Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
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Textbook Question
Chapter 19, Problem 30RQ
lectricity
What reactions occur at the electrodes in the ordinary dry cell?
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Chapter 19 Solutions
Chemistry: The Molecular Nature of Matter
Ch. 19 - Sketch and label a galvanic cell that makes use of...Ch. 19 - Write the anode and cathode half-reactions for the...Ch. 19 - Copper metal and zinc metal will both reduce Ag+...Ch. 19 - A galvanic cell has a standard cell potential of...Ch. 19 - Using the positions of the respective...Ch. 19 - Use the positions of the half-reactions in Table...Ch. 19 - What are the overall cell reaction and the...Ch. 19 - What are the overall cell reaction and the...Ch. 19 - A 1.0 M solution of copper(II) perchlorate and 1.0...Ch. 19 - A galvanic cell is constructed with two platinum...
Ch. 19 - Prob. 11PECh. 19 - Under standard state conditions, which of the...Ch. 19 - A certain reaction has an Ecello of 0.107 volts...Ch. 19 - Calculate G for the reactions that take place in...Ch. 19 - The calculated standard cell potential for the...Ch. 19 - Use the following half-reactions and the data in...Ch. 19 - A galvanic cell is constructed with a copper...Ch. 19 - In Example 19.9, assume all conditions are the...Ch. 19 - In the analysis of two other water samples by the...Ch. 19 - A galvanic cell is constructed with a copper...Ch. 19 - In the electrolysis of an aqueous solution...Ch. 19 - In the electrolysis of an aqueous solution...Ch. 19 - How many moles of hydroxide ion will be produced...Ch. 19 - How many minutes will it take for a current of...Ch. 19 - What current must be supplied to deposit 0.0500 g...Ch. 19 - Suppose the solutions in the galvanic cell...Ch. 19 - Galvanic Cells What is a galvanic cell? What is a...Ch. 19 - Galvanic Cells
19.2 What is the function of a salt...Ch. 19 - Galvanic Cells In a coppersilver cell, why must...Ch. 19 - Galvanic Cells What is the general name we give to...Ch. 19 - Galvanic Cells In a galvanic cell, do electrons...Ch. 19 - Galvanic Cells Explain how the movement of the...Ch. 19 - Galvanic Cells
19.7 Aluminum will displace tin...Ch. 19 - Galvanic Cells
19.8 Make a sketch of the galvanic...Ch. 19 - Galvanic Cells 19.9 Make a sketch of a galvanic...Ch. 19 - Galvanic Cells Make a sketch of a galvanic cell...Ch. 19 - Prob. 11RQCh. 19 - Cell Potentials How are standard reduction...Ch. 19 - If you set up a galvanic cell using metals not...Ch. 19 - Cell Potentials Galvanic cells are set up so that...Ch. 19 - Utilizing Standard Reduction Potentials Describe...Ch. 19 - Utilizing Standard Reduction Potentials What do...Ch. 19 - Prob. 17RQCh. 19 - Utilizing Standard Reduction Potentials Describe...Ch. 19 - Prob. 19RQCh. 19 - Prob. 20RQCh. 19 -
19.21 What is the equation that relates the...Ch. 19 - EcelloandG Show how the equation that relates the...Ch. 19 - Ecello and G What is the cell potential of a...Ch. 19 - Cell Potentials and Concentration 19.24 The cell...Ch. 19 - Cell Potentials and Concentration What is a...Ch. 19 - Cell Potentials and Concentration Describe what...Ch. 19 - Electricity What are the anode and cathode...Ch. 19 - Prob. 28RQCh. 19 - Electricity
19.29 How is a hydrometer constructed?...Ch. 19 - lectricity What reactions occur at the electrodes...Ch. 19 - Electricity
19.31 What chemical reactions take...Ch. 19 - Prob. 32RQCh. 19 - Electricity
19.33 What are the anode, cathode, and...Ch. 19 - Electricity Give two reasons why lithium is such...Ch. 19 - Electricity What are the electrode materials in a...Ch. 19 - Electricity
