4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: 3 Mn +2 Al³+→ 2 Al + 3 Mn²+ (b) What is n? (c) What is AG for this reaction at 25°? (d) What is the equilibrium constant for this reaction at 25°?

4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: 3 Mn +2 Al³+→ 2 Al + 3 Mn²+ (b) What is n? (c) What is AG for this reaction at 25°? (d) What is the equilibrium constant for this reaction at 25°?

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

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.
Which statement is true regarding the galvanic cell in which an electric current is being produced? Zn²* + 2e¯→Zn E° = -0.76 V Cu2* + 2e¯→Cu E° = +0.34 V V Salt Bridge Zn - Cu ZnSO«(aq) CUSO:(aq) (A) Oxidation occurs at the copper electrode. (B) The mass of the copper electrode is increasing. (C) Zinc ions are produced at the copper electrode. (D) Copper ions are produced at the copper electrode.
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20.0oC is measured as +1.03 V. Calculate the experimental equilibrium constant, K, for the reaction (Equation 6). Your answer should have 3 sig figs. Use your answer from question 4. Question 4 + answer: Calculate the experimental standard state free energy change, ΔGo, for the reaction: ANSWER: -1.99e5 Equation 6 Attached:
The following figure represents an electrochemical cell at 25.00C with aqueous solutions that behave ideally: (a) Represent the electrochemical cell using cell notation, by taking into account that concentrations of the ZnSO4 and CuSO4 solutions are 0.25 M and 0.35 M, respectively. (b) Calculate the standard potential of the cell, E0cell. (c) Calculate the potential of the cell, Ecell. (d)Calculate DG0 (e)Calculate DG (f)Calculate the equilibrium constant, K.
19. (a) Write a balanced equation for the reaction that occurs in a car battery when the ignition key is turned on. (b) Suppose that constant current of 450 A flowing through the engine for at least 10.0 seconds is needed to start a pick-up truck. How many grams of lead are consumed during this time? (c) If the battery operates at 12 V of potential, how much energy (in kJ) is produced?
A galvanic cell is constructed as follows. One half-cell consists of a platinum wire immersed in a solution containing 1.00 M Sn2+ and 1.00 M Sn4+. The other half-cell has a thallium rod immersed in a solution of 1.00 M Tl+. What is the equilibrium constant at 25° C?(Eo= Tl+ / Tl = −0.34 V.)? What is the cell voltage if the Tl+ concentration is increased 6−fold?
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20.0oC is measured as +1.03 V. Calculate the experimental equilibrium constant, K, for the reaction Your answer should have 3 sig figs.
Complete the following, providing written work for each part in order to receive credit: (a) Use shorthand notation to describe an electrochemical cell that contains gold (Au) and chromium (Cr) electrodes.(b) Determine which electrode will function as the anode and which will function as the cathode when the cell runs under standard conditions.(c) Calculate ΔG° for the cell under standard conditions. Enter your value for ΔG° in kJ below; do not actually enter the units.