An unknown gas contains 88.8% C and 11.2% H. At 0.404 atm and 435 K, the gas has a density of 0.612 g/L. What is the molecular formula of the gas?

A 3.45 g sample of an unknown gas at 43 °C and 1.10 atm is stored in a 1.85 L flask. What is the density of the gas? density: g/L What is the molar mass of the gas? molar mass: g/mol

A 3.25 g sample of an unknown gas at 37 °C and 1.00 atm is stored in a 1.85 L flask. What is the density of the gas? density: g/L What is the molar mass of the gas? molar mass: g/mol

A 1.85 g sample of an unknown gas at 47 C and 1.00 atm is stored in a 2.85 L flask. What is the density of the gas? density: g/L What is the molar mass of the gas? molar mass: g/mol

A gaseous compound has a density of 1.40 g/L at 21.8 °C and 1.34 atm. What is the molar mass of the compound? molar mass: g/mol

If 1.52 g Ar are added to 3.41 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of the resulting gaseous mixture? Ptotal = atm

A sample of an ideal gas with an initial volume of 18.0 L at a pressure of 679 mm Hg is compressed until the volume is 3.4 L with no change of temperature. What is the final pressure (mm Hg) of the gas?

A 2.65 g sample of an unknown gas at 21 °C and 1.10 atm is stored in a 1.05 L flask. What is the density of the gas? density: g/L What is the molar mass of the gas? molar mass: g/mol

A gas mixture contains 0.600  mol of N2, 0.200  mol of H2, and 0.250  mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 9.00  L vessel at 27.00°C. What is the total pressure of the vessel and the pressure of N2, H2, and CH4 in atm?

A 3.35 g sample of an unknown gas at 79 °C and 1.00 atm is stored in a 2.15 L flask. What is the density of the gas? density: g/L What is the molar mass of the gas? molar mass: g/mol