19.36 What are the electrode materials...Ch. 19 - Prob. 37RQCh. 19 - Electricity Write the cathode, anode, and net cell...Ch. 19 - Electricity What advantages do fuel cells offer...Ch. 19 - Electrolytic Cells What electrical charges do the...Ch. 19 - Electrolytic Cells
19.41 Why must electrolysis...Ch. 19 - Electrolytic Cells Why must NaCl be melted before...Ch. 19 - Electrolytic Cells Write half-reactions for the...Ch. 19 - Electrolytic Cells
19.44 What happens to the pH of...Ch. 19 - Electrolysis Stoichiometry
19.45 What is a...Ch. 19 - Electrolysis Stoichiometry
19.46 Using the same...Ch. 19 - Electrolysis Stoichiometry
19.47 An electric...Ch. 19 - Electrolysis Stoichiometry
19.48 An electric...Ch. 19 - Practical Applications of Electrolysis What is...Ch. 19 - Practical Applications of Electrolysis
19.50...Ch. 19 - Practical Applications of Electrolysis In the...Ch. 19 - Prob. 52RQCh. 19 - Practical Applications of Electrolysis Describe...Ch. 19 - Prob. 54RQCh. 19 - Galvanic Cells Write the half-reactions and the...Ch. 19 - Galvanic Cells Write the half-react ions and the...Ch. 19 - Write the cell notation for the following galvanic...Ch. 19 - Write the cell notation for the following galvanic...Ch. 19 - For each pair of substances, use Table 19.l to...Ch. 19 - 19.60 For each pair of substances, use Table 19.1...Ch. 19 - Use the data in Table 19.1 to calculate the...Ch. 19 - 19.62 Use the data in Table 19.1 to calculate the...Ch. 19 - From the positions of the half-reactions in Table...Ch. 19 - Use the data in Table 19.1 to determine which of...Ch. 19 - 19.65 From the half-reactions below, determine the...Ch. 19 - 19.66 What is the standard cell potential and the...Ch. 19 - What will be the spontaneous reaction among...Ch. 19 - What will be the spontaneous reaction among...Ch. 19 - Will the following reaction occur spontaneously...Ch. 19 - Determine whether the reaction:...Ch. 19 -
19.71 Calculate for the following reaction as...Ch. 19 - EcellandG Calculate G for the reaction...Ch. 19 - Given the following half-reactions and their...Ch. 19 - Calculate Kc for the system Ni2++CoNi+Co2+ Use the...Ch. 19 - 19.75 The system
has a calculated What is the...Ch. 19 - Determine the value of Kc at 25C for the reaction...Ch. 19 - Cell Potentials and Concentrations 19.77 The cell...Ch. 19 - Cell Potentials and Concentrations
19.78 The for...Ch. 19 - *19.79 A cell was set up having the following...Ch. 19 - A silver wire coated with AgCl is sensitive to the...Ch. 19 - At 25C, a galvanic cell was set up having the...Ch. 19 - *19.82 Suppose a galvanic cell was constructed at ...Ch. 19 - *19.83 What is the potential of a concentration...Ch. 19 - *19.84 What is the potential of a concentration...Ch. 19 - Prob. 85RQCh. 19 - Prob. 86RQCh. 19 - What products would we expect at the electrodes if...Ch. 19 - What products would we expect at the electrodes if...Ch. 19 - Using Table 19.1, list the ions in aqueous...Ch. 19 - Prob. 90RQCh. 19 - Electrolysis Stoichiometry
19.91 How many moles of...Ch. 19 - Electrolysis Stoichiometry
