What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag* concentration is 5.91×10-4 M and theCr3+ concentration is 1.42 M?3Ag (aq) + Cr(s) >3Ag(s) + Cr3+(aq)Answer:The cell reaction as written above is spontaneous for the concentrations given:

We first need the standard reduction potentials for each half-reaction. Based on standard reduction…

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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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 1.14 x 10-4 M and the Mn²+ concentration is 1.05 M? 2Ag (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) Ag (aq) +e → Ag(s) Fred=0.799 V Mn²+ (aq) + 2e → Mn(s) E= -1.180 V Ecell = V The cell reaction as written above is spontaneous for the concentrations given: O true O false
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H2 pressure is 2.22×10-3 atm, the H† concentration is 1.38M, and the Cr3+ concentration is 3.60×10-4M ? 6.00H*(aq) + 2Cr(s)→3H2(g) + 2C1³*(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
When the Ag+ concentration is 1.26 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 3.267V. What is the Mg2+ concentration? 2Ag+(aq) + Mg(s)2Ag(s) + Mg2+(aq)
When the Pb2+ concentration is 5.46×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.147V. What is the Mg2+ concentration?Pb2+(aq) + Mg(s) Pb(s) + Mg2+(aq)
What is the standard cell potential for the reaction below? Enter your answer with two decimal places and no units. Mg(s) + Br2() Mg2+(aq) + 2 Br"aq) The standard reduction potential is -2.37 V for the Mg2+/Mg half-cell and +1.09 V for the Bro/Br half-cell. Enter your answer in decimal format using two decimal places, (value + 2%).
A voltaic cell employs the following redox reaction: 2 Fe3+ Calculate the cell potential at 25 °C under each of the following conditions. (ag) + 3 Mg (s) → 2 Fe (s) + 3 Mg²+ (aq) Part C [Fe+] = 3.10 M ; [Mg²+] = 1.2x10-3 M Ecell Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
For the galvanic cell: Zn(s) + 2Tl+(aq) 2Tl(s) + Zn2+(aq) Eocell = 0.42 V The standard reduction potential for the half cell Zn2+(aq) + 2e– Zn(s) is Eored = –0.76 V What is the standard reduction potential for Tl+(aq) + e– Tl(s) Eored = ? V a. +0.17 V b. –0.17 V c. –0.34 V d. +0.34 V
Using standard potentials given in the appendices, calculate the standard cell potentials for the following reaction: Cu(s) + 2Ag+ (aq) = Cu²+ + 2Ag(s) Report the answer in volts with three significant figures. 0.462 V Submit Previous Answers Correct Correct answer is shown. Your answer 0.46 V was either rounded differently or used a different number of significant figures than required for this part. Part B Determine the equilibrium constant for the above reaction.
You have a cell that uses the following overall reaction. Calculate the cell potential at 298 K if [Au3+] = 0.010 M and [Mg2+] = 0.150 M 2 Au3+(aq) + 3 Mg(s) ---> 2 Au(s) + 3 Mg2+(aq)
Bhu Please don't provide the handwriting solution

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