Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Consider a galvanic
Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V
Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V
Which of the following is the half-reaction that takes place at the anode?
A) Cr³⁺(aq) + 3 e⁻ → Cr(s)
B) Cr(s) → Cr³⁺(aq) + 3 e⁻
C) Zn²⁺(aq) + 2 e⁻ → Zn(s)
D) Zn(s) → Zn²⁺(aq) + 2 e⁻
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 3 steps with 3 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Calculate E°cell for the cell for the reaction 2 Ga(s) + 3 Sn4+(aq) → 3 Sn2+(aq) +2 Ga3+(aq).The standard reduction potentials are as follows: Ga3+(aq) + 3 e− → Ga(s) E° = –0.55 V Sn4+(aq) + 2 e− → Sn2+(aq) E° = 0.15Varrow_forwardUse the standard reduction potentials given below to predict if a reaction will occur between Ag(s) and F2 (g), when the two are brought in contact via standard half-cells in a voltaic cell. F2 (g)+2e7 →2F (aq) E red Agt (ag)+e → Ag(s) E red + = If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) - 2.870 V 0.799 V +arrow_forwardConsider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag ℰ° = +0.80 V Fe2+ + 2 e− → Fe ℰ° = −0.44 V (a) Determine the overall cell reaction and calculate ℰ ° cell . (b) Calculate ΔG° and K for the cell reaction at 25°C. (c) Calculate ℰcell at 25°C when [Ag+ ] = 1.0 ✕ 10−4 M and [Fe2+ ] = 1.0 ✕ 10−2 M.arrow_forward
- Use the standard reduction potentials given below to predict if a reaction will occur between Zn(s) and Cl2(g), when the two are brought in contact via standard half-cells in a voltaic cell. | Cl2(g) + 2e¯¯ →2C1¯¯ (aq) E Zn2+ = 1.360 V red (aq) + 2e → Zn(s) E = = -0.763 V red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + +arrow_forwardDesigning a galvanic cell from tw... A chemist designs a galvanic cell that uses these two half-reactions: standard reduction |MnO4(aq)+2H₂O(l)+3e¯ → MnO₂(S)+4OH(aq) Cl₂(g) +2e 2 Cl(aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that 0 happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. 0 half-reaction O Yes O No ☐v - potential Ered = +0.59 V = +1.359 V ロ→ロ X x10 Sarrow_forwardConsider a galvanic electrochemical cell constructed using Cr/Cr³+ and Zn/Zn²+ at 25 °C. The following half-reactions are provided for each metal: Cr³+(aq) + 3 e →→ Cr(s) E°red = -0.744 V Zn²+ (aq) + 2 e →→ Zn(s) Eºred = -0.763 V Write the balanced equation for the overall reaction in acidic solution. 3 Zn(s) + 2 Cr³+ (aq) → 3 Zn²+(aq) + 2 Cr (s) 1 1 + 4- Reset 2 H₂O+ 0 3_ ( ) 3 03 04 4 H H+ 5 5 11 Zn 6 6 ²+ 7 07 (s) H₂O ● 3+ (1) 8 9 0 e 4+ x H₂O 9 (g) (aq) □o Cr Deletearrow_forward
- Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C.2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)Mg2+(aq) + 2 e⁻ → Mg(s) E° = -2.37 VAl3+(aq) + 3 e⁻ → Al(s) E° = -1.66 V A) 1.0 × 1024 B) 1.1 × 10-73 C) 1.1 × 1072 D) 8.9 × 10-73 E) 4.6 × 1031arrow_forwardRefer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): Ni Ag 1.0 M Ni2+ 1.0 M Ag* The standard reduction potentials are as follow: Ni2+ + 2 e- → Ni(s), E° = -0.25 Ag* + e - Ag(s), E° = 0.7996 When current is allowed to flow, which species is oxidised? Select one: а. Ag b. Cannot be determined from the data given. C. Ni2+ O d. Ag* O e. Niarrow_forwardA chemist designs a galvanic cell that uses these two half-reactions: 3+ 2+ Fe (aq)+e → Fe (aq) Cro (aq) + 4H₂O(1)+3e¯ Cr(OH)3(s)+5 OH(aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is half-reaction spontaneous as written. 0 standard reduction potential Ed=+0.771 V 'red E 'red = -0.13 V ロ→ロ × x10 5arrow_forward
- Consider the following galvanic cells. Diagram I Au- cº 1.0 M Au³+ 3+ chemPad XX² (b) balanced cell equation II chemPad 8⁰ XX→→ 1.0 M Cu+ 1.0 M Cu²+ For each galvanic cell, give the balanced cell reaction and determine °. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) (a) balanced cell equation I Help Greek Pt Help Greek Diagram II Cd- 1.0 M Cd2+ -Pt Ai 1.0 M VO₂, 1.0 MH+ 1.0 M VO²+arrow_forwardChemistry Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V Write the balanced equation for the overall reaction in acidic solution.arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY