1. Balance the following redox equations using the half-reaction method: a. N₂H4 + KBrO3 → N₂ + KBr + H₂O b. KBrO2 + K₂S2O3 + H₂O → KBr + K₂S406 + KOH c. Zn + HNO3 → Zn(NO3)2 + NH4NO3 + H₂O

1. Balance the following redox equations using the half-reaction method: a. N₂H4 + KBrO3 → N₂ + KBr + H₂O b. KBrO2 + K₂S2O3 + H₂O → KBr + K₂S406 + KOH c. Zn + HNO3 → Zn(NO3)2 + NH4NO3 + H₂O

Chemistry

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Chapter18: Electrochemistry

Section: Chapter Questions

Problem 100E: A factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What...

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A factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?
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.
Balance the following skeleton equations. The reactions occur in acidic or basic aqueous solution, as indicated. a MnO4+S2MnO2+S8(basic) b IO3+HSO3I+SO42(acidic) c Fe(OH)2+CrO42Fe(OH)3+Ce(OH)4(basic) d Cl2Cl+ClO(basic)
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?
Order the following oxidizing agents by increasing strength under standard-state conditions: O2(g); MnO4(aq); NO3 (aq) (in acidic solution ).
Using Table 17.1, calculate E° for the reaction between (a) chromium(II) ions and tin(IV) ions to produce chromium(III) ions and tin(II) ions. (b) manganese(II) ions and hydrogen peroxide to produce solid manganese dioxide (MnO2)
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
(a) Write equations for the half-reactions that occur at the cathode and the anode when an aqueous solution of KCl is electrolyzed. Which chemical species is oxidized, and which chemical species is reduced in this reaction? (b) Predict the products formed when an aqueous solution of CsI is electrolyzed.
An electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?
Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms. (a) Al(s)+F2(g) (b) Al(s)+CuBr2(aq) (single displacement) (c) P4(s)+O2(g) (d) Ca(s)+H2O(l) (products are a strong base and a diatomic gas)
Consider the following cell running under standard conditions: Fe(s)Fe2+(aq)Al3+(aq)Al(s) a Is this a voltaic cell? b Which species is being reduced during the chemical reaction? c Which species is the oxidizing agent? d What happens to the concentration of Fe3+(aq) as the reaction proceeds? e How does the mass of Al(s) change as the reaction proceeds?
1. If you wish to convert 0.0100 mol of Au3+ (aq) ions into Au(s) in a “gold-plating” process, how long must you electrolyze a solution if the current passing through the circuit is 2.00 amps? 483 seconds 4.83 104 seconds 965 seconds 1450 seconds

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