You have the following; reagents solvents, substances and equipment; Water, ice, Phenylethylbromide, iodomethane, magnesium, HBr, HCI, HI, oxygen, silver, dimethylamine, K₂Cr₂O, H₂SO4, hydrogen cyanide, benzylchloride, NaOH, NaH and heating source in your laboratory Utilize whatever needed of the above shown materials to carry out the synthesis of the following organic compound from formaldehyde, using schematic chemical reactions only. CH3 -CH₂ CH₂
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- Certain amount of pure charcoal (carbon) has to be burnt with supplied natural air. Process engineer allowed exact amount of air required to burn the entire charcoal completely to carbon dioxide. Carbon has no reaction with nitrogen gas present in the air. In the reaction outlet if 5 kg of nitrogen gas was found, calculate the amount of charcoal used. (12C, 16O, 14N)During bad storage of cement the alkalis in the cement react with CO2 to form alkali carbonates, which they react with Ca(OH)2 liberated by the hydrolysis of to form C3S, CaCO3 Calcium Carbonate, C3S Dicalcium silicate, CaCO3 Tricalcium silicate, Calcium CarbonateCertain amount of pure charcoal (carbon) has to be burnt with supplied natural air. Process engineer allowed exact amount of air required to burn the entire charcoal completely to carbon dioxide. Carbon has no reaction with nitrogen gas present in the air. In the reaction outlet if 15 kg of carbon dioxide gas was found, calculate the amount of air used in the reactor. (12C, 16O, 14N)
- Fine particles of metallic iron can be injected underground to remediate pollution of underground aquifers by the industrial solvent trichloroethane. In one experiment, 2400L of an aqueous emulsion containing ~480 kg of Fe(0) consumed 17.0 kg of trichloroethane in 5 months. Write a balanced reaction using H2O and H+ to complete the balancing. What percentage of injected iron was used by this reaction in 5 months? Fe + C2HCl3 ---> Fe2+ + C2H4 + Cl-Pearls are built from calcite and aragonite, essentially two forms of calcium carbonateCaCO3. They disintegrate in vinegar, which contains acetic acid. Formulate the netionic equation for this process.Q2/ Clorine is produced by burning hydrogen cloride gas using air. The reaction taking place in the burner is : 4 HCI (g) + 02 (g) → 2 Cl, (g) + 2 H;0 (g) Air is used in 35% excess of that theoretically/(stoichiometrically) required. Assuming oxidation to be 80% complete and the dry air and hydrogen chloride gas enter the burner at 298 K (25°C), calculate the adiabatic reaction temperature of the product gas stream. Data : Component AH , kJ/rmol H,O (g) HCI (g) - 241.82 -92.31 Heat capacity data : Cp = a + bT + cT2 + dT³, kJ/(kmol-K) Component bx 103 сх106 dx 10° a HCI 30.3088 - 7.609 13.2608 - 4.3336 O2 26.0257 11.7551 - 2.3426 - 0.5623 Cl, 28.5463 23.8795 - 21.3631 6.4726 - 4.5474 - 4.968 H,O 32.4921 0.0796 13.2107 N2 29.5909 -5.141 13.1829
- Write the balanced NET ionic equation for the reaction when aqueous KBr and aqueous AGC2H3O2 are mixed in solution to form aqueous KC:H3O2 and solid AgBr.1. Calcium in a sample solution is determined by atomic absorption spectroscopy (AAS). A stock solution of calcium is prepared by dissolving 1.834 g CaCl, 2H,0 in water and diluting to 1 litre. From this stock solution, the second stock solution is prepared by the dilution factor of 10. Three standard solutions of calcium are prepared from the second stock solution with the following dilution factor: 20 (first standard solution), 10 (second standard solution) and 5 (third standard solution). A blank solution is prepared as well. Absorbance signals of AAS are as follows: 1.5 (blank solution), 10.6 (first standard solution), 20.1 (second standard solution), 38.5 (third standard solution), 29.6 (sample solution). (Molar mass; Ca = 40.00 g mol-, CI = 35.45 g mol-, 0 = 16.00 g mol-', H = 1.00 g mol-1) a. Construct ONE (1) plot that could be used to represent the calibration curve. b. From the plot of Q1a, determine the amount of calcium in parts per million.b) Determine the standard enthalpy change and std. Gibbs free energy change of D reaction at 400 k for the reaction CO(g) +2H2(g) → CH;OH (g) At 298.15 K, AH CO (9)= -26.41 kcal/mol, AH.CH,0H(9)= -48.08 kcal/mol, (9)= -32.8079 kcal/mol, AG CH30H(g)= -38.69 kcal/mol, The standard heat capacity of various components is given by, C = a + bT + cT2 + dT³, where C is in cal/mol-K and T is in K b x10² c x105 d x10º Сomponent CH3OH a 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079
- A 0.879 g sample of a CaCl2·2H2O/K2C2O4·H2O solid salt mixture is dissolved in ~100mL of deionized water. The precipitate, after having been filtered and air-dried, has a mass of 0.284 g. The limiting reactant in the salt mixture was later determined to beCaCl2 ·2H2O. a.Write the ionic equation for the reaction. b.Write the net ionic equation for the reaction. c.How many moles and grams of CaCl2 ·2H2O reacted in the reaction mixture? d.How many moles and grams of the excess reactant, K 2C2O 4H2O, reacted in the mixture? e.How many grams of the K2C2O4·H2O in the salt mixture remain unreacted (inexcess)? f.What is the percent by mass of each salt in the mixtureA magnesium bar with a mass of 6.0 kg is attached to a buried iron pipe to serve as a sacrificial anode. An averagecurrent of 0.020 A flows between the bar and the pipe.(a) Which reactions take place at the surface of the magnesium bar and the surface of the iron pipe? (b) How many years would it take for the entire magnesium bar to be consumed?To remove the tarnish (Ag2S) on a silver spoon the following steps are carried out. the spoon is placed in a large pan filled with water so the spoon was totally immersed. A few tablespoonfuls of baking soda (sodium bicarbonate), which readily dissolves. Is added. Some aluminum foil is placed at the bottom of the pan in contact with the spoon and then heated the solution to about 80° After a few minutes, the spoon is removed and rinsed with cold water. The tarnish is gone and the spoon regains its original shiny appearance. Describe with equations the electrochemical basis for the procedure. Adding NaCl instead of NaHCO3 would also work because both compounds arestrong electrolytes. What is the added advantage of using NaHCO3? (Hint: Consider the pH of the solution.) What is the purpose of heating the solution? Some commercial tarnish removers containing a fluid (or paste) that is a dilute HCl solution. Rubbing the spoon with the fluid will also remove the tarnish. Name two…