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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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
EHide blocks Stane #7 Calculate the standard potential for the reaction shown below at 25°? 6 Hg*2 (aq) + 2 MnO2 (s) + 8 OH (aq) 3 Hg2*2 (aq) + 2 MnO4 (aq) + 4 H2O (I) E° = %3D Check Next p NEXT ACTIVITY S ACTIVITY Writing Equations (PRACTICE ASSIGNMENT) - Not Required Jump to...
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Practice chem question
Question 18A 2 H2(g) + 02(g) → 2 H2O(1) AGan = -474 kJ/mol Electrode Half-Reaction Standard Reduction Potential (V) Cathode O2(9) + 4 H*(aq) + 4 e- → 2 H2O(1) ? Anode 2 H*(ag) + 2 e → H2(g) 0.00 The operation of a hydrogen fuel cell under standard conditions relies on the chemical reaction represented above. The table provides the relevant reduction half-reactions and the standard reduction potentials. Based on the information given, which of the following equations can be used to calculate the standard reduction potential, in volts, of the half-reaction occurring at the cathode? E red (cathode) -474 4 x 96,500 A E' red (cathode) -474,000 4 x 96,500 E red (cathode) = 4 x 96,500 474 4 x 96,500 D E' red (cathode) = -474,000 回く* Q Search or enter website name
the answer is 1.495V but I cant seem to get it
Q20
Chemistry practice question
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 1.27 atm, the Cl- concentration is 8.06x10-3M, and the Hg2+ concentration is 6.78×10-4M ? Cl2(g) + Hg(1) 2CI"(aq) + Hg2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
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.