CHEMISTRY (LOOSELEAF) >CUSTOM<
13th Edition
ISBN: 9781264348992
Author: Chang
Publisher: MCGRAW-HILL HIGHER EDUCATION
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Chapter 18, Problem 18.19QP
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Chapter 18 Solutions
CHEMISTRY (LOOSELEAF) >CUSTOM<
Ch. 18.1 - Balance the following equation for the reaction in...Ch. 18.1 - Determine the number of electrons transferred in...Ch. 18.1 - For the following reaction in acidic solution,...Ch. 18.2 - Write the cell diagram for the following redox...Ch. 18.2 - Write the balanced redox reaction corresponding to...Ch. 18.3 - Can Sn reduce Zn2+(aq) under standard-state...Ch. 18.3 - What is the standard emf of a galvanic cell made...Ch. 18.3 - Prob. 1RCFCh. 18.3 - Prob. 2RCFCh. 18.4 - Prob. 4PE
Ch. 18.4 - Prob. 5PECh. 18.4 - Calculate the equilibrium constant for the...Ch. 18.4 - Prob. 2RCFCh. 18.4 - Prob. 3RCFCh. 18.5 - Prob. 6PECh. 18.5 - Prob. 7PECh. 18.5 - Consider the following cell diagram:...Ch. 18.5 - Calculate the cell voltage at 25C of a...Ch. 18.6 - How many Leclanch cells are contained in a 9-volt...Ch. 18.7 - Prob. 1RCFCh. 18.8 - An aqueous solution of Mg(NO3)2 is electrolyzed....Ch. 18.8 - A constant current is passed through an...Ch. 18.8 - What is the minimum voltage needed for the...Ch. 18.8 - Prob. 2RCFCh. 18.8 - In the electrolysis of molten CaCl2, a current of...Ch. 18 - Balance the following redox equations by the...Ch. 18 - Balance the following redox equations by the...Ch. 18 - Define the following terms: anode, cathode, cell...Ch. 18 - Describe the basic features of a galvanic cell....Ch. 18 - What is the function of a salt bridge? What kind...Ch. 18 - What is a cell diagram? Write the cell diagram for...Ch. 18 - What is the difference between the half-reactions...Ch. 18 - Prob. 18.8QPCh. 18 - Use the information in Table 2.1, and calculate...Ch. 18 - Discuss the spontaneity of an electrochemical...Ch. 18 - Calculate the standard emf of a cell that uses the...Ch. 18 - Calculate the standard emf of a cell that uses...Ch. 18 - Predict whether Fe3+ can oxidize I to I2 under...Ch. 18 - Which of the following reagents can oxidize H2O to...Ch. 18 - Consider the following half-reactions:...Ch. 18 - Predict whether the following reactions would...Ch. 18 - Which species in each pair is a better oxidizing...Ch. 18 - Which species in each pair is a better reducing...Ch. 18 - Consider the electrochemical reaction Sn2+ + X Sn...Ch. 18 - The Ecell for the following cell is 1.54 V at 25C:...Ch. 18 - Write the equations relating G and K to the...Ch. 18 - Prob. 18.22QPCh. 18 - Prob. 18.23QPCh. 18 - The equilibrium constant for the reaction...Ch. 18 - Use the standard reduction potentials to find the...Ch. 18 - Calculate G and Kc for the following reactions at...Ch. 18 - Under standard-state conditions, what spontaneous...Ch. 18 - Given that E = 0.52 V for the reduction...Ch. 18 - Prob. 18.29QPCh. 18 - Write the Nernst equation for the following...Ch. 18 - What is the potential of a cell made up of Zn/Zn2+...Ch. 18 - Calculate E, E, and G for the following cell...Ch. 18 - Calculate the standard potential of the cell...Ch. 18 - Referring to the arrangement in Figure 18.1,...Ch. 18 - Calculate the emf of the following concentration...Ch. 18 - Explain the differences between a primary galvanic...Ch. 18 - Discuss the advantages and disadvantages of fuel...Ch. 18 - The hydrogen-oxygen fuel cell is described in...Ch. 18 - Calculate the standard emf of the propane fuel...Ch. 18 - Prob. 18.41QPCh. 18 - Galvanized iron is steel sheet