To calculate the molar mass of the molecule, we first need to find out what molecule it is. Since you have mentioned it contains both carbon and oxygen, it could be either carbon monoxide (CO) or carbon dioxide (CO2).
Assuming it is carbon dioxide, which is more commonly encountered, we can use the Ideal Gas Law to find the number of moles of CO2 in 1 liter at STP (Standard Temperature and Pressure, which is 0 degrees Celsius and 1 atm pressure).
The Ideal Gas Law states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
At STP, the pressure is 1 atm, the volume is 1 liter, and the temperature is 273 K (0 degrees Celsius + 273).
So, we have:
PV = nRT
(1 atm)(1 L) = n(0.0821 L atm/mol K)(273 K)
n = 0.040 mol CO2
Now, we can calculate the mass of CO2 in 1 liter at STP using its density of 6.02 g/L:
mass = density x volume
mass = (6.02 g/L) x (1 L)
mass = 6.02 g
So, the molar mass of CO2 is:
molar mass = mass / number of moles
molar mass = 6.02 g / 0.040 mol
molar mass = 150.5 g/mol
Therefore, the molar mass of the carbon and oxygen molecule, assuming it is carbon dioxide, is 150.5 g/mol.