Calculating Molar Mass with the Ideal Gas Law

Question

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 (R)           | 0.0821 L·atm/(mol·K)     |

Accepted Answer

Using $$MM = \frac{D * R * T}{P} = \frac{1.50*0.0821*298}{1} \approx 36.7\;g/mol$$

Answer

Calculating molar mass by dividing the density by the product of R and T

Answer

Multiplying density by pressure and temperature to obtain molar mass

Answer

Assuming the density is equal to the molar mass without any calculation

Rank	User	Correct Count	Attempt Count	Total Time	Score
#1	biancahoria86	2	2	0m 32s	168
#2	jerrykim0814	1	1	0m 00s	100
#3	mrorangelaw	1	1	0m 09s	91
#4	kkat.s.music	1	1	0m 11s	89
#5	Derinchiay2013	1	1	0m 17s	83
#6	priyamk1122008	1	1	0m 20s	80
#7	sukaria27	1	1	0m 45s	55
#8	28joseph	1	1	0m 58s	42
#9	batoolmas25	1	1	1m 03s	37
#10	choiyumi0228	1	4	0m 47s	23

Parameter	Value
Density (D)	1.50 g/L
Pressure (P)	1 atm
Temperature (T)	298 K
Gas Constant ®	0.0821 L·atm/(mol·K)

Calculating Molar Mass with the Ideal Gas Law

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