Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 19, Problem 69GQ
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Chapter 19 Solutions
Chemistry & Chemical Reactivity
Ch. 19.1 - Prob. 2CYUCh. 19.1 - Prob. 3CYUCh. 19.1 - 1. Copper(II) sulfide reacts with nitric acid...Ch. 19.1 - Prob. 2RCCh. 19.1 - The balanced half-reaction for Br2 BrO3 in basic...Ch. 19.2 - Describe how to set up a voltaic cell using the...Ch. 19.2 - The following overall chemical reaction occurs in...Ch. 19.2 - Prob. 1RCCh. 19.2 - Prob. 2RCCh. 19.2 - Prob. 3RC
Ch. 19.3 - Prob. 1RCCh. 19.3 - Prob. 2RCCh. 19.4 - (a) Rank the following metals in their ability to...Ch. 19.4 - Prob. 1RCCh. 19.4 - Prob. 2RCCh. 19.4 - Prob. 3RCCh. 19.4 - Prob. 1QCh. 19.4 - Prob. 2QCh. 19.4 - Prob. 3QCh. 19.5 - A voltaic cell is set up with an aluminum...Ch. 19.5 - Check Your Understanding
The half-cells Fe2+(aq,...Ch. 19.5 - Prob. 1RCCh. 19.6 - Prob. 1CYUCh. 19.6 - Calculate the equilibrium constant at 25 C for the...Ch. 19.6 - Prob. 1RCCh. 19.7 - Predict the chemical reactions that will occur at...Ch. 19.7 - Prob. 1RCCh. 19.8 - Prob. 1CYUCh. 19.8 - 1. If you wish to convert 0.0100 mol of Au3+ (aq)...Ch. 19.8 - Prob. 1QCh. 19.8 - Use standard reduction potentials to determine...Ch. 19.8 - Prob. 3QCh. 19.8 - The overall reaction for the production of Cu(OH)2...Ch. 19.8 - Assume the following electrochemical cell...Ch. 19 - Write balanced equations for the following...Ch. 19 - Write balanced equations for the following...Ch. 19 - Balance the following redox equations. All occur...Ch. 19 - Balance the following redox equations. All occur...Ch. 19 - Balance the following redox equations. All occur...Ch. 19 - Prob. 6PSCh. 19 - A voltaic cell is constructed using the reaction...Ch. 19 - A voltaic cell is constructed using the reaction...Ch. 19 - The half-cells Fe2+(aq) | Fe(s) and O2(g) | H2O...Ch. 19 - The half cells Sn2+(aq) |Sn(s) and Cl2(g) |Cl(aq)...Ch. 19 - For each of the following electrochemical cells,...Ch. 19 - For each of the following electrochemical cells,...Ch. 19 - Use cell notation to depict an electrochemical...Ch. 19 - Use cell notation to depict an electrochemical...Ch. 19 - What are the similarities and differences between...Ch. 19 - What reactions occur when a lead storage battery...Ch. 19 - Calculate the value of E for each of the following...Ch. 19 - Calculate the value of E for each of the following...Ch. 19 - Balance each of the following unbalanced...Ch. 19 - Balance each of the following unbalanced...Ch. 19 - Consider the following half-reactions: (a) Based...Ch. 19 - Prob. 22PSCh. 19 - Which of the following elements is the best...Ch. 19 - Prob. 24PSCh. 19 - Which of the following ions is most easily...Ch. 19 - From the following list, identify the ions that...Ch. 19 - (a) Which halogen is most easily reduced in acidic...Ch. 19 - Prob. 28PSCh. 19 - Calculate the potential delivered by a voltaic...Ch. 19 - Calculate the potential developed by a voltaic...Ch. 19 - One half-cell in a voltaic cell is constructed...Ch. 19 - One half-cell in a voltaic cell is constructed...Ch. 19 - One half-cell in a voltaic cell is constructed...Ch. 19 - One half-cell in a voltaic cell is constructed...Ch. 19 - Calculate rG and the equilibrium constant for the...Ch. 19 - Prob. 36PSCh. 19 - Use standard reduction potentials (Appendix M) for...Ch. 19 - Use the standard reduction potentials (Appendix M)...Ch. 19 - Use the standard reduction potentials (Appendix M)...Ch. 19 - Use the standard reduction potentials (Appendix M)...Ch. 19 - Prob. 41PSCh. 19 - Prob. 42PSCh. 19 - Which product, O2 or F2, is more likely to form at...Ch. 19 - Which product, Ca or H2, is more likely to form at...Ch. 19 - An aqueous solution of KBr is placed in a beaker...Ch. 19 - An aqueous solution of Na2S is placed in a