What is the calculated value of the cell potential at298 K for an2+Cu²+ concentration is3.83 × 10-4 M and theA1³+ concentration is1.12 M?Ecellelectrochemicalcell with the following reaction, when the2+3Cu²+ (aq) + 2Al(s) → 3Cu(s) + 2A1³+ (aq)VThe cell reaction as written abovespontaneousnonspontaneousfor the concentrations given.

Answered: Image /qna-images/answer/fb0621b7-46b7-4ff8-9f65-edce712a6998.jpg

What is the calculated value of the cell potential at 298 K for an electrochemical Cu²+ concentration is 3.83 × 10-4 M and the Al³+ concentration is 1.12 M? Ecell = cell with the following reaction, when the 3Cu²+ (aq) + 2Al(s) → 3Cu(s) + 2A1³+ (aq) V The cell reaction as written above spontaneous nonspontaneous for the concentrations given.

What is the calculated value of the cell potential at 298 K for an electrochemical Cu²+ concentration is 3.83 × 10-4 M and the Al³+ concentration is 1.12 M? Ecell = cell with the following reaction, when the 3Cu²+ (aq) + 2Al(s) → 3Cu(s) + 2A1³+ (aq) V The cell reaction as written above spontaneous nonspontaneous for the concentrations given.

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 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..
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. Cl2 + Br- -> Cl- + Br2
Consider the galvanic cell: Pt(s) | H2(1 atm)|H*(1 M) || CI(1 M) | H82CII2(s)|Hg(1) Which of the following changes to the cell would cause the cell potential to increase? O increase the Pt mass decrease the pH O increase the pH O decrease the Pt mass
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)
from question 6 to 12 please
Consider the following galvanic cell: Li (s) | 0.095M LiCl (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s) Using Appendix H in the textbook, determine the Ecell of this galvanic cell. 2.54 V - 2.88 V O -2.92 V 2.88 V 2.92 V
The cell notation for the Galvanic cell is Cd(s)/Ca2+l2(s)/I" The Standard Reduction Potential are as follows: E°Ca2+/cd = -0.403 V; E12/1 = 0.5355 v Calculate the standard cell potential If the Cadmium ions have a concentration of 0.010 M and the iodide ions have a concentration of 0.020 M, calculate the electromotive force (EMF) of the cell. The Gibbs Free Energy of the cell is
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
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 particular galvanic cell has a standard cell potential of Eocell = 0.62 V. If the Eo of the cathode is 0.40 V, what is the Eo of the anode?
Consider the voltaic cell with a standard cell potential of 0.150 V. What is the cell potential of the voltaic cell at 400 K? Cd(s) | Cd²+ (0.100 M) || Ni²+ (1.00 x 10-4 M) | Ni(s) R 8.314 J/mol-K; F = 96,485 J/mol-V O 0.239 V 0.061 V O 0.269 V O 0.031 V
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