A student performs the Electrochemistry, and obtains the following data: [Cu²+], M Potential, V 0.1 0.424 0.01 0.456 0.001 0.482 0.0001 0.512 0.00001 0.552 Lab Temperature, °C 19.0 [Ag+], M 0.1 0.1 0.1 0.1 0.1 Q Cu(s) + Ag+ (aq) → Cu²+ (aq) + Ag(s) 1: Balance the following redox reaction using half reactions, and determine the standard cell potential for the reaction. In Q 2: Calculate Q and In Q for each solution. Show a sample calculation for one trial below. 3: Prepare a plot of Potential vs In Q, and attach it to your submission. Report the standard cell potential, and calculate Faraday's constant below.

A student performs the Electrochemistry, and obtains the following data: [Cu²+], M Potential, V 0.1 0.424 0.01 0.456 0.001 0.482 0.0001 0.512 0.00001 0.552 Lab Temperature, °C 19.0 [Ag+], M 0.1 0.1 0.1 0.1 0.1 Q Cu(s) + Ag+ (aq) → Cu²+ (aq) + Ag(s) 1: Balance the following redox reaction using half reactions, and determine the standard cell potential for the reaction. In Q 2: Calculate Q and In Q for each solution. Show a sample calculation for one trial below. 3: Prepare a plot of Potential vs In Q, and attach it to your submission. Report the standard cell potential, and calculate Faraday's constant below.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 11P

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Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
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The standard potential, E, for the reaction of Zn(s) and Cl2(g) is +2.12 V. What is the standard free energy change, rG, for the reaction?
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG⁰. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 2. cell A B с n 2 2 2 calculated quantities (Check the box next to any that are wrong.) AGⓇ - 152. kJ/mol 81. kJ/mol -216. kJ/mol O K 26 4.26 X 10 1.55 X 10 6.94 X 10 14 37 X 0 E -0.79 V -0.42 V - 1.12 V
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG⁰. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. if any. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. cell A B C n 1 1 1 calculated quantities (Check the box next to any that are wrong.) AGº - 125. kJ/mol - 79. kJ/mol 57. kJ/mol K 1.26 X 10 6.92 × 10 9.68 × 10 - 22 13 0 E - 1.30 V 0.82 V -0.59 V
Using the given thermodynamic data in the table, determine the standard change in Gibbs free energy for this reaction at 298 K for the reaction of silver with hydrogen: 2Ag+(aq) + H2(g)2H+(aq) + 2Ag(s) Δ H f o / kJ∙mol –1 S o / J∙mol –1 ∙K –1 Ag + (aq) 105.58 72.68 Ag(s) 0 42.55 H 2 (g) 0 130.68 H + (aq) 0 0 Options: A. 48.7 kJ B. +162.5 kJ C. +268.1 kJ D. –154.3 kJ
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Consider the following electrochemical cell in, for which Ecell = = 0.18 V at 80C: Pt | H2(g) | HCl(aq) || AgCl(s) | Ag(s) H2(g) + 2AgCl(s) ⇌ 2H+(aq) + 2Cl−(aq) + 2Ag(s) If pH = 1.03 in the anode compartment, and [Cl−] = 3.3 M in the cathode compartment, determine the partial pressure of H2 necessary in the anode compartment for the cell to be 0.27 V at 80C
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG°. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E°. His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 2. calculated quantities (Check the box next to any that are wrong.) cell n aG E K 39 A 226. kJ/mol O 3.92 x 10 1.17 V 21 В 2 120. kJ/mol 1.05 X 10 -0.62 V 2 - 214. kJ/mol 37 3.10 X 10 - 1.11 V ?
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG°. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E°. His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 2. calculated quantities (Check the box next to any that are wrong.) cell n aG° E K 11 8.19 × 10 А 2 68. kJ/ mol O 0.35 V В 2 - 114. kJ/mol 20 1.07 x 10 0.59 V C 2 42. kJ/mol 7 2.28 X 10 - 0.22 V
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG°. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E". His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell AG K 20 1.40 x 10 A 1 - 115. kJ/mol -1.19 V -21 в 1 - 118. kJ/mol 2.12 x 10 -1.22 V -12 1.83 x 10 1 - 67. kJ/mol -0.69 V