[References] a. Will dichromate ions oxidize chloride ions to free chlorine in acidic solution? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction E (V) Cr 0,2 + 14H+ +6e 2Cr* + 7H2O +1.33 Cl + 2e 2C1 +1.36 O yes O no b. Will Fet oxidize'Sn+ to Sn*? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction € (V) Fe +e+Fe* +0.77 Sn +2e Sn²* +0.15 Oyes Ono

[References] a. Will dichromate ions oxidize chloride ions to free chlorine in acidic solution? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction E (V) Cr 0,2 + 14H+ +6e 2Cr* + 7H2O +1.33 Cl + 2e 2C1 +1.36 O yes O no b. Will Fet oxidize'Sn+ to Sn? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction € (V) Fe +e+Fe +0.77 Sn +2e Sn²* +0.15 Oyes Ono

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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Calculate the cell potential, E, for the given reactions at 25.00 "C using the ion concentrations provided. Then, determine if th cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E). Pt(s) + Fe²(aq) = P² (aq) + Fe(s) [Fe²*1 = 0.0064 M E= incorrect -4761 E= Cu(s) + 2 Ag* (aq) = Cu² (aq) + 2 Ag(s) |Cu²+1 = 0.027 M Ag1=0.027 M E [P1²*1 = 0.067 M Co² (aq) + Ti (aq) — Co¹ (aq) + Ti² '(aq) Co²1 = 0.055 M Co= 0.030 M ITP 1 = 0.0070 M T² = 0.0107 M mam V The cell is not spontaneous spontaneous. The cell is spontaneous not spontaneous. incorrect The cell is spontaneous not spontaneoux.
Determine E°, AG°, and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fe3+ + 2 H,0 4 Fe²+ + O, + 4H+ Fe3+ + e-= Fe²+ E° = 0.771 V 0, + 2 H* + 2 e¯2 H,0 E° = 1.229 V E° = V K = Is the overall reaction spontaneous as written? AG° = spontaneous not spontaneous
29b
Standard Reduction Potentials at 25 °C Half-reaction. Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e →→Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Aut 2Au + Au³+ Will Au* disproportionate in aqueous solution? To justify your answer, what is the standard cell voltage for the disproportionation reaction?
Given the following information: • Electrochemical cell: Niº | Ni2+ || Ag+ | Ago • Half-cell reactions with corresponding Reduction Potential: o Ni2+ + 2e Niº ▪ °Ecell = -0.250 V o Ag++ 1e Agº ▪ °Ecell= + 0.800 V . Conditions: 1 molar concentrations for ions at at 25°C How many electrons were exchanged between the two cells? Please indicate your answer as a number (e.g. 15). N
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2+ 4+ a. Will Fe+ oxidize Sn to Sn*t ? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction e° (V) Fes+ +e → Fe2+ +0.77 Sn n4+ + 2e → Sn²+ +0.15 O yes O no b. Will dichromate ions oxidize chloride ions to free chlorine in acidic solution? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction e° (V) Cr2 0, + 14H+ + 6e¯ → 2Cr³+ + 7H2O +1.33 Cl2 + 2e → 2C1 +1.36 O yes O no
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Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)
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