Chemistry In Context
9th Edition
ISBN: 9781259638145
Author: Fahlman, Bradley D., Purvis-roberts, Kathleen, Kirk, John S., Bentley, Anne K., Daubenmire, Patrick L., ELLIS, Jamie P., Mury, Michael T., American Chemical Society
Publisher: Mcgraw-hill Education,
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Textbook Question
Chapter 7, Problem 4Q
What is the difference between a galvanic cell and a true battery? Give an example for each.
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Chemistry In Context
Ch. 7.1 - Prob. 7.2YTCh. 7.2 - Skill Building Coulombs The SI unit of electric...Ch. 7.2 - Prob. 7.4YTCh. 7.4 - Prob. 7.5YTCh. 7.4 - Scientific Practices The Shift from NiCd to NiMH...Ch. 7.5 - Scientific Practices The Battery in Your Car Lets...Ch. 7.7 - Prob. 7.9YTCh. 7.8 - Prob. 7.10YTCh. 7.9 - Prob. 7.11YTCh. 7.9 - Prob. 7.12YT
Ch. 7.10 - Prob. 7.13YTCh. 7.10 - Prob. 7.14YTCh. 7.11 - Skill Building Metal Refining (Smelting) The...Ch. 7.11 - You Decide Could Metals Become Extinct? In 2015,...Ch. 7.11 - Prob. 7.17YTCh. 7 - You Decide The Baghdad Battery Alessandro Volta is...Ch. 7 - Prob. 1QCh. 7 - Prob. 2QCh. 7 - Which chemical species gets oxidized and which...Ch. 7 - What is the difference between a galvanic cell and...Ch. 7 - Two common units associated with electricity are...Ch. 7 - Consider the galvanic cell pictured. A coating of...Ch. 7 - Prob. 7QCh. 7 - a. How does the voltage from a tiny AAA alkaline...Ch. 7 - Identify the type of galvanic cell commonly used...Ch. 7 - The mercury battery has been used extensively in...Ch. 7 - Prob. 12QCh. 7 - During the conversion of O2(g) to H2O(l) in a fuel...Ch. 7 - How does the reaction between hydrogen and oxygen...Ch. 7 - This diagram represents the hydrogen fuel cell...Ch. 7 - What is a PEM fuel cell? How does it differ from...Ch. 7 - How do PEM fuel cells allow H2 and O2 to combine...Ch. 7 - In addition to hydrogen, methane also has been...Ch. 7 - Prob. 19QCh. 7 - Potassium and lithium both are reactive Group 1...Ch. 7 - What challenges keep hydrogen fuel cells from...Ch. 7 - Explain the concept of energy density of a battery...Ch. 7 - Describe how a normal AA battery stores and...Ch. 7 - Prob. 24QCh. 7 - What is the difference between an electrolytic...Ch. 7 - Provide some differences between a leadacid...Ch. 7 - Describe the importance of a separator in primary...Ch. 7 - The company ZPower is promoting its silverzinc...Ch. 7 - Prob. 29QCh. 7 - Prob. 30QCh. 7 - Describe some advantages and disadvantages of...Ch. 7 - You never need to plug in Toyotas gasolinebattery...Ch. 7 - Prob. 33QCh. 7 - Hydrogen is considered an environmentally friendly...Ch. 7 - Fuel cells were invented in 1839 but never...Ch. 7 - Hydrogen and methane both can react with oxygen in...Ch. 7 - Engineers have developed a prototype fuel cell...Ch. 7 - Prob. 38QCh. 7 - Describe some similarities and differences between...Ch. 7 - Prob. 40QCh. 7 - Prob. 41QCh. 7 - Prob. 42QCh. 7 - Small quantities of hydrogen gas can be prepared...Ch. 7 - Prob. 44QCh. 7 - Although Alessandro Volta is credited with the...Ch. 7 - Prob. 46QCh. 7 - Prob. 47QCh. 7 - What is the tragedy of the commons? How does this...Ch. 7 - How can the principles of green chemistry be...Ch. 7 - If all of todays technology presently based on...Ch. 7 - Consider these three sources of light: a candle, a...Ch. 7 - Prob. 52Q
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- 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_forwardThe voltaic cell is represented as Zn(s)Zn2+(1.0M)Cu2+(1.0M)Cu(s) Which of the following statements is not true of this cell? a The mass of the zinc electrode, Zn(s), decreases as the cell runs. b The copper electrode is the anode. c Electrons flow through the external circuit from the zinc electrode to the copper electrode. d Reduction occurs at the copper electrode as the cell runs. e The concentration of Cu2+ decreases as the cell runs.arrow_forwardConsider 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?arrow_forward
- 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)?arrow_forwardAn electrolytic cell is set up with Cd(s) in Cd(NO3)2(aq) and Zn(s) in Zn(NO3)2(aq). Initially both electrodesweigh 5.00 g. After running the cell for several hours theelectrode in the left compartment weighs 4.75 g. (a) Which electrode is in the left compartment? (b) Does the mass of the electrode in the right compartmentincrease, decrease, or stay the same? If the masschanges, what is the new mass? (c) Does the volume of the electrode in the right compartment increase, decrease, or stay the same? If the volumechanges, what is the new volume? (The density of Cd is8.65 g/cm3.)arrow_forwardAs an example of an electrolytic cell, the text states: Sodium chloride is electrolyzed commercially in an apparatus called the Downs cell to produce sodium and chlorine. This is a high-temperature operation; the electrolyte is molten NaCl. Write the half-reaction equations for the changes taking place at each electrode. Is the electrode at which sodium is produced the anode or the cathode? The Downs cell electrolyzes molten melted sodium chloride, producing sodium and chlorine.arrow_forward
- A voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous solution of AgNO3.The other half cell consists of an inert platinum wire in an aqueous solution containing Fe2+(aq) and Fe3+(aq). (a) Calculate the cell potential, assuming standard conditions. (b) Write the net ionic equation for the reaction occurring in the cell. (c) Which electrode is the anode and which is the cathode? (d) If [Ag+] is 0.10 M, and [Fe2+] and [Fe3+] are both 1.0 M, what is the cell potential? Is the net cell reaction still that used in part (a)? If not, what is the net reaction under the new conditions?arrow_forwardConsider the following galvanic cell: Calculate the concentrations of Ag+(aq) and Ni2+(aq) once the cell is dead.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
- Write the equation for the reaction, if any, that occurs when each of the following experiments is performed under standard conditions. (a) Sulfur is added to mercury. (b) Manganese dioxide in acidic solution is added to liquid mercury. (c) Aluminum metal is added to a solution of potassium ions.arrow_forwardIdentify each statement as true or false. Rewrite each false statement to make it true. (a) Oxidation always occurs at the anode of an electrochemical cell. (b) The anode of a discharging voltaic cell is the site ofreduction and is negative. (c) Standard-state conditions for electrochemical cells are aconcentration of 1.0 M for dissolved species and a pressure of 1 bar for gases. (d) The potential of a voltaic cell does not change withtemperature. (e) All product-favored oxidation-reduction reactions have astandard cell potential Ecell, with a negative sign.arrow_forward
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