The reduction half-reaction for a Hall-Heroult electrolytic cell is represented by the following equation. Al³+ + 3e → Al If a current of 10.0A is applied for 5.00 h to the Hall - Heroult electrolytic cell, then the amount of electrons transferred is 5.60 mol 1.87 mol 6.22 x 10-¹ mol 5.18 x 104 mol

The reduction half-reaction for a Hall-Heroult electrolytic cell is represented by the following equation. Al³+ + 3e → Al If a current of 10.0A is applied for 5.00 h to the Hall - Heroult electrolytic cell, then the amount of electrons transferred is 5.60 mol 1.87 mol 6.22 x 10-¹ mol 5.18 x 104 mol

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

3) The standard potential for the following galvanic cell is +0.90 V: 3 Cu2+ (aq) + 2 Ga(s) ⇒ 3 Cu(s) + 2 Ga³+ (aq) Given that the standard reduction potential for the Cu2+/Cu half-cell is +0.34 V, what is the standard reduction potential for the Ga3+/Ga half-cell?
A chemist designs a galvanic cell that uses these two half-reactions: 3+ 2+ Fe (aq)+e → Fe (aq) Cro (aq) + 4H₂O(1)+3e¯ Cr(OH)3(s)+5 OH(aq) 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 half-reaction spontaneous as written. 0 standard reduction potential Ed=+0.771 V 'red E 'red = -0.13 V ロ→ロ × x10 5
Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction at standard conditions. Write the line representations for the Galvanic Cells, indicating the anode and cathode. NO3- + H+ + Zn -> Zn2+ + NO2 + H2O
A certain half-reaction has a standard reduction potential E = 'red +0.09 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. 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 used…
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 silver in a 1.0 M silver 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. Eell = V
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2+ 2 Cr³+ (aq) + 3Ca (s) → 2Cr (s) + 3 Ca²+ (aq) 3+ 2+ Suppose the cell is prepared with 2.68 M Cr in one half-cell and 7.85 M Ca in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 ロ・ロ × μ 0|0 Ś
At 298 K a cell reaction has a standard cell potential of+0.17 V. The equilibrium constant for the reaction is5.5 x 105. What is the value of n for the reaction?
Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction at standard conditions. Write the line representations for the Galvanic Cells, indicating the anode and cathode. MnO4- + H+ + Ce3+ -> Ce4+ + Mn2+ + H2O
A certain half-reaction has a standard reduction potential =E0red−0.34V . An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.60V 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. yes, there is a minimum. =E0red V no minimum 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. yes, there is a…
+ The Nernst Equation The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation i E=E 2.303 RT log10 Q where E is the potential in volts, Eo is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, 12 is the number of moles of electrons transferred, Fis the Faraday constant, and is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E = ED (0.0592) log Q The reaction quotient has the usual form Q [products [reactants A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. Part A For the reaction 2Co²+ (aq) + 2Cl(aq) +2Co²+ (aq) + Ch₂(g). E 0.483 V what is the cell potential at 25°C if the…
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
4)A galvanic cell is constructed that uses the following half-cell reactions: Cu+(aq) + e−→ Cu(s) I2(s) + 2e−→ 2I−(aq) a)Determine the cell potential for the spontaneous reaction under standard conditions. b)If the cell in part a is operated at 298 K with [Cu+] = 2.5 M and [I−] = 3.5 M, calculate the cell potential. Is the reaction spontaneous under these conditions? Explain. c)If [Cu+] was equal to 1.4 M, at what concentration of I− would the cell have zero potential?