In a Dumas bulb experiment, a 1.862-g sample of an organic compound vapor, containing C, H, and O, occupies 1.00-L volume at 120.0C and 760 Torr.  The solvent is 40.00% C and 53.28% O by mass.  What are : (a) the molar mass, and (b) the omlecular formula of the compound? (Answer in sig figs)

A sample of CH4 gas occupies a volume of 575 mL at -25 ºC. If pressure remains constant, what would be the new volume if the temperature changes to: (a) 298 K (b) 32 ºF (c) 45 °C

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2. A chemist collects 3.97 g of NH3) and 4.89 g of O2) and has a total pressure of 23.78 torr calculate the mole fraction and partial pressure of both NH3G) and O2o)-

A sample of gas occupies 100cm3 at 0 degrees C and 1 bar pressure. (a) What is its volume at 50 degrees C and 1 bar pressure? At 0 degrees C and 2.2 bar pressure?

The effusion rate of a gaseous compound at a certain temperature and pressure is 25.0 mL/min. Under the same conditions, the diffusion rate of N, is 57.1 mL/min. (a) Calculate the molar mass of the unknown compound. (b) If the compound is composed of 21.95% S and 78.05% F, by mass, what is the empirical formula of the compound?

What is the mass (in grams) of 24.50 L of propane vapor (C₃H₈) at STP? R = 0.08314 L･bar/mol･K.