Concept explainers
(a)
Interpretation:
The quantity of substance has to be calculated for the following metals
(a)The mass (in grams) of bismuth metal from a bismuth nitrate solution.
(b) The volume (in liters at 273 K and 1atm) of hydrogen gas from a sulfuric acid solution.
(c) The mass of cobalt (in grams) from a cobalt (III) chloride solution.
(b)
Interpretation:
The quantity of substance has to be calculated for the following metals
(a)The mass (in grams) of bismuth metal from a bismuth nitrate solution.
(b) The volume (in liters at 273 K and 1atm) of hydrogen gas from a sulfuric acid solution.
(c) The mass of cobalt (in grams) from a cobalt (III) chloride solution.
(c)
Interpretation:
The quantity of substance has to be calculated for the following metals
(a)The mass (in grams) of bismuth metal from a bismuth nitrate solution.
(b) The volume (in liters at 273 K and 1atm) of hydrogen gas from a sulfuric acid solution.
(c) The mass of cobalt (in grams) from a cobalt (III) chloride solution.
Want to see the full answer?
Check out a sample textbook solutionChapter 6 Solutions
ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM
- How is the pH scale defined? What range of pH values corresponds to acidic solutions? What range corresponds to basic solutions? Why is pH = 7.00 considered neutral? When the pH of a solution changes by one unit, by what factor does the hydrogen ion concentration change in the solution? How is pOH defined? How arc pH and pOH for a given solution related? Explain.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_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_forward
- An 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_forwardWhen molten lithium chloride, LiCl, is electrolyzed, lithium metal is liberated at the cathode. How many grams of lithium are liberated when 2.00 103 C of charge passes through the cell?arrow_forwardWhen aluminum foil is placed in hydrochloric acid, nothing happens for the first 30 seconds or so. This is followed by vigorous bubbling and the eventual disappearance of the foil. Explain these observations.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_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_forwardWrite 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_forward
- 1. If you wish to convert 0.0100 mol of Au3+ (aq) ions into Au(s) in a “gold-plating” process, how long must you electrolyze a solution if the current passing through the circuit is 2.00 amps? 483 seconds 4.83 104 seconds 965 seconds 1450 secondsarrow_forwardSome metals, such as thallium, can be oxidized to more than one oxidation state. Obtain the balanced net ionic equations for the following oxidation reduction reactions, in which nitric acid is reduced to nitric oxide, NO. a Oxidation of thallium metal to thallium(I) ion by nitric acid. b Oxidation of thallium(I) ion to thallium(III) ion by nitric acid. c Oxidation of thallium metal to thallium(III) by nitric acid. [Consider adding the a and b equations.]arrow_forwardUse the appropriate tables to calculate H for (a) the reaction between MgC03(s) and a strong acid to give Mg2+(aq), CO2(g), and water. (b) the precipitation of iron(III) hydroxide from the reaction between iron(III) and hydroxide ions.arrow_forward
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning