Multiple Choice
What is the mass (in grams) of 10.00 L of propane vapor (C₃H₈) at STP?
7. Gases
The Ideal Gas Law: Molar Mass
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An unknown gas has a density of 0.0262 g/mL at a pressure of 0.918 atm and a temperature of 10°C. Using the Ideal Gas Law, what is the molar mass of the gas?
A
44.01 g/mol
B
2.02 g/mol
C
16.04 g/mol
D
28.96 g/mol
Verified step by step guidance1
Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature: \( T = 10 + 273.15 \).
Use the Ideal Gas Law in the form \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is temperature in Kelvin.
Rearrange the Ideal Gas Law to solve for molar mass \( M \): \( M = \frac{dRT}{P} \), where \( d \) is the density of the gas.
Substitute the known values into the equation: \( d = 0.0262 \text{ g/mL} \), \( R = 0.0821 \text{ L atm/mol K} \), \( T \) in Kelvin, and \( P = 0.918 \text{ atm} \).
Calculate the molar mass using the rearranged equation and the substituted values to find the molar mass of the gas.
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