Problem 10 An electrochemical cell utilizes the following redox process at 25°C: 2+ Sn"(aq) + X(s) → Sn(s) + X²“(aq), X(s)x2* (aq, 1 M||Sn* (aq, 1 M|Sn(s) <===> Where X symbolizes some metal. The standard galvanic cell potential (standard emf) is: Eel = 0.14 V. What is the standard reduction half-cell potential, E°, 2+ if E° 2+ = - 0.14 V? "cell Sn /Sn Enter your answer in the box provided with correct units and sig. fig.: The standard reduction : E. x2*x Answer: half-cell potential for X is

Problem 10 An electrochemical cell utilizes the following redox process at 25°C: 2+ Sn"(aq) + X(s) → Sn(s) + X²“(aq), X(s)x2* (aq, 1 M||Sn* (aq, 1 M|Sn(s) <===> Where X symbolizes some metal. The standard galvanic cell potential (standard emf) is: Eel = 0.14 V. What is the standard reduction half-cell potential, E°, 2+ if E° 2+ = - 0.14 V? "cell Sn /Sn Enter your answer in the box provided with correct units and sig. fig.: The standard reduction : E. x2*x Answer: half-cell potential for X is

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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When the Cu2+ concentration is 8.99×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.905V. What is the Al3+ concentration?3Cu2+(aq) + 2Al(s)3Cu(s) + 2Al3+(aq)Answer: ___M
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag+ concentration is 1.18 M and the Mg2+ concentration is 2.99×10-4 M? 2Ag+(aq) + Mg(s) 2Ag(s) + Mg2+(aq) Answer: _______ V The cell reaction as written above is spontaneous for the concentrations given: true or false
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 7.14x10-3 atm, the H* concentration is 1.24M, and the Mg+ concentration is 6.01x10-M ? 2H (aq) + Mg(s)–H2(g) + Mg*"C *(aq) Answer: -0.164 V The cell reaction as written above is spontaneous for the concentrations given: false v
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What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg2+concentration is 3.59×10-4 M and the Cr3+ concentration is 1.07 M ? 3Hg2+(aq) +2Cr(s) ➞ 3Hg(l) + 2Cr3+(aq)Answer: ____ VThe cell reaction as written above is spontaneous for the concentrations given: _______ (true or false)
O ADVANCED MATERIAL Designing a galvanic cell from two half-reactions A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential NO, (aq)+4H (aq)+3e¯ → NO(g)+2 H,O(1) E red = +0.96 V Cl,(9)+2e + 2 Cl (ag) = +1.359 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 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 information to calculate the cell voltage under standard conditions? Yes No If you said it was possible to calculate the cell voltage, do so and enter your answer ||V here. Round your answer to 2 significant digits.
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb2+ concentration is 1.08 M and the Mn2+ concentration is 8.79×10-4 M? Pb2+(aq) + Mn(s) Pb(s) + Mn2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: