Calculate the gram molecular mass of nitrogen if 360cc at STP weigh 0.45g.

I don't know what to do with it but the problem is that I can do it.

To calculate the gram molecular mass of nitrogen, we need to use the ideal gas law equation. The ideal gas law equation is given by:

PV = nRT

Where:
P = Pressure (in atm)
V = Volume (in liters)
n = Number of moles
R = Ideal gas constant (0.0821 L.atm/mol.K)
T = Temperature (in Kelvin)

In this case, we are given the volume (360 cc) and the weight (0.45 g) of nitrogen. We know that at STP (Standard Temperature and Pressure), the temperature is 273.15 K and the pressure is 1 atm.

Step 1: Convert the volume from cc to liters.
Since 1 cc is equal to 0.001 liters, we have:
360 cc * (0.001 liters/1 cc) = 0.36 liters

Step 2: Plug the given values into the ideal gas law equation to find the number of moles.
PV = nRT
(1 atm)(0.36 L) = n(0.0821 L.atm/mol.K)(273.15 K)
0.36 atm.L = n(22.414 L/mol)
n = (0.36 atm.L) / (22.414 L/mol)
n ≈ 0.016 mol

Step 3: Calculate the molar mass of nitrogen.
To find the gram molecular mass of nitrogen, we divide the given mass (0.45 g) by the number of moles (0.016 mol):
Molar mass = Mass / Moles
Molar mass = 0.45 g / 0.016 mol
Molar mass ≈ 28.13 g/mol

Therefore, the gram molecular mass of nitrogen is approximately 28.13 g/mol.