My Home OWLV2 | Online. HBO M: [Roview Topics] [References] Use the References to access important values if needed for this question. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg* concentration is 1.31 M and the Mn²* concentration is 6.85×10 M ? Hg²"(aq) + Mn(s)→ Hg(l) + Mn²*(aq) Answer: The cell reaction as written above is spontaneous for the concentrations given:

My Home OWLV2 | Online. HBO M: [Roview Topics] [References] Use the References to access important values if needed for this question. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg* concentration is 1.31 M and the Mn²* concentration is 6.85×10 M ? Hg²"(aq) + Mn(s)→ Hg(l) + Mn²*(aq) Answer: The cell reaction as written above is spontaneous for the concentrations given:

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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consider these two entries from a ficitional table of standard reduction potentials. (see image) what is the standard potential of a galvanic (voltaic) cell? give answer to 3 sig figs inputting only the numeric value, assuming a measurement of V
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Which of the following is the correct cell notation for an electrochemical cell consisting of an anode where Al(s) is oxidized 3+ 2+ to Al°" (aq) and a cathode where Zn-"(aq) is reduced to Zn(s). (Assume all aqueous solutions have a concentration of 1 mol/L) O AI$* (aq, 1 M) | AI(s) || Zn(s) | Zn²*(aq, 1 M) O zn(s) | Zn²*(aq, 1 M) || Al³+(aq, 1 M)| AI(s) O Al(s) | A13*(aq, I M) || Zn²*(aq, 1 M) I Zn(s) O Zn2*(aq, 1 M) | Zn(s) || AI(s) | AI³*(aq, 1 M) O Al(s) I Zn(s) || AI³*(aq, 1 M) | Zn²*(aq)
Use the References to access important values if needed for this question. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag* concentration is 2.61×104 M and the Zn2+ concentration is 1.08 M ? 2Ag*(aq) + Zn(s) 2Ag(s) + Zn²*(aq) Visited V The cell reaction as written above is spontaneous for the concentrations given:
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CHEMWORK An electrolytic cell is set up to plate Zr(s) from a solution containing Zr"(ag). A current of 4.65 amps is run through this solution for 8.28 hours. The mass of Zr(s) plated out during this process is g Zr Remember Faraday's constant is 96,485 C/mol e".
For the following electrolyte-concentration cell consisting of two cells back to back by electrodes, What is the suitable Nernst Equation at? 25 degree celcius? Pt;H2,HCl(a1), Ag (s),Ag/Ag, AgCl(s), HCl (a2), H2;Pt
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Consider the cell described below. Al | Al³+ (1.00 M) || Pb²+ (1.00 M) | Pb Calculate the cell potential after the reaction has operated long enough for the [A13+] to have changed by 0.46 mol/L. (Assume T= 25°C.) V Need Help? Read It Supporting Materials Periodic Table Watch It Constants & Factors Supplemental Data
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Enter electrons as e". A voltaic cell is constructed in which the anode is a Mn Mn2+ half cell and the cathode is a CI|Cl, half cell. The half- cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: In the external circuit, electrons migrate v the Mn|Mn2+ electrode | v the Cl|Cl, electrode. In the salt bridge, anions migrate v the Cl|Cl2 compartment v the Mn|Mn²+ compartment. +
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