that has been...Ch. 18 - Tarnished silver contains Ag2S. The tarnish can be...Ch. 18 - Prob. 18.44QPCh. 18 - What is the difference between a galvanic cell...Ch. 18 - Describe the electrolysis of an aqueous solution...Ch. 18 - The half-reaction at an electrode is...Ch. 18 - Consider the electrolysis of molten barium...Ch. 18 - Prob. 18.49QPCh. 18 - If the cost of electricity to produce magnesium by...Ch. 18 - One of the half-reactions for the electrolysis of...Ch. 18 - How many moles of electrons are required to...Ch. 18 - Calculate the amounts of Cu and Br2 produced in...Ch. 18 - In the electrolysis of an aqueous AgNO3 solution,...Ch. 18 - A steady current was passed through molten CoSO4...Ch. 18 - A constant electric current flows for 3.75 h...Ch. 18 - What is the hourly production rate of chlorine gas...Ch. 18 - Chromium plating is applied by electrolysis to...Ch. 18 - The passage of a current of 0.750 A for 25.0 min...Ch. 18 - A quantity of 0.300 g of copper was deposited from...Ch. 18 - In a certain electrolysis experiment, 1.44 g of Ag...Ch. 18 - One of the half-reactions for the electrolysis of...Ch. 18 - A steady current of 10.0 A is passed through three...Ch. 18 - Industrially, copper metal can be purified...Ch. 18 - A Daniell cell consists of a zinc electrode in...Ch. 18 - A concentration cell is constructed having Cu...Ch. 18 - For each of the following redox reactions, (i)...Ch. 18 - The oxidation of 25.0 mL of a solution containing...Ch. 18 - The SO2 present in air is mainly responsible for...Ch. 18 - Prob. 18.70QPCh. 18 - Prob. 18.71QPCh. 18 - Oxalic acid (H2C2O4) is present in many plants and...Ch. 18 - Prob. 18.73QPCh. 18 - Prob. 18.74QPCh. 18 - From the following information, calculate the...Ch. 18 - Consider a galvanic cell composed of the SHE and a...Ch. 18 - A galvanic cell consists of a silver electrode in...Ch. 18 - Prob. 18.78QPCh. 18 - Calculate the emf of the following concentration...Ch. 18 - Prob. 18.80QPCh. 18 - Suppose you are asked to verify experimentally the...Ch. 18 - Prob. 18.82QPCh. 18 - An aqueous KI solution to which a few drops of...Ch. 18 - A piece of magnesium metal weighing 1.56 g is...Ch. 18 - Prob. 18.85QPCh. 18 - An acidified solution was electrolyzed using...Ch. 18 - In a certain electrolysis experiment involving...Ch. 18 - Consider the oxidation of ammonia:...Ch. 18 - When an aqueous solution containing gold(III) salt...Ch. 18 - In an electrolysis experiment, a student passes...Ch. 18 - People living in cold-climate countries where...Ch. 18 - Given that...Ch. 18 - A galvanic cell with Ecell = 0.30 V can be...Ch. 18 - Shown here is a galvanic cell connected to an...Ch. 18 - Fluorine (F2) is obtained by the electrolysis of...Ch. 18 - A 300-mL solution of NaCl was electrolyzed for...Ch. 18 - Industrially, copper is purified by electrolysis....Ch. 18 - An aqueous solution of a platinum salt is...Ch. 18 - Consider a galvanic cell consisting of a magnesium...Ch. 18 - A current of 6.00 A passes through an electrolytic...Ch. 18 - Prob. 18.101QPCh. 18 - Explain why most useful galvanic cells give...Ch. 18 - The table here shows the standard reduction...Ch. 18 - Consider a concentration cell made of the...Ch. 18 - A silver rod and a SHE are dipped into a saturated...Ch. 18 - Zinc is an amphoteric metal; that is, it reacts...Ch. 18 - Use the data in Table 18.1 to determine whether or...Ch. 18 - The magnitudes (but not the signs) of the standard...Ch. 18 - A galvanic cell is constructed as follows. One...Ch. 18 - Given the standard reduction potential for Au3+ in...Ch. 18 - Prob. 