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- 5. Gases: You analyze that principal components of a gas inside a valve. Through spectroscopy, you were able to analyze that components of the gas mixture are 02, N2 and H2 respectively. From that you would like to check if you have learned something from GCHEM203A by determining (a) what are the mole fractions of each component in the mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2? (b) What is the partial pressure in atm of each component of this mixture if it is held in a 15.50-L vessel at 15 °C?6. A gas mixture contains 2.01 mol F, and 1.85 mol CH, with a total pressure of 150. kPa. What is the mole fraction and partial pressure (in kPa) of each gas? A: 0.521; 78.1; 0.479; 71.9A gas mixture consists of 0.62 percent N, and 0.38 percent CO, by mole basis. Take 1 kg mole of the mixture and the molecular weight of N2 and CO2 are 28 and 44 kg/kg.mol respectively. Determine the (i) mole fractions of the constituents, (ii) mass fractions of constituents, (ii) the average molar mass of the mixture, and (iv) the average gas constant of the mixture. Take universal gas constant is 8.314 kJ/k mole.K. mole fraction of N2 mole fraction of CO2 Mass fraction of N2 Mass fraction of CO2 Molar Mixture Mixture gas constant
- Calculate mole fraction of each component in a reaction vessel of volume 24.4 dm containing 1.0 mol H2 and 2.5 mol N2 at 298.15 K. OA.XN = 0.63; XH=0.37 %D O B. XN = 0.25; XH= 3.5 %3D OUYND0.15; XH=0.37 OD.XN = 0.25; XH=0.63 OE. XN = 0.72; XH= 0.37A mixture of ideal gases possesses the properties listed in table below when examined at 2 bar and 22 C giving the following gravimetric analysis. A: 20% ; B: 25% ; C: 30%; D 25% Find for the mixture: • Volumetric analysis. • Gas constant. • Enthalpy. Partial pressure for each constituent Gas A Kg/kmol 28 16.7 24.2 21.3 M 18 14 46 C, kJ/kmol K 20.6Gas Pressure Conversions • A given P(atm) takes different column heights (h) of different liquids (p) to balance in a barometer: P(H,0) = p(H,O) gn h(H,0) P(atm) = p(Hg) g, h(Hg) 1 h oc %3D %3D ... Find mm(H,0) that measures 1 atm = 760 mmHg: %3D h(H,O) = h(Hg) x e(Ha= 760 mm(Hg) x 13.5_g/mL = [O,2le0 mm(H,O) %D %3D p(H2O) 1.0 g/mL A barometer with liquid twice as dense as water shows 1 atm as: 0.38 m 1.52 m 5.15 m 20.6 m Convert 3.11 x 10-5 atm into mTorr 1 atm =100 Torr 3.11 x 10-5 atm xloO Torr 1 atm 1 mTorr 10-3 Torr 23.0mTorr (AKA: µ) 1 in(Hg) = 25.t mm(Hg) Pa = 29.92 inHg 80.6 KPa Convert 23.8 inHg into kPa %3D 1 atm = 760 mmHg = (01325 25.4 mm(Hg)x 1 in(Hg) %3D 101325 Pa 760 mmHg 1o Pa 23.8 inHg x x 1 kPa =
- Gas from a coal bed percolates up to the shallow, permeable strata containing groundwater. Methane (CH,, 16.0 g/mol) in the gas has a partial pressure of 0.029 bar. What is the concentration of methane in groundwater if ky is 23 g-bar-1-m-3?Pressure (A) Explain the term pressure and state its S.I. unit. (B) Explain Henry’s law. (C)A bottle of H2 has just been received by the technicians in DkIT for use in the instrumentation lab. It is a 47 litre cylinder at a pressure of 50 atmospheres. The normal working pressures is 2 bar. (i) To what volume of gas will that equate at the working pressure? (ii) For how many hours will the gas last if it used at the rate of 0.5dm3 per hour? D)You see your best friend at the bar and you walk up behind her. You accidentally startle her and she takes a step backwards. Unfortunately, she is wearing high heels and her heels come down on your foot. She weighs only 55kg but the size of her heel is 6mm by 6mm.Determine the pressure that she applies on your foot. (E) If a diver dives to a depth of 35 m what will be: (i) the pressure in Pascals due the water column? (3 marks) (ii) the pressure of the air in…← Aktiv Chemistry KU Portal < 59°F Cloudy X + https://app.101edu.co Ch. 1 Introduction -... Aktiv Chemistry |||| CG Grade Calculator ... Connect-Bio Google Docs Hi What quantity in moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 12.0 L? Q Search Question 14 of 25 R Point Grade Calcula... r a C D Class Search How to Start a
- P 1) Pinte X A ACTIVITY X EX_FjXNtRGOvhgYzM_rMIZzEwnvfJ17evaEjsK94/edit# Last edit was 2 minutes ago 11 BIUA 田回▼ 1三 ニ=,E▼E ... .. 1. Calculations A. Direction: Calculate the given problems and use the gas laws to determine pressure, volume, or temperature of a gas under certain conditions of change. Show your solutions. Encirce your final answer. 1. The gas inside the tire has a volume of 20.00 L at a pressure of 5.00 atm. Calculate the pressure of the gas if its volume is reduced to 10.0 at the same temperature. 2. If 150.00 mL of N2 gas was collected at 760 torr, what is the new volume of the gas when the pressure is compressed to 740 torr at the same temperature? 3. At 300 K, the given amount of fluorine gas has a volume of 30.0 L. What will be the temperature if the gas occupies a volume of 25 L at constant pressure? 4. A certain gas sample has a volume of 40.00 L at 273 K. At constant pressure. the volume increase to 50 00 L What will be the final temperature of the gas? 5 At…Prove that M = (mole IL) %3D is % x 10 x d M. M.wtD. At 25 oC, the mole fraction of N2O4 in an N₂O4/NO2 mixture is 0.35. At 35 oC, the mole fraction of N2O4 is 0.29. What is the mole fraction of N₂O4 at 30 °C?