HOx is a monoprotic weak acid with an acid dissociation constant of 4.78 × 10-5. H₂ Red² is a diprotic weak acid with acid dissociation constants of 5.52 × 10-4 and 3.39 × 10-8 . For the half reaction shown, calculate the standard reduction potential, Eº, at 25 °C. E = HOX(aq) + 2 e- 0.019 Incorrect → H₂ Red²-(aq) E' = 0.0500 V V

HOx is a monoprotic weak acid with an acid dissociation constant of 4.78 × 10-5. H₂ Red² is a diprotic weak acid with acid dissociation constants of 5.52 × 10-4 and 3.39 × 10-8 . For the half reaction shown, calculate the standard reduction potential, Eº, at 25 °C. E = HOX(aq) + 2 e- 0.019 Incorrect → H₂ Red²-(aq) E' = 0.0500 V V

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

› Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Ni²+] = 0.00100 M and [Au³+] = 0.834 M. Standard reduction potentials can be found in this table. 3 Ni(s) + 2 Au³ +(aq) — 3 Ni² †(aq) + 2 Au(s) E = 1.72 Incorrect V
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Agt H+ + Ag+le ←H₂(g) Standard reduction potentials: 2H+ + 2e H₂ Fº = 0 V → Ag E°=0.800 V
Consider the following cell reaction: Fe(s) + 2 H*(? M) –Fe²*(1.00 M) + H2(E)(1.00 atm) If the cell potential at 298 K is 0.261 volts, what is the pH of the hydrogen electrode? pH
1. Al(s) + Fe³+ (aq) →→ Al³+ (aq) + Fe(s) Half-reaction Standard Reduction Potential Fe³+ (aq) +2e-→ Fe(s) +0.771 V AP¹ (4) + 2e- Al(s)-1.660 V ->
HOx is a monoprotic weak acid with an acid dissociation constant of 3.00 × 10¯5. H₂Red²¯ is a diprotic weak acid with acid dissociation constants of 3.80 × 10−4 and 3.72 × 10-8. For the half reaction shown, calculate the standard reduction potential, Eº, at 25 °C. HOX(aq) + 2 e E = 0.00996 Incorrect H₂Red² (aq) E' = 0.0431 V V
Calculate K (both parts of the question)
Help on these two please
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Ag+ H+ Standard reduction potentials: 2H+ +2e¯ → H₂ Eº = 0 V Ag+ le - H₂(g) → Ag Eº=0.800 V
Consider these two entries from a fictional table of standard reduction potentials X+ (aq) + e - Y+ (aq) + e Y(s) O X and Y X and Y+ X and Y X and Y+ X(s) - E = 2.46 V Which pair of species will react under standard conditions at 25 °C? E = 1.25 V
A galvanic cell is made of a Ni2+/Ni half cell with [Ni²+] = 1.00 × 10-3 M and a Ag*/Ag half cell with [Ag*] = 5.00 x 10-2 M. Calculate the electromotive force of the cell at 25 °C. F= 96500 C/mol, R=8.314 J/mol.K The reduction potentials for the two half cells are: Ni2+ (aq) + 2e →Ni(s) E° = -0.24 V Ag*(aq) + e¯ →Ag(s) E° = +0.8 V %3D O a. 1.09 O b. 1.04 O c. 1.06 O d. 0.98 O e. 1.12
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG° for the following redox reaction. Round your answer to 3 significant digits. 6CI (aq)+2Cr0 (aq)+8H,0 (1) → 3Cl, (g)+2Cr(OH), (s) + 10OH (aq)
Calculate Eu for the following cell: Pt(s) | H₂(g) | H *(aq) || Pb2+ (aq) | PbSO4(s) | Pb(s) given the following standard reduction potentials. 2 H(aq) + 2e →→ H₂(g) PbSO4(s) + 2e →→ Pb(s) + SO42 (aq) O a. -0.712 V O b. +0.356 V O c. -0.356 V O d. +0.712 V O e. -0.178 V E° = 0.000 V E = -0.356 V