18.3 Gibbs Free E...1←@25.3 Enthalpies of...Use the information in the ALEKS Data tab to sort the following chemical species by oxidizing power.O ELECTROCHEMISTRYRanking the strength of oxidizing and reducing agents using...speciesAl (aq)Ca²+ (aq)Ag* (aq)Na (aq)Explanation→#3oxidizing powerchoose oneX18.5 Gibbs Free E... Reading Schedulechoose one vchoose one vchoose oneCheck5$ACSearch or type URL%tvLO

Electrochemistry can be defined as the branch of chemistry that deal with oxidation and reduction reactions.Reduction is a process of gain of electrons and oxidation is process of loss of electrons. Higher the value of reduction potential, more easily it get reduced and oxidise other species.So higher will be its oxidising power. Ag+ (aq) has highest oxidising power. Because reduction potential is highest.Higher the value of reduction potential, more easily it get reduced and oxidise other species. Al3+ (aq) has lower oxidising power.than Ag+ (aq). Because reduction potential of Al3+ (aq) is lower than reduction potential of Ag+ (aq) Na+ (aq) has lower oxidising power.than Al3+ (aq).Because reduction potential of Na+ (aq) is lower than reduction potential of Al3+ (aq) Ca2+ (aq) has lowest oxidising power.Because reduction potential of Ca2+ (aq) is lowest.

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Chemistry

18.3 Gibbs Free E... 5.3 Enthalpies of... O ELECTROCHEMISTRY Ranking the strength of oxidizing and reducing agents using... Use the information in the ALEKS Data tab to sort the following chemical species by oxidizing por species Al' (ag) C₂² (aq) Ag (aq) Na (aq) oxidizing power choose one X 18.5 Gibbs Free E... Reading choose one ✓ choose one choose one 5

18.3 Gibbs Free E... 5.3 Enthalpies of... O ELECTROCHEMISTRY Ranking the strength of oxidizing and reducing agents using... Use the information in the ALEKS Data tab to sort the following chemical species by oxidizing por species Al' (ag) C₂² (aq) Ag (aq) Na (aq) oxidizing power choose one X 18.5 Gibbs Free E... Reading choose one ✓ choose one choose one 5

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Chegg.... Grades f... Grades f... 0 O ELECTROCHEMISTRY Using the Nernst equation to calculate nonstandard cell voltage Workshe... A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq) +12H* (aq) + 5Co (s) → 1₂ (s) + 6H₂O (1) + 5 Co²+ (aq) x10 Suppose the cell is prepared with 4.59 MIO3 and 4.70 M H in one half-cell and 7.33 M Co 2+ Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0.0 X A ALEKS -... μ 00 www-awy.aleks.com M Sign In I... 5 2. h Hulu | Pr... in the other. Home
d) For a thermodynamic process, when ΔΗsys > 0, and ΔSsys7, pH<7, or pH-7)
10.)
Given the following two half-reactions, determine which overall reaction is spontaneous, and calculate its standard cell potential. Cd2*(aq) + 2 e- Cd(s); E° = -0.403 V Zn2"(aq) + 2 e-Zn(s); E° = -0.763 V O A. Cd(s) + Zn2*(aq) OB. Cd(s) + Zn(s)¯ OC. ca²*(aq) + Zn²*(aq)' Cd2+(aq) + Zn(s); E° = -0.360 V Cd2*(aq) + Zn²+(aq); E° = -1.166 V PCd(s) + Zn(s); E° = +1.166 V O D. Cd2+(aq) + Zn(s) cd(s) + Zn2*(aq); E° = +0.360 V
Please answer.
Determine whether Sn is stable in 10-6 M Sn acid solution of pH = 2. Estimate: (i) the Gibbs free energy change and (ii) the cell potential for the corrosion cell. The activity coefficients are assumed to be 1. The hydrogen pressure is 1 atm.
Use the References to access important values if needed for this question. Consider the following half-reactions: Half-reaction E° (V) C2(g) + 2e" - 2CI (aq) 1.360V 2H"(aq) + 2e H2(g) 0.000V - Mn"(aq) + 2e¯ - Mn(s)|-1.180V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Cl,(g) oxidize Mn(s) to Mn*(aq)? 2+ (6) Which species can be reduced by H,(g)? If none, leave box blank.
V. (6)H in 0.20 bar Salt bridge |(ag) H(ao) Pt Ag wire coated with Agi(s) Nal (0.10 M) HCI (0.10 M) (a) Write the line notation for this cell. (b) Calculate the potential for each half-cell and the cell voltage E. (c) Write the spontaneous net cell reaction.
Balance the following reaction in basic solution. Ag(s) + Zn²+(aq) → Ag,O(ag) + Zn(s) Fill in the coefficients and substances for the balanced overall equation. Note: Do NOT leave any coeffient fields empty. If the coefficient is 1, choose "1" as opposed to leaving it blank. -- v Ag + -- v Zn2+ + v Zn + Ag,0 + -- v--
1. For the reaction: Cus) + 2Ag+ (aq) → 2+ Oxidation half-reaction: Cu(s) → Cuaq) + 2e¯ + Reduction half-reaction: 2Agaq) +2e → 2Ag Answer the following questions using Table 5.4.1: Table 5.4.1. Selected Standard Reduction Potentials at 25 °C Adapted from https://opentextb_c.ca/chemistry/chapter/17-3- Half-Reaction F2)+2 e2F¯(aq) O2(g) + 4H+ (aq) + 4e¯ → 2H₂O) Ag+(aq) + e → Ag(s) → Fe 2+ (aq) Fe³+ (aq) + e 12(1) + 2e™ 21 (24) Cu²+ (aq) + 2e Cu(s) - 2H*(aq) + 2e H₂0) + 2e → Zn(s) Zn² (29) Mg2 (aq) + 2 e→→ MgG) Ca²+ (aq) + 2e →→ Ca(s) a. What is the Eº of the anode half-cell? b. What is the E° for the cathode half-cell? c. Calculate the Eᵒcell for the reaction. d. Is the reaction spontaneous? Cu²+ (aq) + 2Ag(s) standard-reduction-potentials/ E° (V) +2.87 +1.23 +0.80 +0.77 +0.54 +0.34 0.00 -0.76 -2.37 -2.87
I’m having difficulties answering 4b.