Consider two samples of ethane: C¿H6 (g) and ethane-d6: C2D6 (g) at -30 °C and 2.0 atm. Deuterium (D) is an isotope of hydrogen with atomic mass = 2.014 amu. Calculate the urms and the fraction of molecules that have speed equal to urms for each of the two ethane samples. With reference to the Boltzmann-Maxwell curve, explain the differences in both ums and the fractions of molecules obtained. Given that 3RT and M 3/2 Mu² F(u) = 47| \2TRT Urms u?e-(ZRT %3D M Predict the ratio of 'rate of effusion of C2H6' to that of C2D6. Show your calculations and reasoning.

A mixture of xenon and methane gases contains xenon at a partial pressure of 354 mm Hg and methane at a partial pressure of 380 mm Hg. What is the mole fraction of each gas in the mixture? хе Xxe XCH, =

Calculate the partial pressure of propane (C3H8) in a mixture that contains equal masses of propane and butane (C4H10) at 50°C and 764 Torr.

A mixture of hydrogen and carbon dioxide gases contains hydrogen at a partial pressure of 619 mm Hg and carbon dioxide at a partial pressure of 179 mm Hg. What is the mole fraction of each gas in the mixture? X. = H₂ хсог =

An experiment is performed to determine the volume of gas produced by the following reaction: 2HCl(aq) + Mg­(s)                  MgCl2(aq) + H2(g) A.  What is the maximum mass of Mg in g that could be reacted at 20oC temperature and 1.0atm, if the volume of the gas burette is 50mL? (Hint: Find moles of H2 using the ideal gas law; then, convert to g of Mg.)   B. If the experiment were moved to a higher elevation and the pressure was decreased to 0.95 atm would the maximum amount of Mg increase or decrease?   C. If 16mg of Mg were reacted, what is the volume of gas produced in this reaction?   D. What is the solvent for this reaction?   E. Would the HCl(aq) be considered a strong, weak, or non-electrolyte?   F. Would the MgCl2(aq) be considered a strong, weak, or non-electrolyte?

A student has a 2.97 L bottle that contains a mixture of O2 , N2 , and CO2 with a total pressure of 4.70 bar at 298 K . She knows that the mixture contains 0.277 mol N2 and that the partial pressure of CO2 is 0.336 bar . Calculate the partial pressure of O2 .

150. g of an unknown monatomic gas phase element has just been released into a container of volume 90.95 L at a pressure of 1.0114 atm. If the temperature of the room is 25.4°C, what are the molar mass and the identity of the gas? molar mass identity of the gas

Everything needed is included. An empty 1.0-liter cylinder is filled with 48.0 grams of methane (CH4 ) at 273 K. 2a. Predict (calculate) the pressure, assuming methane behaves as an ideal gas. 2b. Suppose the pressure is measured and is found to actually be 56 atm. Determine the compression factor Z, and indicate whether attractive or replusive intermolecular forces are dominant in methane under these conditions.

The combustion of gasoline (octane, C8H18) as shown in the following equation is what powers most cars. CO2 is a major cause of climate change. What mass of CO2 is produced by one tank of gasoline that holds 1.63x104 L at a temperature of 80.0°C and a pressure of 101.3 kPa? Plants use the CO2 produced to make glucose and O2. A mature tree can absorb 22 kg of CO2 a year. How many trees are required to absorb the CO2 produced by one tank of gas?  2 C8H18 (g)         ->       25 O2 (g)       ->        16 CO2 (g)       ->     18 H2O (g)

Mass of flask +cap= 96.421g temp. of boiling water= 100 C Mass of flask+ cap+ condensed vapor= 97.005g, 96.957g, 96.984g. Volume of Flask= 160 mL What is the mass of condensed liquid? What is the barometric pressure? What are the molar mass of the Vapors?