A Fe Fe²+ || Cd2|Cd galvanic cell is constructed in which the standard cell voltage is 3.70-102 V. Calculate the free energy change at 25°C when 0.863 g of Cd plates out, if all concentrations remain at their standard value of 1 M throughout the process. What is the maximum amount of work that could be done by the cell on its surroundings during this experiment? A

A Fe Fe²+ || Cd2|Cd galvanic cell is constructed in which the standard cell voltage is 3.70-102 V. Calculate the free energy change at 25°C when 0.863 g of Cd plates out, if all concentrations remain at their standard value of 1 M throughout the process. What is the maximum amount of work that could be done by the cell on its surroundings during this experiment? A

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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Calculate the cell potential for the galvanic cell in which the reaction Cd(s) + Cu²+ (aq) Cd²+ (aq) + Cu(s) occurs at 25 °C, given that [Cd²+] = 0.00130 M and [Cu²+] =0.869 M. Refer to the table of standard reduction potentials. E=
a) Balance the following reactions. b) Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. c) Identify the reactions with K > 1 among the following redox reactions. d) Write the line representations for the Galvanic cells, indicating the anode and cathode. Cl2 + Br- --> Cl- + Br2 MnO4- + H+ + Ce3+ --> Ce4+ + Mn2+ + H2O Pb2+ -->Pb + Pb4+ NO3- + H+ + Zn --> Zn2+ + NO2 + H2O
11. Consider the following reaction and its AG-AGo at 25.00 °C 2Ag(aq)+Cu(s) 2Ag(s)+Cu (aq) AG =-88660 J/mol a. Calculate the standard cell potential, E, for the reaction. b. Calculate the equilibrium constant, K, for the reaction.
Consider the following reaction and its AG" at 25.00 °C. Mg(s) + Ni" (aq) – Mg²* (aq) + Ni(s) AG = -408.0 kJ/mol Calculate the standard cell potential, E for the reaction. E = V cell Calculate the equilibrium constant, K, for the reaction. K =
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2+ Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg² ]=0.761 Mand [Ni²+]=0.0180 M. Use the standard reduction potentials from the 2+ appendix in the book. 2+ ↔ Mg²+ (aq) + Ni(s) Give the numeric value only assuming a measurement in V Mg(s) + Ni²+ (aq) → 2+ (aq)
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.
Calculate the cell potential for the galvanic cell in which the reaction Ti(s)+Co2+(aq)↽−−⇀ Ti2+(aq)+Co(s) occurs at 25 °C, given that [Ti2 + ] = 0.00180 M and [Co2 + ] = 0.813 M. Refer to the table of standard reduction potentials.
Consider the following cell: Ni(s)|Ni2+(aq, 0.100 M)||Cl–(aq, 0.200 M)|Cl2(g, 1.50 atm)|Pt If the standard voltage for this cell is 1.59 V at 25oC, calculate the voltage of this cell.
The standard reduction potential, E°, for the reaction Fe2+(aq) + 2e- ⇌ Fe(s) is -0.44 V while for Zn2+(aq) + 2e- ⇌ Zn(s) it is -0.7618 V. i) Write a balanced chemical equation for the spontaneous reaction that occurs between these reagents. Calculate the standard cell potential and comment on its value. ii) Determine the cell potential when a piece of iron is placed in a solution containing 0.1 M Zn2+ and 0.5 M Fe2+ . iii) Determine the concentration of Fe2+ when equilibrium is established and describe what will happen during the course of the reaction. Answer full explanation and details Don't upload image.
The free energy change for the following reaction at 25 °C, when [Cr**]= 2.80×103 M and [H= 1.11 M, is 94.0 kJ: 2Cr*(2.80×10³ M) + H,(g)2Cr*(aq) + 2.00H*(1.11 M) AG = 94.0 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
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. 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, if 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 n A B C 1 calculated quantities (Check the box next to any that are wrong.) AGⓇ 37. kJ/mol - 66. kJ/mol -47. kJ/mol K 6 3.03 × 10 2.74 × 10 5.83 × 10 12 9 X 0 E -0.38 V 0.68 V -0.49 V S