Natural gas is very abundant us many Middle Eastern oil fields. However, the costs of shipping the gas to markets in other parts of the world are high because it is necessary to liquefy the gas% which is mainly methane and has a boding point at atmospheric pressure of —164 °C. One possible strategy is to oxidize the methane to methanol. CH3OH. which has a boiling point of 63°C and can therefore be shipped more readily. Suppose that 10.7
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Chemistry: The Central Science (13th Edition)
- How to compact hydrogen to increase its storage efficiency? FO By the definition, universal gas constant, R, is equal to: R=NA*k where R≈ 8.31 J/(mol K), k 1.38*10-23 J/K is a Boltzman constant, and NA is Avogadro number. In what units NA is expressed At which conditions the property of a real gas approach to the properties of ideal gas? 8 List two main factors (in addition to gas pressure) determining hydrogen storage capacity of gas cylinders for the storage of compressed hydrogen gas. 5 How do you calculate efficiency of a compressor starting from its performances? Which compressor performances are necessary for the calculation? ATarrow_forwardA 1.52 g mixture of sucrose (CH,0, 342.30 g mol") and ethyl alcohol (C,H,O, 46.07 g mol") is reacted with acidic aqueous potassium dichromate (K,Cr,0,) solution. Produced 3.12 L CO, (g) is collected over water at 35 °C and has a barometric pressure of 0.52 atm. Water has a vapor pressure of 42.20 mmHg. Calculate the mass percent of C,H,O, in the mixture. CHOlaq) + Cr,O, (aq) - CO.(g) + Cr"(aq) (not balanced) CH.O(aq) + Cr,0, (aq) - CO.(g) + Cr" (aq) (not balanced) Enter only integer number, do not use % sign, Le. 12.345% should be entered as 12. Answer:arrow_forwardAssume 402.46 g of dry ice (solid CO2) is placed in an empty 26.66L closed tank. Determine the pressure in the tank in atmospheres at a temperature of 41.88°C. Assume that all the CO, has been converted into gas. (Molar Mass CO2 = 44.01) K = 273.15 +°C %3D R = 0.08206 (L*atm)/(mol*K) Give your answer to 2 decimal places. 近arrow_forward
- While ethanol CH3CH2OH is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene CH2CH2 with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 2.0L flask at 21.°C with 5.0atm of ethylene gas and 4.2atm of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 3.7atm of ethylene gas and 2.9atm of water vapor. The engineer then adds another 1.7atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.arrow_forwardA sample of propane is placed in a closed vessel together with an amount of O2 that is 3.05 times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole fraction of each component in the resulting mixture after oxidation assuming the H2O is a gas.arrow_forwardIn a diesel engine the fuel is ignited when it is injected into hot compressed air, heated by the compression itself. In a typical high-speed diesel engine, the chamber in the cylinder has a diameter of 10.7 cm and a length of 13.4 cm. On compression, the length of the chamber is shortened by 12.7 cm (a “5- inch stroke"). The compression of the air changes its pressure from 1.00 to 39.7 atm. The temperature of the air before compression is 385 K. As a result of the compression, what will be the final air temperature (in Kand °C) just before the fuel injection? temperature = K = °Carrow_forward
- [References) Use the References to access important values if needed for this question. Sodium metal reacts with water to produce hydrogen gas according to the following equation: 2Na(s) + 2H,0(1)2N2OH(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 755 mm Hg. If the wet H2 gas formed occupies a volume of 5.20 L, the number of moles of Na reacted was mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.arrow_forwardExplain in terms of the Kinetic Molecular Theory the following situations: a) Why does compressing a gas raise the temperature of the system? b) Explain why the density of a gas is so much lower than the density of its liquid form? c) Explain in detail the dissolving process of KCl in water. d) Explain why the solid precipitate AGl (s) forms when solutions of KCl (aq) and AgNO3 (aq) are mixed.arrow_forwardQ\3: Oxygen gas produced from the reaction below was collected above the water at 30 Cº and in a container has capacity 150 cm³ until the total pressure reached 80.0 kPa. → 2KCl + 30₂ 2KC103 If the vapor pressure of water at 30 Cº equal to 4.24 KPa. Determine: 1. The mass in (g) of dry oxygen produced. (8 degree) 2. The mass in (g) of KClO3that consumed in reaction. (7 degree) g g {K = 40 g mole ,0 16- -, Cl = 35.5- ,R 8.314- mole mole N.m mole. Karrow_forward
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