Textbook Question
Cyclopropane, a gas used with oxygen as a general anesthetic, is composed of 85.7% C and 14.3% H by mass. a. If 1.56 g of cyclopropane has a volume of 1.00 L at 0.984 atm and 50.0°C, what is the molecular formula of cyclopropane?
7. Gases
The Ideal Gas Law: Molar Mass
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A sample of gas has a mass of 0.311 g. At 55°C, its volume is 0.225 L and its pressure is 886 mmHg. Find its molar mass using the Ideal Gas Law.
A
18.0 g/mol
B
28.0 g/mol
C
44.0 g/mol
D
32.0 g/mol
Verified step by step guidance1
Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature: T(K) = 55 + 273.15.
Convert the pressure from mmHg to atm using the conversion factor: 1 atm = 760 mmHg. Calculate the pressure in atm: P(atm) = 886 mmHg / 760 mmHg/atm.
Use the Ideal Gas Law equation: PV = nRT, where P is pressure in atm, V is volume in liters, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is temperature in Kelvin.
Rearrange the Ideal Gas Law to solve for n (number of moles): n = PV / RT.
Calculate the molar mass by dividing the mass of the gas sample by the number of moles: Molar Mass = mass (g) / n (moles).
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