The standard potential of an electrochemical cell has been measured at several different temperatures. T/°C -10 40 90 120 E® / V 0.261 0.269 0.324 0.388 0.421 From these data, determine the values of A.GR, A.SÂ and ArHA for the reaction at 20 °C given that the number of electrons in the balanced half reactions is one.

The standard potential of an electrochemical cell has been measured at several different temperatures. T/°C -10 40 90 120 E® / V 0.261 0.269 0.324 0.388 0.421 From these data, determine the values of A.GR, A.SÂ and ArHA for the reaction at 20 °C given that the number of electrons in the balanced half reactions is one.

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

Consider the following electrochemical cell at a pH of 8.00:Cu(s)|Cu2+(aq, 0.0125 M) || VO2+( aq, 0.00125 M), VO2+( 0.0250 M)b. Calculate E0cell for this system.
For the following cells, write the half-reactions occurring at each electrode and the complete cell reaction. Calculate the cell potential too. Pt, H2 (0.1 atm) | HCI (0.5M) | Cl2 (0.1 atm), Pt Given E o for H2 = 0.000 V E o for Cl2 = 1.359 V
A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 51.0 hours at 25 °C? (E° for Pb²⁺/Pb = -0.130 V and E° for Ni²⁺/Ni = -0.250 V.)
Consider an electrochemical cell made up of Au Au* and Co²+ | Co³+ half-cells. Part 1 of 2 Write the equation for the cell reaction that occurs under standard-state conditions. Be sure to include the physical state of each species in the reaction. Part 2 of 2 E = ローロ V 00 Calculate the standard emf of a cell that uses the Au Au and Co²+ | Co³+ half-cell reaction at 25 °C. Round your answer to 2 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. 09 S
3. Calculate the free energy, AG°, for each electrochemical cell given the following information and determine if the reaction is spontaneous or nonspontaneous. T= 298 K a. E cell =+ 2.10 V, n= 2 b. Каg— 2.2 х 10-3 c. E cell =- 0.677 V, n = 3 =
7
A voltaic cell consists of an Al/Al3+ half-cell and a Fe2+/Fe3+ half-cell. The standard reduction potential for Al3+ is −1.66V and for Fe3+ is 0.77 V. Calculate Ecell at 25 ºC when the concentration of [Al3+] = 9.51 x 10-4 M , [Fe3+]= 6.24 x 10-3 M, and [Fe2+]= 5.74 x 10-5 M
Calculate the cell potential of a voltaic cell given the following standard potentials: X -> X2+ + 2 e- Eo = -1.69 V Y3+ -> + 3 e- -> Y Eo = 0.94 V Note: Answer in 2 decimal places.
If a voltaic cell is created between a Sr2+/Sr electrode and a In3+/In electrode
-3 M solution of Cu(NO3)2. The other half-cell consists of a zinc electrode in One half-cell in a voltaic cell is constructed from a copper wire electrode in a 3.9 x 10 a 0.45 M solution of Zn(NO3)2 . Calculate the cell potential. You may need to use the following data: Zn²+ (aq) + 2 e¯ → Zn(s) E° = -0.763 V Cu²+ (aq) + 2 e¯ → Cu(s) E° = +0.337 V Potential = V
3. The oxidation of methanol, as described by the equation below, has a AG value of -937.9 kJ/mol. What is the standard cell potential for a methanol fuel cell? 2CH3OH +30₂ → 2CO₂ + 4H₂O
Predict reaction and calculate E°cell from standard reduction potentials. A voltaic cell is constructed from a standard AI3+|Al half cell (E°red = -1.660V) and a standard F2|F° half cell (E°red = 2.870V). What is the spontaneous reaction that takes place, and what is the standard cell potential? Spontaneous cell reaction:Write a balanced equation using the smallest integer coefficients possible. + Standard cell potential: V.