The Activity Series of Metals used in this class represents only a portion of metals commonly used in research and design. Below are the results of a few chemical reactions trying to establish information about Cadmium, Copper, Mercury, and Beryllium. Reaction 1: Be(s) + Hg(NO3)2(aq) Hg(l) + Be(NO3)2(laq) -> Reaction 2: Hg(1) + CUNO3(aq) -> No Reaction Reaction 3: Cd(s) + Be(NO3)2(aq) -> No Reaction Reaction 4: Cd(s) + 2CUNO3(aq) -> 2Cu(s) + Cd(NO3)2(aq) Which is the proper order of these metals in terms of increasing ease of oxidation? Be

The Activity Series of Metals used in this class represents only a portion of metals commonly used in research and design. Below are the results of a few chemical reactions trying to establish information about Cadmium, Copper, Mercury, and Beryllium. Reaction 1: Be(s) + Hg(NO3)2(aq) Hg(l) + Be(NO3)2(laq) -> Reaction 2: Hg(1) + CUNO3(aq) -> No Reaction Reaction 3: Cd(s) + Be(NO3)2(aq) -> No Reaction Reaction 4: Cd(s) + 2CUNO3(aq) -> 2Cu(s) + Cd(NO3)2(aq) Which is the proper order of these metals in terms of increasing ease of oxidation? Be

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 108QRT

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Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
Write balanced net ionic equations for the following reactions in acid solution. (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. Nitrogen gas and bromide ions are formed. (b) Solid phosphorus (P4) reacts with an aqueous solution of nitrate to form nitrogen oxide gas and dihydrogen phosphate (H2PO4-) ions. (c) Aqueous solutions of potassium sulfite and potassium permanganate react. Sulfate and manganese(II) ions are formed.
One of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce1,4-dicyanobutane. The reduction reaction is 2CH2CHCH+2H++2eNC(CH2)4CN The NC(CH2)4CN is then chemically reduced using hydrogen gas to H2N(CH2)6NH2, which is used in the production of nylon. What current must be used to produce 150.kg NC(CH2)4CN per hour?
One of the ways to remove nitrogen monoxide gas, a serious source of air pollution, from smokestack emissions is by reaction with ammonia gas, NH3. The products of the reaction, N2 and H2O, are not toxic. Write the balanced equation for this reaction. Assign an oxidation number to each element in the reactants and products, and indicate which element is oxidized and which is reduced.
Chlorine gas was first prepared in 1774 by C. W. Scheele by oxidizing sodium chloride with manganese(IV) oxide. The reaction is NaCl(aq)+H2SO4(aq)+MnO2(s)Na2SO4(aq)+MnCl2(aq)+H2O(l)+Cl2(g) Balance this equation.
4.22 Generally, an excess of O2 is needed for the reaction Sn+O2SnO2 . What is the minimum number of moles of oxygen required to oxidize 7.3 moles of tin?
The Ostwald process for the commercial production of nitric acid involves the Following three steps: 4NH3(g)+5O2(g)4NO(g)+6H2O(s)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) a. Which reaction in the Ostwald process are oxidation-reduction reactions? b. Identify each oxidizing agent and reducing agent.
The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
Hydrazine 1N2H42 and dinitrogen tetroxide 1N2O42 form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N2 and H2O. Which substance serves as the reducing agent and which as the oxidizing agent?
Iron corrodes to produce rust, Fe2O3, but other corrosion products that can form are Fe(O)(OH), iron oxyhydroxide, and magnetite, Fe3O4.It turns out that there are two different kinds of Fe in magnetite that have different oxidation numbers. Suggest what these oxidation numbers are and what their relative stoichiometry must be, assuming oxygen’s oxidation number is -2.
Electric generating plants transport large amounts of hot water through metal pipes, and oxygen dissolved in the water can cause a major corrosion problem. Hydrazine (N2H4) added to the water avoids the problem by reacting with the oxygen: N2H4(aq) + O2(g) --> N2(g) + 2 H2O(l) About 4 × 107 kg of hydrazine is produced every year by reacting ammonia with sodium hypochlorite in the Raschig process: 2 NH3(aq) + NaOCl(aq) --> N2H4(aq) + NaCl(aq) + H2O(l) ΔrH° = −151 kJ (a) If ΔfH° of NaOCl(aq) = −346 kJ/mol, find ΔfH° of N2H4(aq) given that ΔfH° [NH3(aq)] = −80.83 kJ/mol, ΔfH° [NaOCl(aq)] = −346 kJ/mol, ΔfH° [Na+(aq)] = −239.66 kJ/mol, ΔfH° [Cl−(aq)] = −167.46 kJ/mol and ΔfH° [H2O(l)]= −285.840 kJ/mol. What is the heat released when aqueous N2H4 is added to 7.00 × 103 L of plant water that is 2.50 ×10−4 mol/L O2? Enter your answer in scientific notation. (Thanks in advance :))
The proper assignment of oxidation numbers to the elements in the polyatomic ion SO32- would be what?