Consider these two entries from a fictional table of standard reduction potentials. X³+ + 3e → X(s) Eº = -1.75 V Y³+ + 3e¯ →Y(s) Eº = -0.34 V What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? V Eº cell

Consider these two entries from a fictional table of standard reduction potentials. X³+ + 3e → X(s) Eº = -1.75 V Y³+ + 3e¯ →Y(s) Eº = -0.34 V What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? V Eº cell

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 certain half-reaction has a standard reduction potential Ed=+0.45 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must ʼred provide at least 1.40 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 anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? O yes, there is a minimum. E red Ov 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. no minimum Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? yes, there is a maximum. = Ov red 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. no maximum
Standard tables of reduction potentials assume standard conditions, but many electrochemical cells operate under nonstandard conditions. An electrochemical cell is constructed based on the following balanced equation: Cu(s) + 2 Ag*(aq) → Cu2+(aq) + 2 Ag(s) Half-reactions with standard reduction potentials are given below. Cu2+(aq) + 2 e¯ → Cu(s); E° = 0.342 V Ag*(aq) + e¯ → Ag(s); E° = 0.800 V 5th attempt See Periodic Table O Se Calculate Ecell at 298 Kfor an electrochemical cell based on the overall redox reaction between Cu2+ and Ag if [Ag*] = 2.56 × 10 Mand [Cu2+] = 8.25 x 10-4 M. 3 V
A certain half-reaction has a standard reduction potential E=-0.22 V. An engineer proposes using this half-reaction at the cathode of a red galvanic cell that must provide at least 0.90 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. O-0 Is there a minimum standard reduction potential that the half-reaction used at O yes, there is a minimum. Ov %3D red 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 Iimit, check the "no" box. no minimum ? Is there a maximum standard reduction O yes, there is a maximum. = Dv potential that the half-reaction used at red 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. no maximum By using the…
A certain half-reaction has a standard reduction potential Eed=+0.45 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.40 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 anode of the cell. olo Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? yes, there is a minimum. E red Ov Ar 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. no minimum Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? E = Ov yes, there is a maximum. red 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. no maximum
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg²+] = 0.808 M and [Sn² +] = 0.0120 M. Use the standard reduction potentials in this table. Mg(s) + Sn² +(aq) — Mg²+(aq) + Sn(s)
A certain half-reaction has a standard reduction potential -0 red = = +0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.70 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. ロ→ロ 0 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a minimum. ☐v red 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. no minimum Ś ? 0 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a maximum. Ov red 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. no maximum E E = = X
The cell potential for the following galvanic cell is 1.15 V. The standard cell potential is 1.16 V. If [Au³+] = 0.50 M, what is the concentration of Cu2+? (R = 8.314 J/K mol, F = 96,500 C.mol-¹) 3Cu + 2Au3+→ 3℃u²+ + 2Au O 1.61 M O1.37 M O 258 M O 5.16 M
›Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn²+] = 0.867 M and [Fe²+] = 0.0100 M. Use the standard reduction potentials in this table. Zn(s) + Fe²+(aq) ⇒ Zn²¹(aq) + Fe(s) E = V
What is the cell potential (E0) for a galvanic cell formed from the following two half-reactions? Assume that the cell temperature is 45°C and the operating pressure is 0.06 atm. Fe2+(aq) + 2 e− ↔ Fe(s) ; [Fe2+] = 2.25 M E0 = −0.44 V Ag+(aq) + e− ↔ Ag(s) ; [Ag+] = 1.55 × 10−4 M E0 = 0.7994 V
A certain half-reaction has a standard reduction potential E == 'red - 1.02 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 0.80 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 anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode 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 cathode 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…
Pb(s) Determine which of the following statements about the cell shown are True or False. True The standard cell potential, o, equals 0.93 V. True As the reaction proceeds, the concentration of the silver ions decreases. False Cations move to the lead half-cell. True The mass of the silver electrode is increasing. True The silver half-cell is the cathode. False The cell, as represented by the line notation, is a voltaic cell. True True The lead electrode is the anode. Electrons are spontaneously produced in the silver half-cell. salt bridge Ag(s) Pb+2 So Pb2+2e → Pb(s) AS NO3 E--0.13V Ag + le → Ag(s) E° - +0.80V Pb(s) Pb2+ (1M) || Ag+ (1M) | Ag(s)
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