The cell notation for the Galvanic cell is Cd(syCd2+/l/½(syI" The Standard Reduction Potential are as follows: E°Ca2+/cd = -0.403 V; E12/1 = 0.5355 V Calculate the standard cell potential If the Cadmium ions have a concentration of 0.010 M and the iodide ions have a concentration of 0.020 M, calculate the electromotive force (EMF) of the cell. The Gibbs Free Energy of the cell is

The cell notation for the Galvanic cell is Cd(syCd2+/l/½(syI" The Standard Reduction Potential are as follows: E°Ca2+/cd = -0.403 V; E12/1 = 0.5355 V Calculate the standard cell potential If the Cadmium ions have a concentration of 0.010 M and the iodide ions have a concentration of 0.020 M, calculate the electromotive force (EMF) of the cell. The Gibbs Free Energy of the cell is

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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A galvanic cell using Mg / Mg*" and Cu / Cu" half-cells operates under standard-state conditions at 25 °C, and each compartment has a volume of 227 mL. The cell delivers 0.31 A for 32.1 h. (a) How many grams of Cu are deposited? g Cu
Consider a galvanic cell consisting of the Cr3+/Cr (Eo=-0.74 V) and the Ag+/Ag (Eo=+0.8 V) systems in the half-cells. a) What is the standard cell potential, Eocell, for the galvanic cell in volts (V) and millivolts (mV)?
Calculate E° cell from the tabulated standard reduction potentials for each of the following reactions in aqueous solution. Then calculate AG° and K at 25°C from E° cell' 4 F = 9.65 x 10 J/V•mol e R = 8.314 J/mol•K Acidic solution Standard reduction potential, E (Volts) Cu?" (aq) + e → Cu*(aq) Cu'(ag) + e Cu(s) Mno, (ag) + 8H"(ag) + 5e Mn2"(ag) + 4H,0 0.153 0.521 1.507 Fe"(aq) + e Fe?"(aq) 0.771 Basic solution -1.22 Zn(OH)-(s) + 2e Zn(s) + 4OH(aq) Mno, (aq) + 2H,O + 3e → Mno,(s) + 40H (aq) 0,588 Mn04 + 5FE2+= Mn2+ + 5FE3+ (acidic solution) E°cell = AG° = kJ/mol K =
Chemistry Question
Consider the following electrochemical cell notation with a cell potential of 0.300 V. Pt ∣Cr3+(aq, 0.015M) ∣ Cr2+(aq, 0.045M) ∣∣ H+(aq,?M) ∣ H2(g,1.0 atm) ∣ PtWrite the two half reactions (show the overall reaction) andCalculate the standard cell potential and determine if this cell is more or less spontaneous at the nonstandard conditions?
A galvanic (voltaic) cell consists of an inert platinum clectrode in a solution containing 1.0 M tin(IV) ion and 1.0M tin(II) ion, and another inert platinum clectrode in a solution containing 1.0 M iron(III) ion and 1.0M iron(II) ion, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Standard reduction potentials can be found in the standard reduction potentials table. E: cell V
A Galvanic cell consists of Mg electrode in a 1.0 mol L -1 Mg(NO3)2 solution and a Ag electrode in a 1.0 mol L-1 AgNO3 solution. Calculate standard emf for the spontaneous reaction of this electrochemical cell at 25 C
a) Balance the following reactions. b) Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. c) Identify the reactions with K > 1 among the following redox reactions. d) Write the line representations for the Galvanic cells, indicating the anode and cathode. Cl2 + Br- --> Cl- + Br2 MnO4- + H+ + Ce3+ --> Ce4+ + Mn2+ + H2O Pb2+ -->Pb + Pb4+ NO3- + H+ + Zn --> Zn2+ + NO2 + H2O
Consider 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.
Sketch a galvanic cell ( immersed in 1M solution) with the cell notation Cr(s)/Cr 3+ (aq) // Cu2+/Cu (s) Please indicate the anode and cathode, the flow of electrons, the reaction in the anode and cathode, overall reaction, and the voltage of the cell- is it spontaneous
edit: Calculate the cell potential for the following galvanic cell at 25°C: Al(s) Al3+ (0.0632 M)|| Au3+ (0.255 M)|Au(s)
Use the Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of the following half-cell systems: Ag+(0.010M) + e- --> Ag Eo= +0.80 V Cr3+(O.010M) + 3e- --> Cr Eo= -0.74 V