18.111QPCh. 18 - When 25.0 mL of a solution containing both Fe2+...Ch. 18 - Consider the Daniell cell in Figure 18.1. When...Ch. 18 - Use the data in Table 18.1 to show that the...Ch. 18 - Consider two electrolytic cells A and B. Cell A...Ch. 18 - A galvanic cell consists of a Mg electrode in a 1...Ch. 18 - The concentration of sulfuric acid in the...Ch. 18 - Consider a Daniell cell operating under...Ch. 18 - An electrolysis cell was constructed similar to...Ch. 18 - Prob. 18.120QPCh. 18 - Prob. 18.121QPCh. 18 - Prob. 18.122QPCh. 18 - A piece of magnesium ribbon and a copper wire are...Ch. 18 - The zinc-air battery shows much promise for...Ch. 18 - Calculate E for the reactions of mercury with (a)...Ch. 18 - Because all alkali metals react with water, it is...Ch. 18 - A galvanic cell using Mg/Mg2+ and Cu/Cu2+...Ch. 18 - Given the following standard reduction potentials,...Ch. 18 - Compare the pros and cons of a fuel cell, such as...Ch. 18 - Lead storage batteries are rated by ampere hours,...Ch. 18 - Use Equations (17.10) and (18.3) to calculate the...Ch. 18 - A construction company is installing an iron...Ch. 18 - A 9.00 102-mL 0.200 M MgI2 was electrolyzed. As a...Ch. 18 - Based on the following standard reduction...Ch. 18 - Calculate the equilibrium constant for the...Ch. 18 - The nitrite ion (NO2) in soil is oxidized to...Ch. 18 - The diagram here shows an electrolytic cell...Ch. 18 - Fluorine is a highly reactive gas that attacks...Ch. 18 - Show a sketch of a galvanic concentration cell....Ch. 18 - The emf of galvanic cells varies with temperature...Ch. 18 - A concentration cell ceases to operate when the...Ch. 18 - It has been suggested that a car can be powered...Ch. 18 - Estimate how long it would take to electroplate a...Ch. 18 - The potential for a cell based on the standard...
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- For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)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_forwardFor the reaction Cu2+(aq) + Zn(s) → Cu(s) + Zn2+ (aq), why can’t you generate electric current by placing a piece of copper metal and a piece of zinc metal in a solution containing CuCl2(aq) and ZnCl2(aq)?arrow_forward
- Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?arrow_forwardAn 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 standard galvanic cell is constructed so that the overall cell reaction is 2A13++(aq)+3M(s)3M2+(aq)+2A1(s) Where M is an unknown metal. If G = 411 kJ for the overall cell reaction, identify the metal used to construct the standard cell.arrow_forward
- At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.arrow_forwardUse the data from the table of standard reduction potentials in Appendix H to calculate the standard potential of the cell based on each of the following reactions. In each case, state whether the reaction proceeds spontaneously as written or spontaneously in the reverse direction under standard-state conditions. (a) H2(g)+Cl2(g)2H+(aq)+2Cl(aq) (b) Al3+(aq)+3Cr2+(aq)Al(s)+3Cr3+(aq) (c) Fe2+(aq)+Ag+(aq)Fe3+(aq)+Ag(s)arrow_forwardGive the notation for a voltaic cell whose overall cell reaction is Mg(s)+2Ag+(aq)Mg2+(aq)+2Ag(s) What are the half-cell reactions? Label them as anode or cathode reactions. What is the standard cell potential of this cell?arrow_forward
- The 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_forwardAt 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.arrow_forwardYou have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.arrow_forward
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