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QUESTION 9 For a particular cell based on the reaction: 3 AgCl(s) + Al(s) - 3...
For a particular cell based on the reaction: 3 AgCl(s) + Al(s) + 3 Ag(s) + A13+ (aq) + 3 C (aq) E° = +1.884 V at 298K. What is the value of the equilibrium constant, K, at 298 K for the reaction? Enter your answer in exponential format (example 1.23E-4) with two decimal places and no units If you use the constants R and F in your calcłılation, use ONLY these values R = 8.31451 J/K F = 96,485...
he standard cell potential for the following galvanic cell is 0.71 V. Mg(s)|Mg2+(aq)||Al3+(aq)|Al This reaction has an equilibrium constant, K = ________. Enter your answer in exponential format (sample 1.23E-4) with two decimal places and no units.
Part A For the galvanic cell that uses the reaction 2 Al(s) + 3 Cu2+ (aq) + 2 A13+ (aq) + 3 Cu(s) the value of n in the relationship AG'-nFEis Express your answer as an integer. Η ΑΣΦ ?
A voltaic cell is constructed using silver and aluminum. The following is the unbalanced redox reaction: Ag+ (aq) + Al(s) Ag (s) + A13+ (aq) What is the correct, balanced redox reaction that occurs in the cell? O A 5 Ag+ (aq) + 3 AI (5) - 5 Ag (s) + 3 A13+ (aq) O B. Ag* (aq) + 4 AI (5) ► Ag (s) + 4 A13+ (aq) OC 3 Ag* (aq) + Al(s) — 3 Ag (s) +...
Use the standard half-cell potentials listed below to calculate the standard free energy(K]for the following reaction occurring in an electrochemical cell at 25°C. Pb 2+ (aq) +2e--- Pb(s) E* - -0.13 Volt A13+ (aq) + 3 e-Al(s) E* =-1.66 volt a. 1.53 b. - 886 c-434 d. - 443 e. -1036 What is the standard free energy Gº) in Kilojoules for the reaction below at 298 Kelvin: Farady's constant = 96,485 joules/V. mole e Zn2+ (aq) + 2e ......> Zn(s)...
D Question 14 3 pts The following redox reaction is conducted with [A13+] = 0.80 M and [Mn2+] = 0.30 M. 2 Al(s) + 3 Mn2+(aq) + 2 A13+(aq) + 3 Mn(s) Ecell = 0.48 V Determine the moles of electrons transferred for the reaction as written (n), Q, and the cell potential (cell) at 298 K. n= (Select] Q = (Select] Ecell = (Select)
Use measured cell potential to calculate concentration. When [ Hg2+ ]=1.35 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.582 V. What is the Al** concentration in this cell? 3 Hg2+ (aq) + 2 Al (s) — 3 Hg (1) + 2 A1+ (aq) [A13+]= M
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+(aq) ----> Cu+2 (aq) + 2Ag(s) where [Ag+] = 0.00275 M and [Cu2+] = 8.75×10-4 M.
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+(aq) ----> Cu+2 (aq) + 2Ag(s) where [Ag+] = 0.00275 M and [Cu2+] = 8.75×10-4 M.
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V