Write a balanced half-reaction describing the reduction of solid diiodine to aqueous iodide anions.☐ローロX

The steps in balancing half reactions are the following: Step 1: Balance the atoms other than…

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Chemistry In Focus

7th Edition

ISBN:9781337399692

Author:Tro, Nivaldo J.

Publisher:Tro, Nivaldo J.

Chapter14: Oxidation And Reduction

Section: Chapter Questions

Problem 8E: Why is bromine reduced in the following reaction (i.e., in what sense is bromine gaining electrons)?...

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Similar questions

(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.
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.
Briefly explain why different products are obtained from the electrolysis of molten NaCl and the electrolysis of a dilute aqueous solution of NaCl.
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?
Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode reaction is 2Cl(aq)Cl2(g)+2e How long will it take to produce 2.00 kg of chlorine if the current is 5.00 102 A?
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
Hydrazine, N2H4, has been proposed as the fuel in a fuel cell in which oxygen is the oxidizing agent. The reactions are N2H4(aq) + 4 OH(aq) N2(g) + 4 H2O() + 4e O2(g) + 2 H2O() + 4e 4 OH(aq) (a) Which reaction occurs at the anode and which at thecathode? (b) What is the overall cell reaction? (c) If the cell is to produce 0.50 A of current for 50.0 h, calculate what mass in grams of hydrazine must be present. (d) Calculate what mass (g) of O2 must be available to reactwith the mass of N2H4 determined in part (c).
Calcium metal can be obtained by the direct electrolysis of molten CaCl2, at a voltage of 3.2 V. (a) How many joules of electrical energy are required to obtain 12.0 1b of calcium? (b) What is the cost of the electrical energy obtained in (a) if electrical energy is sold at the rate of nine cents per kilowatt hour?
Why is bromine reduced in the following reaction (i.e., in what sense is bromine gaining electrons)? H2+Br22HBr
In an analytical determination of arsenic, a solution containing arsenious acid, H3AsO3, potassium iodide, and a small amount of starch is electrolyzed. The electrolysis produces free iodine from iodide ion, and the iodine immediately oxidizes the arsenious acid to hydrogen arsenate ion, HAsO42. I2(aq)+H3AsO3(aq)+H2O(l)2I(aq)+HAsO42(aq)+4H+(aq) When the oxidation of arsenic is complete, the free iodine combines with the starch to give a deep blue color. If, during a particular run, it takes 65.4 s for a current of 10.5 mA to give an endpoint (indicated by the blue color), how many grams of arsenic are present in the solution?
Write a balanced half-reaction for the reduction of nitrate ion NO−3 to gaseous nitric oxide NO in acidic aqueous solution. Be sure to add physical state symbols where appropriate.
Why is it impossible to isolate sodium by electrolysis of aqueous solutions of sodium salts?

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Write a balanced half-reaction describing the reduction of solid diiodine to aqueous iodide anions. ☐ ローロ X