lower pressures.

Have a nice day!

i think the answer is terrae but not 100 percent sure. ▓▬▬ §

where are the choice options?