volume = 322 mL
temperature = 150 celcius
pressure = 175 kPa
mass = 0.448
Calculate the molar mass of the gas.
First I converted volume to 0.332 L.
Second I converted 150 celcius into 423 kelvin.
PV = nRt
(175)(0.322) = n(8.314)(423)
n= 0.016022988
molar mass = 0.448/0.016022988
= 30.5 g/mol
If the gas is known to be diatomic, predict it's identity.
I divide the 30.5 by 2 to get 15.25. That number falls inbetween nitrogen and oxygen so i'm not too sure which one it would be. Apparently there is one correct answer. Im not too sure if I did the first part correctly :S
The first part looks ok for the method but I think you made a bobble on the calculator. I get something closer to 28 than 30. And 1/2 of about 28 would be about 14 which would be ok.
I did make a mistake on my calculator. Thanks a lot :)
To calculate the molar mass of the gas, you correctly converted the volume to liters and the temperature to Kelvin. Then you used the ideal gas law equation 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.
You substituted the values given into the equation and solved for n:
(175 kPa)(0.332 L) = n(8.314 kPa L/mol K)(423 K)
n = 0.016022988 mol
Next, you divided the given mass (0.448 g) by the number of moles (0.016022988 mol) to find the molar mass:
molar mass = 0.448 g / 0.016022988 mol = 27.95 g/mol
So the molar mass of the gas is approximately 27.95 g/mol.
To predict the identity of the gas, you divided the molar mass by 2 assuming it is diatomic. However, this approach is not correct because diatomic gases have formulas like N2 and O2, where the molar mass would be the sum of the atomic masses of the elements.
Since the molar mass you calculated falls between nitrogen (28.02 g/mol) and oxygen (31.99 g/mol), the gas is likely either nitrogen or oxygen. Without additional information or more precise measurements, it is difficult to determine the exact identity of the gas.