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- An important process for the production of acrylonitrile (C3H3N) (U.S.production is greater than 109 lb) is given by the following reaction: 2C!H"(?) + 2NH!(?) + 3O#(?) H⎯⎯⎯J 2C!H!N(?) + 6H#O(?)A 150.-L reactor is charged to the following partial pressures at 25°C: ? = 0.500 MPa? = 0.800 MPa ? = 1.500 MPa What mass of acrylonitrile can be produced from this mixture (MPa = 106 Pa)?1) Commercial fuming Sulphuric acid (Oleum-H2S2O6) is 99.9% solution. Please convert it into molarity.2) Find out the Volume (dm3) of product (gas) at RTP when 0.58 M, 150 mL NaOH (aq.) reacts with 350 mL, 0.25 NH4Cl.There is actually something im confused about, when you calculating V0 for S0=200uM --> V = 0.48*200/ 2.42 + 1 Why are you only using the S0 value=200uM one place in the equation and then using the S0 value from given data the second place in the equation? Shouldnt S0 be 200 uM both places in the equation?
- Your body deals with excess nitrogen by excreting it in the form of urea, NH2CONH2. The reaction producing it is the combination of arginine (C6H14N4O2) with water to give urea and ornithine (C5H12N2O2). C6H14N4O2 + H2O ? NH2CONH2 + C5H12N2O2 [Molar masses: 174.2 18.02 60.06 132.2] If you excrete 95 mg of urea, what quantity of arginine must have been used? What quantity of ornithine must have been produced?1)Please express the normal salt (NaCl) concentration in body fluid into molarity (mM).2) Commercial fuming Sulphuric acid (Oleum-H2S2O6) is 99.9%. solution. Please convert it into molarity.3) Find out the Volume (dm3) of product (gas) at RTP when 0.58 M, 150 mL NaOH (aq.) reacts with 350 mL, 0.25 NH4Cl.4) The above reaction has the product Ammonia, which when dissolved in 650 mL ethanol makes an alkaline ethanolic solution. Find its molarity (M) 5) Calculate the adult dose as per the BW of the baby. (Child dose-50 mg and the BW of the baby is 48 lb (British pound) (1lb=0.453 Kg)Inorganic Chem Please help answering this question Use equation V = (N)(q1)(q2)(k) / r where k = 9.0x10^9
- Chemistry In an analysis of the content of carbohydrate present in a glycoprotein, the following results were found: 12.6, 11.9, 13.0, 12.7 and 12.5 g of carbohydrate per 100 g of protein. Taking into account that σ is unknown, the confidence interval for the average value at a 90% confidence level of the carbohydrate content is: Select one:to. 12.5 ± 0.4b. 12.5 ± 0.2c. 12.5 ± 0.5d. 12.5 ± 0.3Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.07(a) A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas City (MCI) to Baltimore (BWI) burned 11,800 lb (about 1700 gallons) of Jet A fuel en route. Jet A fuel is kerosine based, consisting primarily of CnH2n+2 hydrocarbons, with n =6 to 16, so the carbon:hydrogen ratio is close to 1:2. During this flight, how much CO2 was released into the atmosphere? Assume the combustion of the fuel was complete, so all the fuel was burned to form CO2 and H2O. Give both the mass of CO2 produced (in kg and in lbs) and the volume it would occupy at 298 K, 1 atm.(b) How much CO2 would be released into the atmosphere if those passengers and crew made the trip instead, in pairs, in hybrid cars at 40 miles per gallon. Assume the density of the gasoline is 0.75 kg L-1 and that carbon and hydrogen dominate the composition in a ratio of 1:2. The road trip is 1082 miles.
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