Calculate the value of the cell potential, E cell for the following reaction:2 Au(s) + 3 Ca2+(aq)- →2 Au3+(aq) + 3 Ca(s)O-1.26 V-11.3 V+ 4.26 V-4.26 V+1.26 V

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Answered: Calculate the value of the cell…

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 volts) in which the following reaction occurs at 25.0∘C, given than [Ti2+] = 2.773 M and [Au3+] = 0.582 M. Use Standard reduction potentials
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
Calculate the standard cell potential and note whether the reaction is spontaneous under standard conditions. Mg(s) + Cu2+ --> Mg2+ + Cu(s)
Balance the following reaction. Calculate the cell potential and the Gibbs free energy of the reaction at standard conditions. Write the line representations for the Galvanic cells, indicating the anode and cathode.
Calculate the standard cell potential (E°cell) of a galvanic cell made of lead and cadmium. Then determine the non-standard cell potential (Ecell) if the molarity of the cadmium solution was 0.20 M, and the molarity of the lead solution was 0.10 M. The temperature of the cell is 300 K. Cd2+(aq) + 2e– → Cd(s) E° = –0.403 V Pb2+(aq) + 2e– → Pb(s) E° = –0.126 V E°cell = ______________ Ecell = ______________
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Nit] = 0.00170 M and [Au] = 0.868 M. Standard reduction potentials can be found in this table. %3D 3 Ni(s) + 2 Au*(aq) 3 Ni?+(aq) + 2 Au(s) E = V
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2+ Cu²+ (aq) + 21 (aq) → Cu(s) + I₂ (s) From the table of standard reduction potentials: Cu²+/Cu 0.337 V, E₁₂/1 Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K:I AGO for this reaction would be than zero. = = 0.535 V
The cell potential for a voltaic cell composed of zinc and copper is 1.0 V under standard conditions. Zn(s) + Cu2+(aq) => Cu(S) + Zn2+(aq) What is the cell potential when one of the following deviations from standard conditions are made? A) [Zn2+] = 0.25 M; [Cu2+] = 0.25 M B) [Zn2+] = 0.25 M; [Cu2+] = 0.50 M C) [Zn2+] = 0.75 M; [Cu2+] = 0.75 M D) [Zn2+] = 0.75 M; [Cu2+] = 0.25 M E) [Zn2+] = 0.25 M; [Cu2+] = 0.75 M
This galvanic cell uses the reaction: Cu(s) + 2 Ag*(aq) → 2 Ag(s) + Cu2+(aq). f a C oxidation half cell reduction half cell Identify the composition of electrodes and the direction of electron flow. O a is Ag, c is Cu and electrons flow from c to a O a is Ag, c is Cu and electrons flow from a to c O a is Cu, c is Ag and electrons flow from c to a. O a is Cu, c is Ag and electrons flow from a to c. an
Gibbs free energy= -434250 J/mol for a galvanic cell whose two half-reactions: Mt3+ (aq) + 3 e1- → Mt (s), and R2+ (aq) + 2 e1- → R (s), have standard reduction potentials of 1.09 V and 0.34 V respectively

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Calculate the value of the cell potential, E cell for the following reaction: 2 Au(s) + 3 Ca2+(aq)- →2 Au3+(aq) + 3 Ca(s) O-1.26 V -11.3 V + 4.26 V -4.26 V +1.26 V