In a galvanic cell based on the oxidation-reduction reaction, Zn + 2 Ag+ = Zn²+ + Ag, with 298°° = +0.0378 V, the anode would bethe wire connecting the two half-cells that comprise the cellthe electrode containing Zn metalthe positive end of the salt bridge connecting the half-cellsthe negative end of the salt bridge connecting the half-cellsthe electrode containing Ag metalO O O O

Given redox reaction is Zn + 2 Ag+ ⇌Zn2+ + 2 Ag, ε2980 = +0.0378 V The anode in the above redox…

In a galvanic cell based on the oxidation-reduction reaction, Zn + 2 Ag+ Zn²+ + Ag, with 298° = +0.0378 V, the anode would be the wire connecting the two half-cells that comprise the cell O the electrode containing Zn metal O the positive end of the salt bridge connecting the half-cells O the negative end of the salt bridge connecting the half-cells O the electrode containing Ag metal

In a galvanic cell based on the oxidation-reduction reaction, Zn + 2 Ag+ Zn²+ + Ag, with 298° = +0.0378 V, the anode would be the wire connecting the two half-cells that comprise the cell O the electrode containing Zn metal O the positive end of the salt bridge connecting the half-cells O the negative end of the salt bridge connecting the half-cells O the electrode containing Ag metal

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

The two half cells that make up a battery are shown below with their reduction potentials: Br2(aq) + 2e → 2B1¯(aq); E= 1.07 V Cu²+(aq) + e – Cu*(aq); E= 0.16 V What is the equation for the galvanic cell made with these two half equations? Oa. 2Cu*(aq) + Br2(aq) – 2Cu2+(aq) + 2Br (aq) Ob. 2Cu2*(aq) + Br2(aq) → 2Cu*(aq) + 2Br"(aq) Oc. 2Cu*(aq) + 2Br (aq) – 2Cu²* (aq) + Br2(aq) Od. 2Cu2*(aq) + 2B1°(aq) → 2Cu*(aq) + Br2(aq) Oe. None of the other options
A galvanic (voltaic) cell consists of an inert platinum clectrode in a solution containing 1.0 M tin(IV) ion and 1.0M tin(II) ion, and another inert platinum clectrode in a solution containing 1.0 M iron(III) ion and 1.0M iron(II) ion, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Standard reduction potentials can be found in the standard reduction potentials table. E: cell V
A chemist designs a galvanic cell from the following two half-reactions NO3(aq) + 4H+ (aq) + 3e → NO(g) + EO red = +0.96 V 2H₂0 (1) Cu2+ (aq) + e → Cut (aq) Ere red= +0.153 V The standard cell potential for this galvanic cell is [Select] The standard free energy for this galvanic cell is AG [Select] The equilibrium constant (K) for this galvanic cell is [Select] V..
Consider a galvanic electrochemical cell constructed using Cr/Cr³+ and Zn/Zn²+ at 25 °C. The following half-reactions are provided for each metal: Cr³+(aq) + 3 e →→ Cr(s) E°red = -0.744 V Zn²+ (aq) + 2 e →→ Zn(s) Eºred = -0.763 V Write the balanced equation for the overall reaction in acidic solution. 3 Zn(s) + 2 Cr³+ (aq) → 3 Zn²+(aq) + 2 Cr (s) 1 1 + 4- Reset 2 H₂O+ 0 3_ ( ) 3 03 04 4 H H+ 5 5 11 Zn 6 6 ²+ 7 07 (s) H₂O ● 3+ (1) 8 9 0 e 4+ x H₂O 9 (g) (aq) □o Cr Delete
A galvanic cell is constructed from a silver half-cell and a copper half-cell. The copper half-cell contains 0.10M Cu(NO3)2 and the concentration of silver ions in the other half-cell is unknown. If the silver electrode is the cathode and the cell emf is measured and found to be 0.10 v at 25oC, what is the Ag+ ion concentration?
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
red A certain half-reaction has a standard reduction potential E = +0.16 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.30 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used…
Suppose a galvanic cell is established using the following cell reaction, Cu(s) + 2Ag+(0.100 M) Cu2+(0.200 M) + 2Ag(s) Each compartment of the cell contains 125 mL of solution. How long would it take at a constant current of 0.10 A for the potential to drop by 10%? By how many grams will the total mass of the two electrodes change during this time period? The change in mass of the copper electrode = g The change in mass of the silver electrode = g The total change in mass of the two electrodes =
Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag^+(aq)+e^-→Ag(s) What mass of silver plates onto the cathode when a current of 7.9 A flows through the cell for 73 min ?
A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of copper in a 1.0 M copper(I) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. E cell || = V
. Consider the oxidation-reduction reaction Mg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s) Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Cu (aq)+e Cu (aq) = +0.153 V NO3 (aq)+4 H (aq)+3e NO(g)+2 H,O(1) E=+0.96 V red 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 O Yes Explanation Check . Terms of Us 02022 McGraw Hill LLC. All Riahts Reserved. MAR étv 16