EBK WEBASSIGN FOR ZUMDAHL'S CHEMICAL PR
8th Edition
ISBN: 9780357119099
Author: ZUMDAHL
Publisher: VST
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Chapter 11, Problem 77E
A factory wants to produce
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Chapter 11 Solutions
EBK WEBASSIGN FOR ZUMDAHL'S CHEMICAL PR
Ch. 11 - Prob. 1DQCh. 11 - Prob. 2DQCh. 11 - You want to “plate out” nickel metal from a nickel...Ch. 11 - A copper penny can be dissolved in nitric acid but...Ch. 11 - Sketch a cell that forms iron metal from iron(II)...Ch. 11 - Which of the following is the best reducing agent:...Ch. 11 - You are told that metal A is a better reducing...Ch. 11 - Explain the following relationships: G and w, cell...Ch. 11 - Explain why cell potentials are not multiplied by...Ch. 11 - What is the difference between andWhen is equal to...
Ch. 11 - Prob. 11DQCh. 11 - Look up the reduction potential for Fe3+toFe2+ ....Ch. 11 - Prob. 13DQCh. 11 - Is the following statement true or false?...Ch. 11 - What is electrochemistry? What are redox...Ch. 11 - When magnesium metal is added to a beaker of...Ch. 11 - Prob. 17ECh. 11 - How can you construct a galvanic cell from two...Ch. 11 - Prob. 19ECh. 11 - Prob. 20ECh. 11 - Prob. 21ECh. 11 - Consider the following galvanic cells: For each...Ch. 11 - Prob. 23ECh. 11 - Prob. 24ECh. 11 - Answer the following questions using data from...Ch. 11 - Prob. 26ECh. 11 - Using data from Table 11.1, place the following in...Ch. 11 - Prob. 28ECh. 11 - Use the table of standard reduction potentials...Ch. 11 - Use the table of standard reduction potentials...Ch. 11 - Prob. 31ECh. 11 - A patent attorney has asked for your advice...Ch. 11 - The free energy change for a reaction G is an...Ch. 11 - The equation also can be applied to...Ch. 11 - Prob. 35ECh. 11 - Glucose is the major fuel for most living cells....Ch. 11 - Direct methanol fuel cells (DMFCs) have shown...Ch. 11 - The overall reaction and standard cell potential...Ch. 11 - Calculate the maximum amount of work that can...Ch. 11 - Prob. 40ECh. 11 - Prob. 41ECh. 11 - Chlorine dioxide (ClO2) , which is produced by...Ch. 11 - The amount of manganese in steel is determined...Ch. 11 - The overall reaction and equilibrium constant...Ch. 11 - Prob. 45ECh. 11 - Calculate for the reaction...Ch. 11 - A disproportionation reaction involves a substance...Ch. 11 - Calculate for the following half-reaction:...Ch. 11 - For the following half-reaction AlF63+3eAl+6F...Ch. 11 - Prob. 50ECh. 11 - The solubility product for CuI(s) is 1.11012....Ch. 11 - Explain the following statement: determines...Ch. 11 - Calculate the pH of the cathode compartment for...Ch. 11 - Consider the galvanic cell based on the...Ch. 11 - Prob. 55ECh. 11 - Consider the following galvanic cell at 25°C:...Ch. 11 - The black silver sulfide discoloration of...Ch. 11 - Consider the cell described below:...Ch. 11 - Consider the cell described below:...Ch. 11 - Prob. 60ECh. 11 - Prob. 61ECh. 11 - Prob. 62ECh. 11 - What are concentration cells? What is in a...Ch. 11 - A silver concentration cell is set up at 25°C as...Ch. 11 - Consider the concentration cell shown below....Ch. 11 - Prob. 66ECh. 11 - Prob. 67ECh. 11 - An electrochemical cell consists of a nickel metal...Ch. 11 - You have a concentration cell in which the cathode...Ch. 11 - Consider a galvanic cell at standard conditions...Ch. 11 - An electrochemical cell consists of a zinc metal...Ch. 11 - How long will it take to plate out each of the...Ch. 11 - What mass of each of the following substances can...Ch. 11 - It took 2.30 min with a current of 2.00 A