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 K E A 2 226. kJ/ mol 39 3.92 x 10 1.17 V В 120. kJ/mol 1.05 x 10 -0.62 V 37 – 214. kJ/mol 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 K E A 2 226. kJ/ mol 39 3.92 x 10 1.17 V В 120. kJ/mol 1.05 x 10 -0.62 V 37 – 214. kJ/mol 3.10 x 10 -1.11 V

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...

See similar textbooks

Similar questions

The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is E = E-2.303RTn Flog 10Q where E is the potential in volts, Eo is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E = E-(0.0592n)logQ The reaction quotient has the usual form Q = [products]x[ reactants]y A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. Part A For the reaction 2C03 + (aq) + 2CI-(aq)-> 2Co2 + (aq )+ Cl2(g). E = 0.483 V what is the cell potential at 25° C if the concentrations are…
Calculate the standard free energy, ∆G°, for a galvanic cell represented by the following notation: M| M+||N3+|N with reduction potential of 0.36 V for M and 1.05 V for N, respectively. (Note that M and N are fake metals). Calculate the value of ∆G° in J. F = 96500 C/mol e- Enter your answer in scientific notation with 2 decimal places and be sure to include the correct sign. Example: -2.34e+6 or 1.23e-5. Note e is used for "x10" in this notation! Do NOT type "x 10"!
Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.5M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.19 volts. Your Answer:
Consider the following electrochemical cell at 25 C: Pt|H2(g,p)|HCl(aq), 0.010 mol.kg-1|AgCl(s)|Ag For this cell the cell reaction is as follows: 2AgCl(s) + H2(g)  2Ag(s) + 2HCl(aq) (a) Give the electrode half-reactions and determine the standard cell potential.
The anode compartment of a galvanic cell consists of a Zn anode immersed in 0.05M ZnCl2 The cathode compartment consists of a Cu cathode immersed in an 0.10M CuCl2 solution. Using the cell potentials found on page 815 of your textbook, calculate the cell potential for this reaction. Assume T = 298K.
Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g, 1.0 atm) ∣ H+(aq,1.0M) ∣∣ Au3+(aq,? M) ∣ Au (s)Determine the standard cell potential and if the cell is more spontaneous or less spontaneous at standard conditions.
Calculate the cell potential of a cell composed of a cathode consisting of a Co wire immersed in a 1.44 M Co²+ solution and an anode consisting of a Co wire immersed in a 5.60×10-5 M Co²+ solution. Assume the temperature of the solutions is 298 K. Cell potential: V
Given the balanced electrochemical reaction below (M and N represent generic metals), what is the cell potential (Ecell), in volts, for this reaction at 35.4 °C when [M+] = 0.00533 M and [N2+] = 0.725 M? Enter your answer to the thousandths place. Do not include units. 2M+(aq) + N(s) → 2M(s) + N2+(aq) E°cell = 0.128 V
Determine the cell potential (in volts) of a standard galvanic cell constructed using iron and lead metals and their associated solutions, 1M FeSO4 and 1M PbSO4.
1) For the following cell at 25°C: a) Zn(s) | ZnCl₂(aq) || AgCl (aq) | Ag(s) Write the half-reactions; b) write the overall cell reaction; c) calculate the standard cell potential; d) calculate the cell potential assuming the ZnCl₂ solution is made up with an activity of 0.5 instead of 1.0; calculate AG; e) calculate AG"; f) calculate K. Atrempt only if you can answer all parts I'll upvote your answer otherwise I'll downvote
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. cell A B C₁ n 1 1. 1 calculated quantities (Check the box next to any that are wrong.) ·a AG 77. kJ/mol O 64. kJ/mol 35. kJ/mol O O K 3.09 X 10 6:13 X 10 13. 6 1.35 X 10 - 12. O X 0. 0.80 V 0.66 V -0.36 V Ś
The standard cell potential is a thermodynamic state func-tion. How are E° values treated similarly to ΔH°, ΔG°, and S°values? How are they treated differently?