he following reaction occurs in basic solution. Balance it by adding only OH or H20. (enter your answer as the sum of the coefficients) 2H4(aq) + Cu(OH)2(s) – N2(g)+Cu(s) Submit Answer Incorrect. Tries 1/99 Previous Tries

he following reaction occurs in basic solution. Balance it by adding only OH or H20. (enter your answer as the sum of the coefficients) 2H4(aq) + Cu(OH)2(s) – N2(g)+Cu(s) Submit Answer Incorrect. Tries 1/99 Previous Tries

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter3: Chemical Reactions

Section3.9: Classifying Reactions In Aqueous Solution

Problem 1RC: 1. Sometimes a reaction can fall in more than one category. Into what category (or categories) does...

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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?
1. Sometimes a reaction can fall in more than one category. Into what category (or categories) does the reaction of Ba(OH)2(aq) + H+PO4(aq) fit? acid-base and oxidation-reduction oxidation-reduction acid-base and precipitation precipitation
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.
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.
Balance the following equations. (Use the lowest possible whole-number coefficients. These may be zero.) (a) Fe(CN) 6³ (aq) + N₂H5+(aq) ⇒ Fe(CN) 6+ (aq) + N₂(g) Fe(CN)6³- + (b) Clo (aq) + I₂(s) ⇒ Cl(aq) + 103 (aq) clo Cro₂²- + N₂H5+ + I₂ + Tl₂O3 + (c) Cro4² (aq) + C₂04² (aq) = Cr(OH)3(s) + CO₂(g) C₂04²- + H+ (d) Tl₂O3(s) + NH₂OH(aq) TIOH(s) + N₂(g) NH₂OH + H+ + OH + H₂O= OH + H₂O = H₂O= H₂O= Fe(CN) 64- 103 + Cr(OH)3 + TIOH(s) + N₂ CO₂ + N₂ + H+ + H₂O OH + OH + H₂O H₂O H₂O
What is the sum of all the coefficients when this equation is balanced with the smallest whole number coefficients. Al(s)+FeO(s)->Fe(s)+Al2O3(s)
Balance the following equations. (Use the smallest whole numbers possible. Enter 1 where appropriate - do not leave any answer box blank.) Ticla() + H20() - TiO2(s) HCI(ag) (b) B2S3(s) + H20() - | H3BO3(aq) +O HyS(g) (c) Fe(OH)3(s) + H2504(aq) - Fez(SO4)3(aq) + H20()
Balance the following equations. (Use the lowest possible whole-number coefficients. These may be zero.) (a) Fe(CN)6³(aq) + N₂H5+ (aq) Fe(CN) 6+ (aq) + N₂(g) 4 +0 5 0 (b) Clo (aq) + I₂(s) ⇒ Cl(aq) + 10₂ (aq) Fe(CN)6³ +7 H₂O 2 CIO +1 H₂O OH + (c) Cro4² (aq) + C₂042 (aq) = Cr(OH)3(s) + CO₂(g) CrO4² +1 OH +0 XN₂H5 +0 X Tl₂O3 + H₂O X H₂O 1₂ +0 (d) Tl₂O3(s) + NH₂OH(aq) = TIOH(s) + N₂(g) XC₂04² +0 X NH₂OH + H+ + 0 H+ +1 OH +8 X OH + H₂O 4 H₂O=5 H₂O = 2 | H2O= Fe(CN) 64 + 7 CI + 2 Cr(OH)3 + 2 X TIOH(s) + XN₂ + 35 103 +2 * H* XN₂ + H+ + X CO₂ + 10 X
One way to determine the hardness of a water sample is to precipitate the calcium out of solution as a carbonate. The net ionic reaction for this precipitation is: Ca2+(aq) + CO32-(aq) → CaCO3 (s) A 1.00 L sample of water is drawn from a Phoenix, AZ well and 0.534 g of calcium carbonate is recovered using the above reaction. What was the Ca2+ concentration of the original water sample in ppm? Show your work and include units. Hint: ppm stands for parts per million, and in the case of an aqueous solution, this is equivalent to mg/L.
Gold(III)hydroxide is used for electroplating gold onto other metals. It can be made by the following reaction (note the equation is unbalanced) KAuCl4(aq) + Na2CO3(aq) + 3H2O(l) → Au(OH)3(aq) + NaCl(aq) + KCl(aq) + CO2(g) To prepare a fresh supply of Au(OH)3, a chemist at an electroplating plant has mixed 20.00g of KAuCl4 with 25.00g of Na2CO3 (both dissolved in excess water) a. How many grams of Na2CO3 will b required to react with KAuCl4? (only 3 decimal places) ________g of Na2CO3 b. what is the maximum number of grams of Au(OH)3 than can be formed? (only 2 decimal places) ________ g of Au(OH)3