5-eleWhat is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu²* concentration is3.68×10-4 M and the Mg?+ concentration is 1.29 M ?Cu2*(aq) + Mg(s)-→ Cu(s) + Mg²*(aq)Answer:VThe cell reaction as written above is spontaneous for the concentrations giver vtruefalseSubmeit Ane werRotmu Entire

Answered: Image /qna-images/answer/4eeff32b-0ca8-4d7f-af78-ed35ff40c82b.jpg

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu²+ concentration is 3.68×10-4 M and the Mg²+ concentration is 1.29 M ? Cu2*(aq) + Mg(s)→ Cu(s) + Mg²*(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations giver v true false

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu²+ concentration is 3.68×10-4 M and the Mg²+ concentration is 1.29 M ? Cu2(aq) + Mg(s)→ Cu(s) + Mg²(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations giver v true false

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

When the Cu2+ concentration is 1.35 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.610V. What is the Mn2+ concentration? 2+ Cu²*(aq) + Mn(s)→ Cu(s) + Mn²*(aq) Answer: M
Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.012 M at 25 °C. 2 Fe²+ (aq) + H₂O₂(aq) + 2 H+(aq) → 2 Fe³+ (aq) + 2 H₂0 (1) Acidic Solution Standard Electrode Potential, E (volts) +1.77 2 H₂O(l) H₂O₂(aq) + 2 H*(aq) + 2 e Au*(aq) + e —»Au(s) Au*'(aq)+3e — Au(s) +1.68 +1.50 +1.08 NO(g) + 2 H₂O +0.96 Br₂(l) + 2 e2 Br(aq) NO3(aq) + 4 H*(aq) + 3 e Ag (aq) + e→→→→→→ Ag(s) Hg₂²(aq) + 2 e→→→→→2 Hg(l) +0.80 +0.789 Fe³(aq) + e-→→→→→→ Fe²¹(aq) +0.77 Cu²+ (aq) + 2 e → Cu(s) +0.337 HgzClz(s) + 2 e2 Hg() + 2 Cl(aq) +0.27 Sn¹+ (aq) + 2e → Sn²+ (aq) +0.15 2 H*(aq) + 2 e→→→→→→ H₂(g) 0.00 Pb²+ (aq) + 2 e Pb(s) -0.126 Sn²+ (aq) + 2 e → Sn(s) -0.14 Ni²+ (aq) + 2 e → Ni(s) -0.25 Cd²+ (aq) + 2 e → Cd(s) -0.40 Cr³+ (aq) + e →Cr²+ (aq) -0.408 Fe²+ (aq) + 2 e → > Fe(s) -0.44 Zn²+ (aq) + 2 e→→→→→→ Zn(s) -0.763 Cr²+ (aq) + 2 e →→ Cr(s) -0.91 Al³+ (aq) + 3 e →Al(s) -1.66 Mg²+ (aq) + 2 e -2.37 Mg(s) V
Determine the value of the equilibrium constant for the cell reaction below at 25 °C? 2 MnO2(s) + 8 OH (aq) + 3 Hg2²"(aq) → 2 MnO4 (aq) + 6 Hg(1) + 4 H20(1) 2+ O A. 9.40×1072 O B, 2.47x104 O.6.08×108
Given the standard electrode reduction potentials, which reaction will occur spontaneously?
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Cl, pressure is 1.43 atm, the CI concentration is 8.50×10-3 M, and the Cd2+ concentration is 8.53×10-4 M ? Cl2(g) + Cd(s)- →2CI(aq) + Cd²+(aq) Answer: The cell reaction as written above is spontaneous for the concentrations give v true false Submit Answer Retry Entire Group 9 more group attempts remaining
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 3.37×10-3 atm, the H* concentration is 1.04M, and the Mg2+ concentration is 7.01×10-4M ? 2H (аq) + Mg(s)—— Н2(g) + - Mg2*(aq) Answer: The cell reaction as written above is spontaneous for the concentrations give v true false Submit Answer Retry Entire Group 9 more group attempts remaining
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 1.19 M and the Mn2+ concentration is 4.85×10-4 M? Cu2+(aq) + Mn(s) Cu(s) + Mn2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 3.55x10-4 M and the Al3+ concentration is 1.22 M? 3Hg2+ (aq) + 2Al(s) 3Hg(l) + 2Al³+ (aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: (
9
When the Agt concentration is 1.01 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.072V. What is the Mn2+ concentration? 2Ag+(aq) + Mn(s)→2A9(s) + Mn2+(aq) Answer: M
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Ag+ concentration is 6.17 x 10-4 M and the Mn²+ concentration is 1.04 M ? Ecell 2+ 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) V The cell reaction as written above is Submit Answer Retry Entire Group spontaneous nonspontaneous for the concentrations given. y attempts remaining
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg** concentration is 2.89x104 M and the Mg concentration is 1.41 M ? Hg**(aq) + Mg(s)→ Hg(1) + Mg*(aq) Answer: The cell reaction as written above is spontaneous for the concentrations given: