26 Consider the standard electrode potentials of the following reactions. Cr3+(aq) + 3e--Cr(s) Cd2+(aq) + 2e-- Cd(s) What is the approximate value of the electrical energy(E) in kilojoules? The value of Faraday's constant is 96,500 J/v.mol.e-. -0.75 V -0.40 V 2Cr + 3Cd 2Cr, + 3Cd) O 200 KJ O 201 KJ O 202 KJ O 203 KJ

26 Consider the standard electrode potentials of the following reactions. Cr3+(aq) + 3e--Cr(s) Cd2+(aq) + 2e-- Cd(s) What is the approximate value of the electrical energy(E) in kilojoules? The value of Faraday's constant is 96,500 J/v.mol.e-. -0.75 V -0.40 V 2Cr + 3Cd 2Cr, + 3Cd) O 200 KJ O 201 KJ O 202 KJ O 203 KJ

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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14.
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Cr3+(aq) → Cr(s)Zn2+(aq) → Zn(s) a. What will be the overall balanced reaction if you want to make a galvanic cell? b. What is the standard cell potential, E°cell?(use values from the provided SRP table) c. If the initial concentrations are [Cr3+]=0.010 M and [Zn2+]=0.0085 M, what is Ecell?
For the galvanic cell: Zn(s) + 2TI* (aq) → 2TI(s) + Zn2*(aq) E°cell = 0.42 V If the standard reduction potential for Zn-*(aq) + 2e Zn(s) Ered = -076 V what is the standard reduction potential for TI*(aq) + eTI(s) E°red = ? V O -0.34 V O -0.17 V +0.17 V +0.34 V
Calculate the concentration of an unknown solution in a concentration cell. A concentration cell consisting of two hydrogen electrodes (P H2- latm), where the cathode is a standard hydrogen electrode and the anode solution has an unknown pH, has a cell voltage of 0.193 V. What is the pH in the unknown solution? Assume the temperature of the solutions is 298 K. !! pH =
Based on the standard reduction potentials in Table 2, which of the following metals could provide cathodic protection to iron: Al, Cu, Ni, Zn?
Consider the following standard reduction potentials, Al3+(aq) + 3 e- → Al(s) E° = -1.66 V I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V Under standard conditions, A) Al3+(aq) is a stronger oxidizing agent than I2(s), and I-(aq) is a stronger reducing agent than Al(s). B) I2(s) is a stronger oxidizing agent than Al3+(aq), and Al(s) is a stronger reducing agent than I-(aq). C) Al(s) is a stronger oxidizing agent than I-(aq), and Al3+(aq) is a stronger reducing agent than I2(s). D) I-(aq) is a stronger oxidizing agent than Al(s), and I2(s) is a stronger reducing agent than Al3+(aq).
Given the following2AgCl(s) +X(s) → 2Ag(s) + 2Cl-(aq) + X2+(aq) E°cell = 0.73 V and AgCl(s) → Ag(s) + Cl-(aq) E°= 0.222 V What is the standard reduction potential for X2+(aq)?
Calculate the K and AG for the following reaction at 25 °C: Zn(s) + CuSO₂(aq) → ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Bo = Part 2 of 2 AGⓇ ☐x10 = Round your answer to 4 significant digits. X kJ mol 0x10 3 X Ś
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Cl₂ (g) + 2 e →2 Cl(aq) O2(g) + 4 H3O+ (aq) + 4 e 6 H₂O(1) 1.360 1.229 2 H2O(l) + 2e Al3+ (aq) + 3 e → Al (s) H2(g) + 2 OH(aq) -0.828 -1.660 A 0.114 M neutral aqueous AlCl3 solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials. Half-reaction at anode: + + + + Half-reaction at cathode: + + + + (b) What is the expected decomposition potential?
Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = V
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