beaker...Ch. 19 - In the electrolysis of a solution containing...Ch. 19 - In the electrolysis of a solution containing...Ch. 19 - Electrolysis of a solution of CuSO4(aq) to give...Ch. 19 - Electrolysis of a solution of Zn(NO3)2(aq) to give...Ch. 19 - A voltaic cell can be built using the reaction...Ch. 19 - Assume the specifications of a Ni-Cd voltaic cell...Ch. 19 - Prob. 53GQCh. 19 - Balance the following equations. (a) Zn(s) +...Ch. 19 - Magnesium metal is oxidized, and silver ions are...Ch. 19 - You want to set up a series of voltaic cells with...Ch. 19 - Prob. 57GQCh. 19 - Prob. 58GQCh. 19 - In the table of standard reduction potentials,...Ch. 19 - Prob. 60GQCh. 19 - Four voltaic cells are set up. In each, one...Ch. 19 - The following half-cells are available: (i)...Ch. 19 - Prob. 63GQCh. 19 - Prob. 64GQCh. 19 - A potential of 0.142 V is recorded (under standard...Ch. 19 - Prob. 66GQCh. 19 - The standard potential, E, for the reaction of...Ch. 19 - An electrolysis cell for aluminum production...Ch. 19 - Electrolysis of molten NaCl is done in cells...Ch. 19 - A current of 0.0100 A is passed through a solution...Ch. 19 - A current of 0.44 A is passed through a solution...Ch. 19 - Prob. 72GQCh. 19 - Prob. 73GQCh. 19 - Prob. 74GQCh. 19 - The products formed in the electrolysis of aqueous...Ch. 19 - Predict the products formed in the electrolysis of...Ch. 19 - Prob. 77GQCh. 19 - The metallurgy of aluminum involves electrolysis...Ch. 19 - Prob. 79GQCh. 19 - Prob. 80GQCh. 19 - Prob. 81GQCh. 19 - Prob. 82GQCh. 19 - Two Ag+(aq) | Ag(s) half-cells are constructed....Ch. 19 - Calculate equilibrium constants for the following...Ch. 19 - Prob. 85GQCh. 19 - Use the table of standard reduction potentials...Ch. 19 - Prob. 87GQCh. 19 - Prob. 88GQCh. 19 - Prob. 89GQCh. 19 - A voltaic cell is constructed in which one...Ch. 19 - An expensive but lighter alternative to the lead...Ch. 19 - The specifications for a lead storage battery...Ch. 19 - Manganese may play an important role in chemical...Ch. 19 - Prob. 94GQCh. 19 - Iron(II) ion undergoes a disproportionation...Ch. 19 - Copper(I) ion disproportionates to copper metal...Ch. 19 - Prob. 97GQCh. 19 - Prob. 98GQCh. 19 - Consider an electrochemical cell based on the...Ch. 19 - Prob. 100ILCh. 19 - A silver coulometer (Study Question 106) was used...Ch. 19 - Four metals, A, B, C, and D, exhibit the following...Ch. 19 - Prob. 103ILCh. 19 - The amount of oxygen, O2, dissolved in a water...Ch. 19 - Prob. 105SCQCh. 19 - The free energy change for a reaction, rG, is the...Ch. 19 - Prob. 107SCQCh. 19 - (a) Is it easier to reduce water in acid or base?...Ch. 19 - Prob. 109SCQ
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- 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_forwardThe carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forwardA rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forward
- 4.60 Why are fuel additives used?arrow_forwardThree reactions very important to the semiconductor industry are The reduction of silicon dioxide to crude silicon, SiO2(s) + 2 C(s) → Si(s) + 2 CO(g) ΔrH° = 689.9 kJ/mol The formation of silicon tetrachloride from crude silicon, Si(s) + 2 Cl2(g) → SiCl4(g) ΔrH° = −657.01 kJ/mol The reduction of silicon tetrachloride to pure silicon with magnesium, SiCl4(g) + 2 Mg(s) → 2 MgCl2(s) + Si(s) ΔrH° = −625.6 kJ/mol Calculate the overall enthalpy change when 1.00 mol sand, SiO2, changes into very pure silicon by this series of reactions.arrow_forwardWhen lightning strikes, the energy can force atmospheric nitrogen and oxygen to react to make NO: N2(g)+O2(g)2NO(g)H=+181.8kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = +181.8 kJ? (c) What is the enthalpy change when 3.50 g nitrogen is reacted with excess O2(g)?arrow_forward
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