Given a sample of gas (2.49 g) with a volume of 752 mL at 335K and 1.98 atm, what is the gas, SO2 or NO2?

PV=nRT
(1.98atm)(0.752L)= X (0.08206L-atm/mol-K)(335K)
X = 0.0541634989

mol= g/gfm

2.49/X= 0.0541634989
X = 45.97

NO2 has 46g, whereas SO2 is 64.1g.

Therefore, would the solution be NO2?

NO2 is correct but you have too many s.f. again. You are allowed three s.f., (from the 1.98) so the answer of 45.97 would round to 46.0 = molar mass.

Well, based on the calculations, it seems like the gas is NO2, which weighs approximately 46 grams. So, yeah, NO2 seems to be the answer. But to be honest, I don't really get NO2's choice of name. I mean, what kind of gas wants to go by the name "NO2"? It sounds more like a license plate number than a gas. Maybe it should go see a gas name therapist.

Yes, based on the calculations, the solution would be NO2. The molar mass calculated for the gas sample is approximately 45.97 g/mol, which is closer to the molar mass of nitrogen dioxide (NO2) at 46 g/mol than to sulfur dioxide (SO2) at 64.1 g/mol.

Yes, based on the calculations, the gas in the sample is most likely NO2. To determine the identity of the gas, the ideal gas law equation, PV = nRT, is used. In this equation, P refers to pressure, V refers to volume, n refers to the number of moles of the gas, R is the ideal gas constant, and T refers to the temperature.

First, the variables are plugged into the equation: (1.98 atm)(0.752 L) = X (0.08206 L-atm/mol-K)(335 K).

Simplifying the equation, we get: 1.48696 = 0.0541634989X.

To find the number of moles (n), we rearrange the equation to get: X = 2.49 g / n.

Using the calculated value for X from the previous step, we set up an equation: 2.49 g / 0.0541634989 = 45.97 g/mol.

Comparing this value to the molar masses of SO2 (64.1 g/mol) and NO2 (46 g/mol), we can see that the closest match is NO2 with a molar mass of 46 g/mol.

Therefore, the gas in the sample is most likely NO2.