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- Calculate the volume occupied by 11.2 g of the gas at NTP. Given that the vapour density of a gas is 11.2.ons/17136 V/suonsənb/əxeı/6 177 1. This is the data sheet for Molar mass of vapor; 1. Unknown Liquid #:N/A 2. Mass of flask+ cap + rubber band 56.45 g se 3. Temperature of boiling water 97 °C ३ 4. Barometric Pressure 755.7 mmHg 5. Mass of flask + rubber band + cap + condensed vapor_57.88 6. Mass of condensed vapor 7. Volume of flask 243.8 mL 8. Molar Mass of Vapor g/mol What is the molar mass of vapor? O 179200 O 1.79 0179.2 N beatsqudioIn a Victor Meyer Experiment involving the determination of the molecular weight of ethyl alcohol the data obtained were Wt. of liquid taken = 0.1211gVolume of air measured over water=67.30ccTemperature=28.0CAtmospheric pressure=755.2mmHg Vapor pressure of water at 28C = 28.3 mmHg From these data (a) calculate the molecular weight of the alcohol and (b) compare the result with that calculated from the atomic weights.
- The Molecular Weight of an unknown liquid is determined using the Dumas Method. The following data has been obtained: Atmospheric Pressure = 754.6 TorrVolume of the Flask = 213 mLTemp. of Water Bath = 100 °CMass of Re-Condensed Liquid = 0.582 g What is the Molecular Weight of the liquid?1. A vessel of volume 24.4 dm3 contains 1.0 mol H2 and 2.5 mol N2 at 298.15 K. Calculate(a) the mole fractions of each component, (b) their partial pressures, and (c) their totalpressure. 2. The critical constants of carbon dioxide are Pc = 72.85 atm, Vc = 94.0 cm3 mol–1, and Tc =304.2 K. Calculate the van der Waals parameters of the gas. Please provide complete solutions.The density of nitrogen at its critical point is 0.3131 gcm-3 . At a very low temperature, 0.3131 g solid nitrogenis sealed into a thick-walled glass tube with a volume of1.000 cm3 . Describe what happens inside the tube as thetube is warmed past the critical temperature, 126.19 K.
- A sample of vapor weighing 0. 200 g occupies a volume of 55 cc at 270C and 760 mmHg pressure. The critical pressure of the vapour is 47.7 atm, while the critical temperature is 288.50C. by use of the Berthelot equation, calculate the molecular weight of the vapour, and compare the result with that calculated by the ideal gas law.What would be the volume of 2.0 moles of a gas vapours having pressure of 4.994 Nm-2at 298 K using idealgas equation and Van der Waal’s equation. (a = 2.576 Nm4 mol-2, b = 0.1453 x 10-3 m3 mol-1A volatile hydrocarbon (a binary compound of carbon and hydrogen) was determined to be 92.3 % carbon, by mass. In a separate experiment, utilizing the Dumas method, 4.00 mL pure liquid sample of this hydrocarbon is vaporized in an Erlenmeyer flask when the barometric pressure is 768.0 torr. The empty flask was fitted with a foil cap pierced with a pinhole and weighed 25.3478 g. After the excess gas escaped, the temperature was measured as 98.0 °C. The flask and contents were subsequently cooled to 25 °C and the vapor condensed into a liquid. The weight of the flask and contents is found to be 25.6803 g. The exact volume of the flask was determined to be 128.5 mL. Using this information, determine both the empirical and molecular formula of this hydrocarbon. Show/explain the steps of your work.
- Show that the following equation can be used to calculate the percentage of nitrogen in a sample having a mass of W grams when the N₂ has a volume of V mL and is collected over water at t in °C at a total pressure of P in torr. The vapor pressure of water occurs in the equation as Po H₂0 Percentage N = 0.04489 x The equation can be rearranged to give: 0.04489 x 0.4489 x 0.04489 x 0.04489 x P – PÅ₂0) V (P PH₂0) W (273 + tc) 273 + tc V(P - P₂0) 273 + tc V(PH₂0 = Percent N x W P) 273 + tc 273 + tc V(P PH₂0) = Percent N x = = W Percent N x W Percent N x WThe vaporization of water is one factor that contributes to the raising of baked goods. When 1.0g of water is vapourized inside a cake at 150c and 105kPa what volume in L of vapour is produced?If 0.80 g of the vapor of the unkknown liquid occupied 280ml at 100 degrees celcius and 750 mm Hg, calcuate the molecular weight of the liquid