19.92 How many moles of...Ch. 19 - 19.93 How many grams of Fe(OH)2 are produced at an...Ch. 19 - 19.94 How many grams of would be produced in the...Ch. 19 - Prob. 95RQCh. 19 - 19.96 How many hours would it take to generate...Ch. 19 - 19.97 How many amperes would be needed to produce...Ch. 19 - 19.98 A large electrolysis cell that produces...Ch. 19 - *19.99 The electrolysis of 250 mL of a brine...Ch. 19 - *19.100 A 100.0 mL sample of 2.00MNaCl was...Ch. 19 - *19.101 A watt is a unit of electrical power and...Ch. 19 - Suppose that a galvanic cell were set up having...Ch. 19 - Prob. 103RQCh. 19 - *19.104 The value of for AgBr is . What will be...Ch. 19 - 19.105 Based only on the half-reactions in Table...Ch. 19 - A student set up an electrolysis apparatus and...Ch. 19 - *19.107 A hydrogen electrode is immersed in a 0.10...Ch. 19 - *19.108 What current would be required to deposit ...Ch. 19 - *19.109 A solution containing vanadium in an...Ch. 19 - Consider the reduction potentials of the following...Ch. 19 - An Ag/AgCl electrode dipping into 1.00MHCl has a...Ch. 19 - Prob. 112RQCh. 19 - Consider the following galvanic cell:...Ch. 19 - The electrolysis of 0.250 L of a brine solution...Ch. 19 - A solution of NaCl in water was electrolyzed with...Ch. 19 - How many milliliters of dry gaseous H2, measured...Ch. 19 - *19.117 At , a galvanic cell was set up having the...Ch. 19 - Given the following reduction half-reactions and...Ch. 19 - The normal range of chloride ions in blood serum...Ch. 19 - An unstirred solution of 2.00 M NaCl was...Ch. 19 - What masses of and O2 in grams would have to react...Ch. 19 - *19.122 Draw an atomic-level diagram of the events...Ch. 19 - *19.123 In biochemical systems, the normal...Ch. 19 - Calculate a new version of Table 19.1 using the...Ch. 19 - In Problem 19.83, the potential at 75C was...Ch. 19 - There are a variety of methods available for...Ch. 19 - *19.128 Most flashlights use two or more batteries...Ch. 19 - 19.129 If two electrolytic cells are placed in...Ch. 19 - Prob. 130RQCh. 19 - Prob. 131RQ
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- Predict the chemical reactions that will occur at the two electrodes in the electrolysis of an aqueous sodium hydroxide solution.arrow_forward. In which direction do electrons flow in a galvanic cell, from anode to cathode or vice versa?arrow_forwardWrite the cell notation for a voltaic cell with the following half-reactions. Ni(s)Ni2+(aq)+2ePb2(aq)+2ePb(s)arrow_forward
- Give 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_forwardAs the voltaic cell shown here runs, the blue solution gradually gets lighter in color and the gray solution gets darker. (a) What species is oxidized and what is reduced? (b) Which electrode is the anode and which is the cathode? (C) Which metal electrode gains mass? (d) In which direction do electrons flow through the external circuit?arrow_forwardThe following two half-reactions arc involved in a voltaic cell. At standard conditions, what species is produced at each electrode? Ag++eAgE=0.80VNi2++2eNiE=0.25Varrow_forward
- For a voltage-sensitive application, you are working on a battery that must have a working voltage of 0.85 V. The half-cells to be used have a standard cell potential of 0.97 V. What must be done to achieve the correct voltage? What information would you need to look up?arrow_forwardConsider the voltaic cell Zn(s)Zn2+(aq)Cr3(aq)Cr(s) Write the half-cell reactions and the overall cell reaction. Make a sketch of this cell and label it. Include labels showing the anode, cathode and direction of electron flow.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
- As 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_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_forwardA voltaic cell has an iron rod in 0.30 M iron(III) chloride solution for the cathode and a zinc rod in 0.20 M zinc sulfate solution for the anode. The half-cells are connected by a salt bridge. Write the notation for this cell.arrow_forward
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