Asealed container holds 0.020moles of nitrogen (n2) gas, at a pressure of 1.5 atmospheres and a temperature of 290k. the atomic mass of nitrogen is 14.0 g/mol.

So it appears that this is asking for what the volume (V) of the N2 gas is under those conditions. For this we use the Ideal Gas Law:
PV = nRT, where P = the pressure in atm, V = the volume in liters (L), n = the number of moles of gas, R = the Ideal gas constant, which is 0.0821 (atm•L)/(mol•K), and T = the temperature in Kelvin which is the °C + 273
So to solve for V: V = (nRT)/P
V = [(0.020molN2)×(0.0821atm•L/(mol•K)×290K] ÷ 1.5atm
V = [(0.476•atm•L N2] ÷ 1.5atm
V = 0.317 L N2
If you look at each step, you can see that I included the units, because you can see them cross each other out to give you the final product, volume, which is in liters (L).
I hope that helps you understand these types if problems better!

For cyclohexane compounds drawn in a chair conformation:   -axial bonds are vertical  -equatorial bonds are parallel to two bonds within the ring.  thus, as i assume the chair conformation is drawn:   -the x group is in an axial position, as are the five other vertical bonds.  -three axial bonds are on the top face of the ring  -the other three axial bonds are on the bottom face  the position of the second substituent on each ring carbon is equatorial.  gauche groups must be on an adjacent carbon such as carbon 6 and carbon 2, and also gauche groups are rotated by 60 degrees relative to each other.  drawing the newman projections for c1–c2 and c1–c6 aids in visualizing the groups that are gauche to the y group on c1.  click this link and watch some academic videos that may you more understand the topic