Voltaic Cells Under Non-Standard Conditions Step 1-2 Identify the reduction half-reaction. E° for this reaction is E°cathode- Step 3-4 Identify the oxidation half-reaction. E° for this reaction is E°anode- Step 5 Determine the number of electrons transferred in the process. Step 6 Calculate E° cell- E°cell = E°cathode - E°anode Step 7 Identify the form of the reaction quotient, Q. This is of the same form as the equilibrium constant expression for the system being studied. Step 8 Calculate the numerical value of Q. Step 9 Use the Nernst equation to calculate the cell potential. Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.025 M at 25 °C. 2 Fe (aq) + H,O2(aq) + 2 H¨(aq) → 2 Fe¯(aq) + 2 H,O(t) Acidic Solution Standard Electrode Potential, E(volts)

Voltaic Cells Under Non-Standard Conditions Step 1-2 Identify the reduction half-reaction. E° for this reaction is E°cathode- Step 3-4 Identify the oxidation half-reaction. E° for this reaction is E°anode- Step 5 Determine the number of electrons transferred in the process. Step 6 Calculate E° cell- E°cell = E°cathode - E°anode Step 7 Identify the form of the reaction quotient, Q. This is of the same form as the equilibrium constant expression for the system being studied. Step 8 Calculate the numerical value of Q. Step 9 Use the Nernst equation to calculate the cell potential. Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.025 M at 25 °C. 2 Fe (aq) + H,O2(aq) + 2 H¨(aq) → 2 Fe¯(aq) + 2 H,O(t) Acidic Solution Standard Electrode Potential, E(volts)

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 utilizes the following reaction: 4 Fe2+1aq2 + O21g2 + 4 H+1aq2 ¡ 4 Fe3+1aq2 + 2 H2O1l2 What is the emf of this cell when 3Fe2+4 = 1.3 M, 3Fe3+4= 0.010 M, PO2 = 0.50 atm, and the pH of the solution in the cathode half-cell is 3.50?
Consider the following reaction and their reduction potential values: Cu+ + Ni2+ —> Cu2+ + Ni (Format: half reaction, E⁰) Cu2+ + e- —> Cu+, 0.15 V Ni2+ + 2e- —> Ni, -0.25 V What is the overall cell potential and is the overall reaction spontaneous?
The correctly-calculated value for Ecell in the previous question is lower than the standard cell potential (Eºcell) that you derived from the two half-reactions. Which of the following best explains why the potential for the operating cell was lower than the standard potential? The concentration of the product was much lower than that of reactants The redox reaction is nonspontaneous The redox reaction is spontaneous The concentrations of reactants was much lower than that of the product The stoichiometric coefficient on solid aluminum in the balanced equation is "2".
Study each overall cell reaction. Identify and write the half-reaction that occurs in the anode and in the cathode. Calculate the standard cell potential and describe the reaction as spontaneous or non-spontaneous. Li(s) + F2(g) → Li+(aq) + 2F-(aq)
Set up the Nernst equation in the oxidation half-cell reaction. Zn2+ + 2e- ⇆ Zn E° = -0.762 V
Mercuric oxide dry-cell batteries are often used where a flat discharge voltage and long life are required, such as in watches and cameras. The two half-cell reactions that occur in the battery are HgO1s2 + H2O1l2 + 2 e- ¡ Hg1l2 + 2 OH-1aq2 Zn1s2 + 2 OH-1aq2 ¡ ZnO1s2 + H2O1l2 + 2 e- Why is the potential of the anode reaction diferent than would be expected if the reaction occurred in an acidic medium?
Enter your answer in the provided box. What is the emf of a cell consisting of a Pb2+ / Pb half-cell and a Pt / H / H₂ half-cell if [Pb²+] = 0.64 M, [H] = 0.018 M and PH₂ = 1.0 atm ? V
The Zn/Zn2 + electrode has a standard electrode potential of E° = -0.76 V. How does the relative potential energy of an electron at the Zn/Zn2 + electrode compare to the potential energy of an electron at the standard hydrogen electrode?a) An electron at the Zn/Zn2 + electrode has a higher potential energy than an electron at the standard hydrogen electrode.b) An electron at the Zn/Zn2 + electrode has a lower potential energy than an electron at the standard hydrogen electrode.c) An electron at the Zn/Zn2 + electrode has the same potential energy as an electron at the standard hydrogen electrode.d) Nothing can be concluded about the relative potential energy of an electron at the standard electrode potential.
A voltaic cell is set up at 25 °C with the following halfcells:Al/Al3+ (0.001 M) and Ni/Ni2+ (0.50 M)Write an equation for the reaction that occurs when the cell generates an electric current and determine the cell potential.[ENi2+/Ni = – 0.25 V and EAl3+/Al= – 1.66 V]
What is the value of n, the number of electrons transferred during the reaction? H,O2 reduced at cathode Fe2* oxidized at anode Submit What is the value of E° for the reaction, in volts? H2O2 reduced at cathode Fe2* oxidized at anode 2 e transferred V Submit
If a voltaic cell is created between a Sr2+/Sr electrode and a In3+/In electrode
Consider the cell described below. Al | Al³+ (1.00 M) || Pb²+ (1.00 M) | Pb Calculate the cell potential after the reaction has operated long enough for the [Al³+] to have changed by 0.45 mol/L. (Assume T= 25°C.) V Need Help? Read It Watch It