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When the Hg2+ concentration is 7.21x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.938V. What is the Mn2+ concentration? Hg²+ (aq) + Mn(s)→→→→→→ Hg(l) + Mn²+ (aq) Answer: M When the Hg2+ concentration is 3.34×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.492V. What is the Cr³+ concentration? 3Hg2+ (aq) + 2Cr(s) 3Hg(1) + 2Cr³+ (aq) Answer: M

When the Hg2+ concentration is 7.21x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.938V. What is the Mn2+ concentration? Hg²+ (aq) + Mn(s)→→→→→→ Hg(l) + Mn²+ (aq) Answer: M When the Hg2+ concentration is 3.34×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.492V. What is the Cr³+ concentration? 3Hg2+ (aq) + 2Cr(s) 3Hg(1) + 2Cr³+ (aq) Answer: M

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Chemistry
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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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Nernst 2-part question (0.722 is not correct answer for either part)

 

When the Hg2+ concentration is 7.21×104 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.938V. What is the Mn²+ concentration? Hg²+ (aq) + Mn(s)→→→ Hg(1) + Mn²+ (aq) Answer: M When the Hg2+ concentration is 3.34×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.492V. What is the Cr³+ concentration? 3Hg2+ (aq) + 2Cr(s)- →3Hg(1) Answer: M + 2Cr³+ (aq)
Transcribed Image Text:When the Hg2+ concentration is 7.21×104 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.938V. What is the Mn²+ concentration? Hg²+ (aq) + Mn(s)→→→ Hg(1) + Mn²+ (aq) Answer: M When the Hg2+ concentration is 3.34×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.492V. What is the Cr³+ concentration? 3Hg2+ (aq) + 2Cr(s)- →3Hg(1) Answer: M + 2Cr³+ (aq)
A non-standard cell or half-cell potential can be calculated using the Nernst Equation: RT where E = Eº E யய் R T n F = = potential under non-standard conditions = standard potential ideal gas constant = kelvin temperature nF = In Q = number of moles of electrons for the reaction as written = charge carried by 1 mol of electrons reaction quotient It is customary to use the equation in a form where numerical values are substituted for R, T and F at a temperature of 25 °C. For = 8.314 J mol-¹K-1 T = 298.15 K F = 96,485 J V-1 mol-1 RT (8.314 J mol-¹ K-¹)(298.15 K) E = Eº F 96,485 J V-1 mol-1 and the Nernst equation with the potentials in volts is: 0.0257 n = 0.0257 V In Q natural logarithm
Transcribed Image Text:A non-standard cell or half-cell potential can be calculated using the Nernst Equation: RT where E = Eº E யய் R T n F = = potential under non-standard conditions = standard potential ideal gas constant = kelvin temperature nF = In Q = number of moles of electrons for the reaction as written = charge carried by 1 mol of electrons reaction quotient It is customary to use the equation in a form where numerical values are substituted for R, T and F at a temperature of 25 °C. For = 8.314 J mol-¹K-1 T = 298.15 K F = 96,485 J V-1 mol-1 RT (8.314 J mol-¹ K-¹)(298.15 K) E = Eº F 96,485 J V-1 mol-1 and the Nernst equation with the potentials in volts is: 0.0257 n = 0.0257 V In Q natural logarithm
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