Calculate the mass of water vapor present in a room of volume 400 m3 that contains air at 290C when the relative humidity is 53.0%. Compute for the vapor pressure of water?
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1. Calculate the mass of water vapor present in a room of volume 400 m3 that
contains air at 290C when the relative humidity is 53.0%. Compute for the vapor
pressure of water?
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- Show complete solutions and enclose all final answers in a box. Round off final answers to 4 decimal places and use floating values for intermediate answers. A gas column is separated into two segments by a non-permeable partition. On the first segment is 1.63 moles of Helium with volume V1 and on the second segment is 3.84 moles of Oxygen gas with volume V2. Consider both gases to be ideal and at the same pressure P and temperature T. If the partition is removed, calculate the change in entropy of the gaseous system.Constants | Periodic Table Eleanoron gas is a newly discovered toxic gas with a very noxious odour. A sample of Eleanoron is collected over water at a temperature of 310 K . A volume of 1.38 Lof gas is collected with a total pressure of 1,175 bar. The vapour pressure of water at 310 K is 46.12 mmHg Determine the partial pressure of the Eleanoron gas, in units of bar. Express your answer using four significant figures. P = 1.114 bar Submit Previous Answers Completed Part B The partial pressure of the Eleanoron gas is 1.114 bar. If the density of the gas at this temperature is 2.81 g· L, determine the the molar mass of Eleanoron gas. Express your answer to three significant figures. ? MM = g mol1Eleanoron gas is a newly discovered toxic gas with a very noxious odour. A sample of Eleanoron is collected over water at a temperature of 310 K.A volume of 1.38 Lof gas is collected with a total pressure of 1.175 bar . The vapour pressure of water at 310 K is 46.12 mmHg . Part A Determine the partial pressure of the Eleanoron gas, in units of bar. Express your answer using four significant figures. V AE ? P = bar Submit Request Answer
- 1. A piece of metal "X" weighing 0.0382 g was placed in an eudiometer containing dilute aqueous HCI. After the metal fully dissolved,15.4 mL of hydrogen gas was collected by displacement of water and a 400 mm column of water was observed. The water temperature was 25 degrees Celcius and the barometric pressure was 758.8 mm Hg (torr). Refer to the introduction and data sheet to solve the following problems. a) Calculate the volume occupied by the hydrogen gas at STP. b) How many moles of the metal were consumed in the reaction? c) What is the molar mass of the metal?A gas mixture of 2.31 g NH3, 31.2 g N2, and 0.58 g mol of H2O vapor is contained at a total pressure of 89. mmHg and 336 K. assuming ideal gas behavior.Solve for; 1. volume percent composition of the mixture2. partial pressure of each component3. total volume of the mixture4. density of the gas mixturePS. Solution without explanations is okay, as long as the solution is understandableUnder constant-pressure conditions a sample of hydrogen gas initially at 47°C (320K) and 6700 mL is heated to 122°C (395K). What is the final volume?
- Calculate the mass of dissolvednitrogen at 25°C in an aquariumcontaining 64.7 L of water. Assume thetotal pressure is 97.8 kPa and the molefraction of nitrogen in air is 0.78.Recall that the partial pressure ofa gas in a gas mixture can bedetermined from the full pressure andits mole fraction (Henry's law, Dalton'slaw).Bottle Volume (10L) Contain mixture (210ml CH4) (500mL H₂) (600mL N₂) at 25 C. Colculate :- The Pressure in bottle The partial Pressure Seach gas.Calculate the molar volume of water at 50 ºC and 1 atm, and at 50 ºC and100 atm.Data: ρ50 ºC, 1 atm = 0.98804 g/cm3; κ = 4.4•10-10 Pa-1.
- A piece of metal "X" weighing 0.0382 g was placed in an eudiometer containing dilute aqueous HCI. After the metal fully dissolved ,15.4 mL of hydrogen gas was collected by displacement of water and a 400 mm column of water was observed. The water temperature was 25 degrees Celcius and the barometric pressure was 758.8 mm Hg ( torr). Refer to the introduction and data sheet to solve the following problems. a) Calculate the volume occupied by the hydrogen gas at STP. b) How many moles of the metal were consumed in the reaction? c) What is the molar mass of the metal?What is w when 1.83 kg of H20(1), initially at 25.0 °C, is converted into water vapour at 185 °C against a constant external pressure of 1.00 atm? Assume that the vapour behaves ideally and that the density of liquid water is 1.00 g/ml (Remember to include a+or-sign as appropriate.) Enter your answer in acceptable SI units, accurate to 3. significant figures. Use an acceptable Sl symbol for units.Deviations from ideal behavior occur at low concentrations True or False