Write a balanced half-reaction for the reduction of gaseous nitrogen N2 to aqueous hydrazine N2H4 in basic aqueous solution. Be sure to add physical state symbols where appropriate. Show work
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- (a) Determine the mass of Na,S2O3.5H20 required to prepare 0.1N solution in 50 ml volume. (b) Compare combustion of Anthracene and Xylene in sufficient supply of air. Which one will produce more carbon rich sooty flame and why? (c) Consider electrode potential data given in Question 4 (c). Predict which two electrodes combination will give maximum potential. Provide justification. (d) Explain two industrial applications of acidic buffer solutions. (e) Discuss the importance of Hess law with suitable example.Magnesium, the element, is produced commercially byelectrolysis from a molten salt (the “electrolyte”) using acell similar to the one shown here. (a) What is the mostcommon oxidation number for Mg when it is part of a salt?(b) Chlorine gas is evolved as voltage is applied in the cell.Knowing this, identify the electrolyte. (c) Recall that in anelectrolytic cell the anode is given the + sign and the cathodeis given the – sign, which is the opposite of what we seein batteries. What half-reaction occurs at the anode in thiselectrolytic cell? (d) What half-reaction occurs at the cathode?(a) Predict the products of electrolysis in each of the following:(i) An aqueous solution of AgNO3 with platinum electrode.(it) An aqueous solution of H2S04 using platinum electrode.(b) Estimate the minimum potential differences needed to reduce Al203 at 500°C. The gibbs free energy change for the decomposition reaction2/3 Al2O3——>4/3 Al+O2
- Calculate the amounts of Cu and Br: produced at the inert elecuvues by passing a current of 4.5 A through a solution of CuBr, for 1.0 hr.Metallic magnesium can be made by the electrolysis ofmolten MgCl2. (a) What mass of Mg is formed by passinga current of 4.55 A through molten MgCl2, for 4.50 days?(b) How many minutes are needed to plate out 25.00 g Mgfrom molten MgCl2 using 3.50 A of current?Write a balanced half-reaction for the reduction of aqueous hydrogen peroxide H2O2 to liquid water H2O in basic aqueous solution. Be sure to add physical state symbols where appropriate.
- (a) What is an electrolytic cell? (b) The negative terminal ofa voltage source is connected to an electrode of an electrolyticcell. Is the electrode the anode or the cathode of thecell? Explain. (c) The electrolysis of water is often done witha small amount of sulfuric acid added to the water. What isthe role of the sulfuric acid? (d) Why are active metals suchas Al obtained by electrolysis using molten salts rather thanaqueous solutions?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 13.1829A 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?
- Write the balanced half-reaction corresponding to the oxidation involved in the air oxidation of Fe2+(aq) to Fe2O3⋅3H2O .=Give balanced equations for the overall reaction in the electrolysis of molten lithium chloride and for the reactions occurring at the electrodes. You may wish to review the chapter on electrochemistry for relevant examples.(a) Assuming standard conditions, arrange the followingin order of increasing strength as oxidizing agents in acidicsolution: Cr2O72-, H2O2, Cu2+, Cl2, O2. (b) Arrange the followingin order of increasing strength as reducing agents inacidic solution: Zn, I-, Sn2+, H2O2, Al.