Consider the following data for the cell: Pt(s) |H2(g)| HBr(aq,b)|AgBr(s) |Ag(s),taking place at 25°C, and with the hydrogen gas at 1 bar.b/(10-4 b°) 4.0428.44437.19Ecell N0.473810.43636 0.36173Determine the standard cell potential.

### Step 1: Use Nernst Equation to Determine Standard Cell PotentialThe cell potential (E_cell) at…

Answered: Consider the following data for the…

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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The net ionic cell reaction for the 'Bunsen cell ' is Zn(s) +2 NO3-(aq) + 4 H+(aq) → Zn2+(aq) + 2 H2O(I) + 2 NO2(g). Thestandard cell potential at 25 °C is -0.04 V. Calculate the electricalwork that can be done by the cell.
For the reaction 2Co3+(aq)+2Cl(aq)->2Co2+(aq)+Cl2(g). Excell=0.46 V what is the cell potential at 25 °C if the concentrations are [Co3+]=0.168mol L-1, [Co2+]=0.574mol L-1, and [CI-]=2.30\times 10-2mol L-1 and the pressure of Cl2 is PC12=9.70bar ?
The standard cell potential for the reactions Sn(s) + CuSO4(aq) → Cu(s) + SnSO4(aq) at 25 °C exceeds +0.20V
A galvanic cell Mn(s)|Mn2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Mn electrode that weighs 34.9 g and a Pb electrode immersed in 532 mL of 1.00 M Pb2+(ag) solution. A steady current of 0.0519 A is drawn from the cell as the electrons move from the Mn electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Pb electrode gained when the cell is completely discharged? g (d) What is the concentration of the Pb2+(aq) when the cell is completely discharged? (Assume that the limiting reactant is 100% reacted.) M
Like equilibrium constants, E values are temperature dependent. At 80°C, E for the cell cell cell diagram shown is 0.18 V. Pt | H₂(g) | HCl(aq) || AgCl(s) | Ag(s) The corresponding cell reaction is H₂(g) + 2AgCl(s) + 2Ag(s) + 2H¹ (aq) + 2C1 (aq) Calculate the equilibrium constant for this reaction at 80°C. x 10 (Enter your answer in scientific notation).
Gibbs energy change, A-G", is related to cell potential, E. by the equation A,G nFE Part A where n is the number of moles of electrons transferred and F = 96 500 C mo]1 is the Faraday's constant. Calculate the standard Gibbs energy change at 25 °C for the following reaction: Mg(s) + Fe" (ag) »Mg+ (ag) + Fe(s) Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? kJ A,G = 380.20 mol- Submit Previous Answers
+|| Σ D. For the cell shown, the measured cell potential, Ecell, is-0.3621 V at 25 °C. Pt(s) | H, (g, 0.853 atm) | H* (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2H*(aq) + 2 e¯ – H, (g) A 00'0 = 07 24, Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V %3D Calculate the Ht concentration. M. = [,H] 10:23 AM M. 11/9/2021 7734 F4 F5 F7 F8 F10 F11 F12 PrtScr Insert Delete Eゴ #3 Backspace 2$ ) 4. 5. 9. 7. R } 1 Enter F. K. H. Sh

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Consider the following data for the cell: Pt(s) |H2(g)| HBr(aq,b)|AgBr(s) |Ag(s), taking place at 25°C, and with the hydrogen gas at 1 bar. b/(10-4 b°) 4.042 8.444 37.19 Ecell N 0.47381 0.43636 0.36173 Determine the standard cell potential.