Concept explainers
(a)
Interpretation:
The balancing of given half-reaction of redox should be explained.
Concept introduction:
Redox:
The reduction and oxidation reactions are occur simultaneously with in a single reaction is known as
The unbalanced charge (electron) and atoms (ions) in the equation of redox reactions are commonly balanced by half reaction method.
In this method, the given redox reaction is separated by two half reactions, one is oxidation and another one is reduction.
The medium of the reaction is used to balance the Hydrogen and Oxygen ions in the half cell reactions.
Balancing of redox reaction in acid medium:
In the acid medium, the addition of
Charge is balanced by addition of electron in the sides with the greater positive charge.
Balancing of redox reaction in basic medium:
In the acid medium, the addition of
Charge is balanced by addition of electron in the sides with the greater positive charge.
(b)
Interpretation:
The balancing of given half-reaction of redox should be explained.
Concept introduction:
Redox:
The reduction and oxidation reactions are occur simultaneously with in a single reaction is known as redox reaction.
Balancing of redox reaction:
The unbalanced charge (electron) and atoms (ions) in the equation of redox reactions are commonly balanced by half reaction method.
In this method, the given redox reaction is separated by two half reactions, one is oxidation and another one is reduction.
The medium of the reaction is used to balance the Hydrogen and Oxygen ions in the half cell reactions.
Balancing of redox reaction in acid medium:
In the acid medium, the addition of
Charge is balanced by addition of electron in the sides with the greater positive charge.
Balancing of redox reaction in basic medium:
In the acid medium, the addition of
Charge is balanced by addition of electron in the sides with the greater positive charge.
(c)
Interpretation:
The balancing of given half-reaction of redox should be explained.
Concept introduction:
Redox:
The reduction and oxidation reactions are occur simultaneously with in a single reaction is known as redox reaction.
Balancing of redox reaction:
The unbalanced charge (electron) and atoms (ions) in the equation of redox reactions are commonly balanced by half reaction method.
In this method, the given redox reaction is separated by two half reactions, one is oxidation and another one is reduction.
The medium of the reaction is used to balance the Hydrogen and Oxygen ions in the half cell reactions.
Balancing of redox reaction in acid medium:
In the acid medium, the addition of
Charge is balanced by addition of electron in the sides with the greater positive charge.
Balancing of redox reaction in basic medium:
In the acid medium, the addition of
Charge is balanced by addition of electron in the sides with the greater positive charge.
(d)
Interpretation:
The balancing of given half-reaction of redox should be explained.
Concept introduction:
Redox:
The reduction and oxidation reactions are occur simultaneously with in a single reaction is known as redox reaction.
Balancing of redox reaction:
The unbalanced charge (electron) and atoms (ions) in the equation of redox reactions are commonly balanced by half reaction method.
In this method, the given redox reaction is separated by two half reactions, one is oxidation and another one is reduction.
The medium of the reaction is used to balance the Hydrogen and Oxygen ions in the half cell reactions.
Balancing of redox reaction in acid medium:
In the acid medium, the addition of
Charge is balanced by addition of electron in the sides with the greater positive charge.
Balancing of redox reaction in basic medium:
In the acid medium, the addition of
Charge is balanced by addition of electron in the sides with the greater positive charge.
Want to see the full answer?
Check out a sample textbook solutionChapter 7 Solutions
General Chemistry: Atoms First
- Consider 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_forwardOrder the following oxidizing agents by increasing strength under standard-state conditions: Mg2+(aq), Hg2+(aq), Pb2+(aq).arrow_forward
- What is the standard cell potential you would obtain from a cell at 25C using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?arrow_forwardA solution contains the ions H+, Ag+, Pb2+, and Ba2+, each at a concentration of 1.0 M. (a) Which of these ions would be reduced first at the cathode during an electrolysis? (b) After the first ion has been completely removed by electrolysis, which is the second ion to be reduced? (c) Which, if any, of these ions cannot be reduced by the electrolysis of the aqueous solution?arrow_forwardConsider these half-reactions: (a) Which is the weakest oxidizing agent? (b) Which is the strongest oxidizing agent? (c) Which is the strongest reducing agent? (d) Which is the weakest reducing agent? (e) Will Sn(s) reduce Ag+(aq) to Ag(s)? (f) Will Hg() reduce Sn2+(aq) to Sn(s)? (g) Name the ions that can be reduced by Sn(s). (h) Which metals can be oxidized by Ag+(aq)?arrow_forward
- Write balanced equations for the following half-reactions. Specify whether each is an oxidation or reduction. (a) H2O2(aq) O2(g)(in acid) (b) H2C2O4(aq) CO2(g)(in acid) (c) NO3(aq) NO(g)(in acid) (d) MnO4(aq) MnO2(s)(in base)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_forwardA 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_forward
- A 1.0-L sample of 1.0 M HCl solution has a 10.0 A current applied for 45 minutes. What is the pH of the solution after the electricity has been turned off?arrow_forwardAn electrode is prepared by dipping a silver strip into a solution saturated with silver thiocyanate, AgSCN, and containing 0.10 M SCN . 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 0.45 V. What is the solubility product of silver thiocyanate?arrow_forwardCalculate the equilibrium constant at 25 C for the reaction 2 Ag+(aq) + Hg() 2 Ag(s) + Hg2+(aq)arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- General 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 LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning