Answered: The cell potential E for the cell Pt(s)…

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...

See similar textbooks

Similar questions

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).
Calculate ΔG° for the redox reaction represented by the cell diagram Pt(s) | Cl2(g, 1 atm) || ZnCl2(aq, 1 M) | Zn(s).
+|| 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
4. The standard electromotive force of the cell Pt(s) H2(g)|HCl(aq)|AgCl(s)|Ag(s) has been determined from 0°C to 90°C, and the data were found to fit the expression E*/V = 0.237-4.856 × 10-4T(°C) - 3.421 × 10-T²(°C) + 5.869 × 10-ºT³ (°C) Calculate the equilibrium constant, the standard reaction Gibbs energy, entropy and enthalpy for the cell reaction at 25°C. F = 96485 C mol-¹ AgCl(s) + H2(g) → Ag(s) + HCl(aq)
Predict the products of this organic reaction: H₂O* + H NH2 ? • Draw all the reasonable products in the drawing area below. If there are no products, because no reaction will occur, check the box under the drawing area. Include both major and minor products, if some of the products will be more common than others. • Be sure to use wedge and dash bonds if you need to distinguish between enantiomers.
The battery Pt|H2(1 atm)|HBr(aq)|AgBr(s)|Ag| pt At 25°C, with HBr molality 0.1000 mol/kg has ε = 0.200 V. Find the coefficient of mean ionic activity of HBr(aq) at this molality.Write the overall reaction of the cell and indicate the species that is oxidized and the one that is reduce.
Calculate the standard potential of the cell Ag(s)|AgNO3(aq)||Cu(NO3)2(aq)|Cu(s) and the standard Gibbs energy and enthalpy of the cell reaction at 25 °C. (ii) Estimate the value of A,GE at 35 °C.
3. At 298 K, the EMF of the cell shown below is +0.84 V. Pt(s)|Fe²*(aq, a = 1), Fe³*(aq, 1)|| Ce**(aq, a = 1), Ce³*(aq, a = 1)|Pt(s) a = (i) Define what is meant by the standard EMF of the cell. (ii) Write down the cell reaction and the Nernst equation for the cell. (iii) Calculate the equilibrium constant for the cell reaction at 298 K.