When the Ag+ concentration is 1.36×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is2.937V. What is the Mg2+ concentration?2Ag*(aq) + Mg(s)2Ag(s) + Mg²+ (aq)Answer: 0.66 M Consider the following cell reaction:Ni(s) + 2 H*(? M) →Ni²+(1.00 M) + H₂(g)(1.00 atm)If the cell potential at 298 K is 0.100 volts, what is the pH of the hydrogen electrode?pH = 2.65|

Answered: Image /qna-images/answer/6adf567d-22a3-4614-a100-2c93d334a88a.jpg

When the Ag* concentration is 1.36x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.937V. What is the Mg2+ concentration? 2Ag (aq) + Mg(s) →2Ag(s) + Mg2+(aq) Answer: 0.66 M

When the Ag* concentration is 1.36x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.937V. What is the Mg2+ concentration? 2Ag (aq) + Mg(s) →2Ag(s) + Mg2+(aq) Answer: 0.66 M

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 Pb2+ concentration is 1.16 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 0.732V. What is the Zn2+ concentration? Pb2+(aq) + Zn(s) Pb(s) + Zn2+(aq)
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Pb²+ concentration is 1.69 × 10-4 M and the Mg²+ concentration is 1.43 M? Pb²+ (aq) + Mg(s) → Pb(s) + Mg²+ (aq) (aq) + 2e → Pb(s) Fred = -0.126 V Mg(s) Fred Eº = -2.370 V Pb²+ Mg2+ (aq) + 2e Ecell = The cell reaction as written above is spontaneous for the concentrations given: O true Ofalse V
1a. When the Cu2+ concentration is 7.81×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.612V. What is the Mg2+ concentration?Cu2+(aq) + Mg(s) Cu(s) + Mg2+(aq) 1b. When the Hg2+ concentration is 1.14 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.726V. What is the Zn2+ concentration?Hg2+(aq) + Zn(s) Hg(l) + Zn2+(aq) 1c. When the Hg2+ concentration is 2.15×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.406V. What is the Al3+ concentration?3Hg2+(aq) + 2Al(s)3Hg(l) + 2Al3+(aq)
When the Ag concentration is 8.41 x 10 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.274V. What is the Al+ concentration? 3Ag+ (aq) + Al(s) 3Ag(s) + AIs+ (aq) [Ar*+] = M
If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2 is 1.00 atm, calculate the cell potential at 25.0°C.The standard reduction potentials are:Ag+(aq)+1e−Ag(s) Eo = 0.80 V2H+(aq)+2e−H2(g) Eo = 0.00 V V
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Agt concentration is 1.09 M and the Zn² concentration is 7.69 x 10-4 M? 2Ag+ (aq) + Zn(s) → 2Ag(s) + Zn²+ (aq) 0.799 V Ag (aq) + e → Ag(s) E Zn²+ red (aq) + 2e → Zn(s) E red = Ecell The cell reaction as written above is spontaneous for the concentrations given: O true O false -0.763 V V
When the Agt concentration is 5.60x104 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.972V. What is the Mg2+ concentration? 2Ag*(aq) + Mg(s)2Ag(s) + Mg2+(aq)
When the Cu2+ concentration is 1.00 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.799V. What is the Mg2+ concentration? Cu2+(aq) + Mg(s) Cu(s) + Mg2+(aq)
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Agt concentration is 2.56 x 10-4 M and the A1³+ concentration is 1.00 M? 3Ag+ (aq) + Al(s) → 3Ag(s) + A1³+ (aq) Ag+ (aq) +e → Ag(s) Ed red = 3+ Al³+ (aq) + 3e → Al(s) Fred Ecell The cell reaction as written above is spontaneous for the concentrations given: O true O false 0.799 V -1.660 V V
Calculate the cell potential for the following concentration cell at 25 °C. Ni(s) Ni(NO3)2(0.00522M)|Ni(NO3)2(3.07 M)Ni(s)
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)
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Pb²+ concentration is 9.40 × 10-4 M and the Zn²+ concentration is 1.18 M? Pb²+ (aq) + Zn(s) → Pb(s) + Zn²+ (aq) Pb2+ (aq) + 2e7 →→ Pb(s) E red Zn²+ (aq) + 2e → Zn(s) Ee red Ecell = -0.126 V = -0.763 V Otrue Ofalse = The cell reaction as written above is spontaneous for the concentrations given: