Calculating Molar Mass with the Ideal Gas Law
The table below provides data for a sample of an unknown gas. Based on the ideal gas law, which of the following shows the correct calculation for the molar mass of the gas?
| Parameter | Value |
|---|---|
| Density (D) | 1.50 g/L |
| Pressure (P) | 1 atm |
| Temperature (T) | 298 K |
| Gas Constant ® | 0.0821 L·atm/(mol·K) |
A
Calculating molar mass by dividing the density by the product of R and T
B
Using $$MM = \frac{D * R * T}{P} = \frac{1.50*0.0821*298}{1} \approx 36.7\;g/mol$$
C
Multiplying density by pressure and temperature to obtain molar mass
D
Assuming the density is equal to the molar mass without any calculation
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