There is 2.878 x 10-4 mol of an unidentified gaseous substance effuses through a tiny hole in 98.9 s. Under identical conditions, 1.740 x 10-4 mol of argon gas takes 61.5 s to effuse. What is the molar mass of the unidentified substance (in g/mol)? What is the molecular formula of the substance? Under identical conditions, how many moles of ethene (C2H4) gas would effuse in 91.0 s?

A gas of unknown molecular mass was allowed to effuse through a small opening under constant pressure conditions. It required 72 s for 1.0 L of the gas to effuse. Under identical experimental conditions it required 27 s for 1.0 L of 02 gas to effuse. Calculate the molar mass of the unknown gas. (Remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0 L; that is, rate and time are inversely proportional.) 367.1175859 X g/mol

MI < CO C. Under identical conditions, separate samples of O2 and an unknown gas were allowed to effuse through identical membranes simultaneously. After a certain amount of time, it was found that 5.75 mL of O2 had passed through the membrane, but only 3.86 mL of of the unknown gas had passed through. What is the molar mass of the unknown gas? unknown molar mass: g/mol MacBook Pro The %23 %$4 delet 4. 5. 3. R. P. H. K. B. MOSISO command uondo

It takes 66.2 s for an amount of Kr(g) (molar mass = 83.80 g/mol) to completely escape from a container through a small opening. It takes 75.2 s for the same amount of an unknown gas to completely escape from the same container under identical conditions. Identify the unknown gas.

A sample of H2(g) was collected over water in a volume of 12.0 mL at 18 °C under atmospheric pressure of 770. Torr. Partial pressure of water is P(H2O, 18 °C) = 16 Torr. Find the mol’s of H2(g) in the sample

A sample of O3 gas is observed to effuse through a pourous barrier in 1.06 minutes. Under the same conditions, the same number of moles of an unknown gas requires 0.736 minutes to effuse through the same barrier. The molar mass of the unknown gas is g/mol.

A 8.00 L tank at 29.8 °C is filled with 14.1 g of chlorine pentafluoride gas and 17.2 g of boron trifluoride gas. You can assume both gases behave as ideal gase under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas chlorine pentafluoride boron trifluoride mole fraction 0 0 X

A sample of nitrogen gas at a pressure of 888 torr and a temperature of 24.4°C, occupies a volume of 646 mL. If the gas is compressed at constant temperature until its pressure is 1050 torr, the volume of the gas sample will be mL.

A 9.00 L tank at 8.6 °C is filled with 11.0 g of sulfur tetrafluoride gas and 9.86 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas sulfur tetrafluoride dinitrogen difluoride mole fraction 1 0 X S

A 7.00 L tank at 19. °C is filled with 7.37 g of sulfur hexafluoride gas and 6.63 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. sulfur hexafluoride sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: a atm 0 atm atm x10 X Ś