TUTOR Voltaic Cells Under Non-Standard ConditionsCalculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.033 M at 25 °C.2 Fe2"(aq) + H2O2(aq) + 2 H"(aq) → 2 Fe"(aq) + 2 H,O(E)Acidic SolutionStandard Electrode Potential, E°(volts)H2O2(aq) + 2 H'(aq) + 2 e →2 H2O(E)Au*(aq) + e – Au(s)Au3 (aq) + 3 e →Au(s)+1.77+1.68+1.50Br2(t) + 2 e -→2 Br(aq)+1.08NO3 (aq) + 4 H'(aq) + 3 e → NO(g) + 2 H20+0.96Ag*(aq) + e –Ag(s)Hgz2"(aq) + 2 e →2 Hg(8)Fe (aq) + e--→ Fe²"(aq)Cu2"(aq) + 2 e → Cu(s)+0.80+0.789+0.77+0.337HgzClz(s) + 2 e →2 Hg(t) + 2 C(aq)Sn**(aq) + 2e → Sn2*(aq)+0.27+0.152 H*(aq) + 2 e →H2(g)Pb?*(aq) + 2 e → Pb(s)0.00-0.126Sn2*(aq) + 2 e → Sn(s)Ni2"(aq) + 2 e → Ni(s)Cd2*(aq) + 2 e → Cd(s)Cr**(aq) + e – Cr**(aq)Fe2"(aq) + 2 e → Fe(s)Zn2"(aq) + 2 e → Zn(s)Cr2*( aq) + 2 e → Cr(s)A* (aq) + 3 eMg2*(aq) + 2 e → Mg(s)-0.14-0.25-0.40-0.408-0.44-0.763-0.91Al(s)-1.66-2.37 Cr²*( aq) + 2 e – Cr(s)Aß* (aq) + 3 e – Al(s)Mg2 (aq) + 2 e --0.91-1.66→ Mg(s)-2.37VSubmitShow Approach Hide Tutor StepsTUTOR STEPWhat is the numerical value of Q?H2O2 reduced at cathodeFe2+ oxidized at anode2 e transferredE° = 1.00 V[Fe**}°Q[Fe?+]*[H2O2][H+]°

In the given question we have to calculate the cell potential developed by a voltaic cell.

Answered: TUTOR Voltaic Cells Under Non-Standard…

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

A voltaic cell is being constructed from an Al/A|^ 3+ electrode and a Sn/Sn^ 2+ electrodeWhen constructed properly and the circuit is closed, the tin electrode is observed to gain mass and the overall cell potential to be 1.52V. Which of the following chemical reactions takes place at the cathode? Al3+(aq) + 3e- → Al(s) Sn(s) → Sn2+(aq) + 2e- Sn2+(aq) + 2e- → Sn(s) Al(s) → Al3+(aq) + 3e- Based on the overall reaction taking place across the voltaic cell, how many moles of electrons are involved? When electrons are flowing in the cell, which electrode gains mass? True or false: If an aluminum electrode is set to be part of a voltaic cell that also involves a standard hydrogen electrode (SHE), the aluminum electrode would be the anode.
4 Consider the voltaic cell: Sn(s) | Sn*2(aq) II Fe*3(aq) | Fe*2(aq) a) Write the overall cell reaction. b) Calculate the standard cell potential at 25°C. c) Calculate the change in free-energy of the reaction at 25°C d) What is the maximum work you can obtain from 25.0 g of nickel? e) What is the value of the equilibrium constant of the reaction? f) Which is the stronger oxidizing agent: Sn*2 or Fe*3? Explain
What is the potential of the reaction?
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential CrO2−4 (aq)+4H2O(l)+3e−→ CrOH3(s)+5OH−(aq) =E0red−0.13V Cl2(g)+2e−→ 2Cl−(aq) =E0red+1.359V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of significant digits. V
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
A certain metal è forms a soluble sulfate salt ₂(so). Suppose the left half cell of a galvanic cell apparatus is filled with a 5.00 M solution of M₂(SO4)3 and the right half cell with a 250. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. Which electrode will be positive? O left Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. O right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 x10 X
Consider the voltaic cell: Mg Mg2+ (1.0 M)||H* (1.0 M)|H₂ (1 atm)|Pt(s) Which of the following changes will cause a decrease in the cell voltage? increase the pressure of H₂ at 2.0 atm decrease the mass of the Mg electrode O decrease the concentration of Mg2+ ion lower the pH of the catholyte
A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction: Cr(s) + 3 Ag*(aq) → Cr³*(aq) + 3 Ag(s) Which of the multiple choices correctly describes how the cell emf changes when a change is made to the cell? Ca) Adding water to the anode compartment makes the cell emf less positive. C b) Increasing the size of the silver electrode makes the cell emf stay the same. C C) Adding a solution of 1.0 M AGNO, to the cathode compartment makes the cell emf more negative. C d) Adding Na,s to the anode compartment to precipitate chromium sulfide makes the cell emf less positive. Ce) Adding a solution of 5 M Ag* to the cathode compartment makes the cell emf stay the same.
Consider these two entries from a fictional table of standard reduction potentials. X3++3e−⟶X(s)?o=−1.63 V Y3++3e−⟶Y(s)?o=−0.41 V What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? ?ocell= V
write the answers properly
Calculate the standard cell potential (E°cell) of a galvanic cell made of lead and cadmium. Then determine the non-standard cell potential (Ecell) if the molarity of the cadmium solution was 0.20 M, and the molarity of the lead solution was 0.10 M. The temperature of the cell is 300 K. Cd2+(aq) + 2e– → Cd(s) E° = –0.403 V Pb2+(aq) + 2e– → Pb(s) E° = –0.126 V E°cell = ______________ Ecell = ______________
What will be the products of the electrolysis of an 1-M aqueous aluminum chloride (AICI3) solution at 25 °C? (The electrodes themselves are platinum.) (Use the standard electrode potentials table in your online textbook's Appendix to help you answer the question.) No products will be produced. H₂(8) +20H (aq) + Cl₂(g) 4Al(s) + 30₂(g) + 12H*(aq) O 2H₂(g) + 4H₂O(l) + O₂(g) O2Al(s) + 3Cl2(g)

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

TUTOR Voltaic Cells Under Non-Standard Conditions Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.033 M at 25 °C. 2 Fe2“(aq) + H2O2(aq) + 2 H¨(aq) → 2 Fe*(aq) + 2 H20(()