to plate...Ch. 11 - The electrolysis of BiO+ produces pure bismuth....Ch. 11 - A single HallHeroult cell (as shown in Fig. 11.22)...Ch. 11 - A factory wants to produce 1.00103 kg barium...Ch. 11 - Why is the electrolysis of molten salts much...Ch. 11 - What reaction will take place at the cathode and...Ch. 11 - What reaction will take place at the cathode and...Ch. 11 - Prob. 81ECh. 11 - a. In the electrolysis of an aqueous solution of...Ch. 11 - A solution at 25°C contains 1.0 M...Ch. 11 - An aqueous solution of an unknown salt of...Ch. 11 - Consider the following half-reactions: A...Ch. 11 - An unknown metal M is electrolyzed. It took 74.1 s...Ch. 11 - Electrolysis of an alkaline earth metal chloride...Ch. 11 - Prob. 88ECh. 11 - What volume of F2 gas, at 25°C and 1.00 atm, is...Ch. 11 - Prob. 90ECh. 11 - In the electrolysis of a sodium chloride solution,...Ch. 11 - What volumes of H2(g)andO2(g) at STP are...Ch. 11 - Copper can be plated onto a spoon by placing the...Ch. 11 - Prob. 94AECh. 11 - Prob. 95AECh. 11 - Prob. 96AECh. 11 - Prob. 97AECh. 11 - Prob. 98AECh. 11 - Prob. 99AECh. 11 - Prob. 100AECh. 11 - Prob. 101AECh. 11 - Prob. 102AECh. 11 - Prob. 103AECh. 11 - Prob. 104AECh. 11 - In 1973 the wreckage of the Civil War ironclad...Ch. 11 - A standard galvanic cell is constructed so that...Ch. 11 - Prob. 107AECh. 11 - Prob. 108AECh. 11 - Prob. 109AECh. 11 - Prob. 110AECh. 11 - Prob. 111AECh. 11 - Prob. 112AECh. 11 - Prob. 113AECh. 11 - Consider a galvanic cell based on the following...Ch. 11 - Prob. 115AECh. 11 - Prob. 116AECh. 11 - Prob. 117AECh. 11 - Prob. 118AECh. 11 - Prob. 119CPCh. 11 - Prob. 120CPCh. 11 - A zinccopper battery is constructed as follows:...Ch. 11 - Prob. 122CPCh. 11 - Prob. 123CPCh. 11 - Prob. 124CPCh. 11 - Prob. 125CPCh. 11 - Prob. 126CPCh. 11 - Prob. 127CPCh. 11 - Prob. 128CPCh. 11 - Prob. 129CPCh. 11 - Prob. 130CPCh. 11 - Prob. 131CPCh. 11 - Prob. 132MPCh. 11 - Prob. 133MP
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- 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?arrow_forwardA 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?arrow_forwardAn 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)?arrow_forward
- An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?arrow_forwardA lead storage battery delivers a current of 6.00 A for one hour and 22 minutes at a voltage of 12.0 V. (a) How many grams of lead are converted to PbSO4? (b) How much electrical energy is produced in kilowatt hours?arrow_forwardAn active (metal) electrode was found to lose mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode part of the anode or cathode? Explain.arrow_forward
- In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?arrow_forwardConsider the electrolysis of NiCl2 to Ni(s) and Cl2(g). (a) What is the minimum voltage required to carry out this reaction at standard conditions? (b) If a voltage of 3.0 V is actually used, and 10.00 kJ of energy are consumed, how many grams of Ni(s) are obtained? (1J=1volt-coulomb)arrow_forwardAtomic masses can be determined by electrolysis. In one hour, a current of 0.600 A deposits 2.42 g of a certain metal, M, which is present in solution as M+ ions. What is the atomic mass of the metal?arrow_forward
- Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If a plant has a continuous capacity of 1.00 million A, what mass of aluminum can be produced in 2.00 h?arrow_forwardAn 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?arrow_forwardThe mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).arrow_forward
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