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- Ammonia is produced industrially by reacting N2 with H₂ at elevated pressure and temperature in the presence of a catalyst: N₂(g) + H₂(g) → NH3(g) (unbalanced) In actual practice, this reaction gives a yield of only 13%, taking this into account what mass of ammonia would be produced from a 1:1 mole ratio mixture in a reactor that has a volume of 3.91 x 103 L, under a total pressure of 116 bar at T = 632 °C? Actual amount = g مه7. A technician is setting up a laboratory to standardise ~0.0200 mol dm–3 KMnO4. What mass of Mohr’s salt [FeSO4(NH4)2SO4·6H2O] would the technician be required to weigh out to produce a 5.00 L solution of Mohr’s salt such that 25.0 cm3 aliquots of the salt would require a titre of 20.0 cm3 to standardise the KMnO4 solution?what is obtained when CaC2 is heated in nitrogen at 1000 degree celsius ?
- 2. a. Given the following composition, calculate the average molar mass of air. Molar ratio: Nitrogen: 78%, oxygen: 21%, argon: 0.93%, carbon dioxide: 0.04%, and water. I b. Calculate the concentration of CO2 in ppm. c. Imagine a parallel universe, in which nitrogen has a structure similar to P4. What kind of changes would you expect in the composition of air and earth's crust? d. Assume that there is hypothetical Ns molecule, in which each nitrogen atom makes a total of 3 bonds since it is a group V element. Draw a feasible structure for N8.A 2.5 L canister under a pressure of 150 kPa at 20 °C is compressed to a volume of 1.5 L at 35 °C. What is the resulting pressure? K H Li Be Na Mg "K Ca Sc Ti V Cr Rb Cs Fr Ba Ra La La 158.2 kPa 329.3 kPa 56.8 kPa 180.3 kPa 98.3 kPa 262.8 kPa M 89-108 104 M Hf Ta Ac Metal Rf Db Sg Periodic Table of the Elements W Re Os A He Aline TH Symbel 41 42 M45 Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Basic 13 IKA LAS B Pt MAN 14 VE 15 AI Si P 17 VILA Cl w! Mn Fe Co NI Cu Zn "Ga Ge As Se Br Kr Neble LIONS Au Hg Tl Pb Bi Po At Rn 108 10 Sg Bh Bh Hs Mt Ds Rg Cn Uut "FI Uup "Lv Uus Uuo VIA He Ne 18 Yb Lu Pa U Np Pu Am Cm Bk Cf Es Fm Md No Ar(Record your answer with rounded answer to proper significant digits and the proper units.) 1.How many moles of butane (C4H10(g)) were combusted in the presence of excess oxygen gas if 55.8 L of water vapour at STP is collected?Hint: Write a balanced chemical reaction equation first. 2.One of the steps to sweeten sour gas using the Claus process is reacting hydrogen sulfide gas with sulfur dioxide gas to produce water vapour and sulfur. 16H2S(g)+8SO2(g)----->16H2O(g)+3S8(s) 8.75 kL of hydrogen sulfide at 175 kPa and 250 °C reacts with excess sulfur dioxide. Calculate the mass, in kg, of sulfur produced.
- 3C. and 3HThe nitrogen content of organic compounds can be determined by the Dumas method.The compound in question is first passed over hot CuO(s): Compound N2(g) + CO2(g) + H2O(g) The gaseous products are then passed through a concentrated aqueous KOH solution to remove the CO2.The remaining gas contains N2 and water vapor.A 0.127-g sample of a compound was treated as above, producing 89.0 mL of N2 saturated with water vapor at 25 °C and 739.3 torr.What is the mass percent of nitrogen in the compound? . The vapor pressure of water at 25 °C is 23.8 torr.16. The combustion of gasoline (octane) in a car engine can be represented by the following equation: 2C3H18(1) + 2502(g) a. What mass of oxygen is used up to burn a full tank of 36.00 kg of gasoline? Text --> 16CO2(g) +18H20(g) b. Why might a vehicle that is calibrated to run perfectly at sea level run poorly at higher elevations? Text Тext According to the Canadian Automobile Association, the average Canadian drives 20,000 km/yr. C. Assuming that distance, how many more kg of carbon dioxide are added to the atmosphere each year by a Toyota Tacoma (fuel economy of 12.8 L/100 km) than a Toyota Prius (4.52 L/100 km)? The density of gasoline is 0.719 kg/L.
- From the sequential hydrolysis of ammonia borane in 10 mL aqueous solution at 25 ºC and 1 atm with 2 mM Rh catalysis, 730.4 mL H2 was obtained in 8 hours. What is the TON of the catalyst used in the reaction?In 1897 the Swedish explorer Andree tried to reach the North Pole in a balloon. The balloon was filled with hydrogen gas. The hydrogen gas was prepared from iron splints and diluted sulfuric acid. The reaction is Fe(a) + H,S0, (ag) + PeSO(og) + H;(s) The volume of the balloon was 4800 m and the loss of hydrogen gas during filling was estimated at 20% What mass of iron splints and 98 (by mas) H,S0, were nooded to enre the complete filling of the balloon? Assume a temperature of oC, a presaure of 10 atm during filling nd 100 yield. Mass of Fe Mass of HaS0, -What is the difference between a CFC and an HFC?
