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 is1.04M, 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 vtruefalseSubmit AnswerRetry Entire Group9 more group attempts remaining

Answered: What is the calculated value of the…

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...

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Can you please answer these two sub problems and show all of the steps to the solution
Practice: will the reaction be spontaneous? If not write the spontaneous direction, and calculate the Ecell. Sketch the cell and write the line notation of the spontaneous reaction. Zn + Ca2+ → Zn2+ + Ca a) Spontaneous b) Not spontaneous c) Not sure Zn2+(aq) + 2e Zn(s) -0.76 Cr³+ (aq) + 3e Cr(s) -0.73 2 H₂O(l) + 2e Mn2+( Al3+(aq) + 3e Mg2+(aq) + 2e H2(g) +20H(aq) -0.83 +(aq) + 2e¯ Mn(s) -1.18 Al(s) -1.66 Mg(s) -2.37 Na+ (aq) + e Na(s) -2.71 Ca2+ (aq) + 2e →Ca(s) -2.76
The free energy change for the following reaction at 25 °C, when [Ag*] = 1.20 M and [Cu2+] = 8.38x10-3 M, is -101 kJ: 2Ag*(1.20 M) + Cu(s)2Ag(s) + Cu2+(8.38x10-3 M) AG = -101 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction v forward reverse
6
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
the standard cell potential (E°cell) for the voltaic cell based on the reaction below is what? Cr(s) + 3Fe3+(aq) --> 3Fe2+(aq) + Cr3+(aq)
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: (
When the Hg2+ concentration is 2.22×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.486V. What is the Cr³+ concentration? 3Hg²*(aq) + 2Cr(s)3Hg(1) + 2C1³*(aq) Answer: M
Item 1 < 1 of 25 Constants | Periodic Table Part A The standard cell potential (E') of the reaction below is -0.55 V. The value of A G for the reaction is J/mol. I2 (5) + 2Br (aq) → 21 (aq) + Brz (1) O 1.1- 105 O 0.54 O 0.55 O 5.5 - 106 O none of the above Submit Request Answer
When the Ag+ concentration is 4.19×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.257V. What is the Al3+ concentration? 3Ag+(aq) + Al(s)3Ag(s) + Al3+(aq)Answer: M
When the Hg+ concentration is 8.47×104 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.422V. What is the Al3+ concentration? 3Hg*"(aq) + 2Al(s)- →3H9(1) + 2A1*(aq) Answer: 7.53x10^6
What is the potential (inV) of the cell given below at 25 degree celsius ?

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