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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Consider the silver iodide cell below: Ag(s)|AgI(s)||Cu2+(aq)|Cu(s)T=298 K Based on this reaction: 2Ag(s)+2I−(aq)+Cu2+(aq)↽−−⇀Cu(s)+2AgI(s)ΔrG∘=−94.6 kJ/mol What is Ecell for this reaction when the concentration of iodide is 1.0 M and copper ions is 222 μM? What is E∘cell for this reaction? (V) Ecell(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 n AGº K A 1 -19. kJ/mol 4.69 × 10 0 E 0.20 V 13 B 1 77. kJ/mol 3.09 × 10 0.80 V -14 C 1 75. kJ/mol 7.25 X 10 0.78 V
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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If the potential of a galvanic cell is +1.20 V, what is the Gibbs free-energy change when one mole of electrons is transferred in the oxidation–reduction reaction?
Calculate the G in kJ for the following cell: Al(s)|Al3+(0.0035M)||Fe3+(0.55M)|Fe(s) Eocell=+1.59 V Al(s)|Al3+(0.0035M)||Fe3+(0.55M)|Fe(s) Group of answer choices -473 -374 -158 -734 -658 Calculate Ecell in volts. Cu(s)|Cu2+(3.00x10-4)||Ag+(0.15M)|Zn(s) Eocell=+0.620 V 0.700 0.544 0.944 0.644 0.800
The free energy change for the following reaction at 25 °C, when [Pb2+] = 3.82×10-3 M and [Cu2+] = 1.20 M, is 68.1 kJ: Pb2+(3.82×10-3 M) + 2Cu+(aq)Pb(s) + 2Cu2+(1.20 M) ΔG = 68.1 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 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 K E - 16 1.14 X 10 A 2 -91. kJ/mol -0.47 V - 49 1.98 x 10 B 2 - 278. kJ/mol 1.44 V - 44 5.34 x 10 2 247. kJ/mol 1.28 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 n 46° K 1 - 124. kJ/mol 5.30 x 10 21 -1.28 V -18 4.53 x 10 B 1 - 99. kJ/mol -1.03 V -7 2.20 x 10 1 - 38. kJ/mol 0.39 V
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.
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGº. • 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 n aG K E -21 1.42 x 10 A 1 119. kJ/mol O 1.23 V -- В - 51. kJ/mol 1.16 X 10 -0.53 V -11 2.06 X 10 1 -61. kJ/mol 0.63 V