What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions?E =[H+] = 0.33 MPH₂ = 3.6 atmT = 298 K

Here's how to find the potential of the SHE under these conditions:Standard Hydrogen Electrode…

Answered: What would the potential of a standard…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 3QRT

See similar textbooks

Similar questions

The standard potential, E, for the reaction of Zn(s) and Cl2(g) is +2.12 V. What is the standard free energy change, rG, for the reaction?
What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions? [H+]=0.67 M?H2=2.7 atm?=298 K ?=
What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions?
What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions? [H+] = 0.50 M PH₂ = 3.9 atm E = T = 298 K
What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions? [H+] = 0.83 M PH₂ = 3.1 atm E = T = 298 K V
For the cell below, the standard potential is Eocell = 1.62 V ( F =96500 C/mole e-)( 1VC=1J) Mg(s) | Mg2+ (1M) || Zn 2+ (1M) | Zn (s)Calculate ΔGo for the cell at standard conditions in kJ. Select one: a. -1.62 kJ b. -313 kJ c. -3.13 x 105 kJ d. -156 kJ
https://www.google.com/url?sa=t&source=web&rct=j&url=http:calculate the electrode potentials of the following half cells: HCL (3.50M) | H2 (0.950atm), Pt.
Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E° (V) 2H2 O(1) + 2e = H2 (g) + 20H¯ (ag) -0.83 Cu?+ (aq) + e¯ = Cu*(aq) 0.16 Cu?+ (ag) + 2e Cu(s) 0.34 O2 (g) + 4H† (aq) + 4e¯ – 2H2O(1) 1.23 Cl2 (g) + 2e 2C1¯ (aq) F2 (g) + 2e = 2F¯(aq) 1.36 2.87 Write the overall reactions that you would expect to happen when the following solutions are electrolyzed: (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. Add H,0, H*, or OH to any side of the reaction if it is needed.) a. Aqueous CuCl2. + + + b. Aqueous Cu(NO3)2. The nitrate ion is not oxidized. + + 1
Consider the electrolysis reactions cathode Cu²+ (aq, 0.253 M) + 2e = Cu(s) anode H₂O(1) whose standard reduction potentials can be found in this table. Calculate the voltage needed to drive the net reaction if the current is negligible. Ecell = -0.858 Ecell = 1 O₂(g, 1 bar) + 2 H+ (aq, 0.202 M) + 2 e¯ 2 The cell has a resistance of 57.0 2 and a current of 4.73 mA when the cathode overpotential is 0.232 V and the anode overpotential is 0.054 V. Calculate the voltage needed to overcome these effects and drive the net reaction. Incorrect V V
11
After plotting the cell potential (Ecell) measured at 298 K on the y-axis versus the natural logarithm of the equilibrium quotient (ln(Q)) on the x-axis, the line of best fit is represented by the equation: y = (-0.00855)x + 1.674 What is the number of electrons transfered in the balanced equation of the redox reaction? Report your answer as a whole number. R = 8.31 V/mol·K F = 96500 C/mol
28 Calculate standard electrode potential and Gibbs free energy of the cell: Ga | Ga³+ || Ag* | Ag a. b. C. d. 1.23 V; -285 kJ 1.43 V; -365 kJ 1.33 V; -385 kJ 1.53 V; -265 kJ

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions? E = [H+] = 0.33 M PH₂ = 3.6 atm T = 298 K