An aqueous CeF3 solution is electrolyzed under 1 bar pressure using platinum electrodes. Write the half-reactions predictedto occur at the anode and cathode, based on the standard cell potentials given below.Standard Reduction Potentials (Volts) at 25 °CF2+2 e 2 FO2 + 4 H3O++ 4 e6 H₂O2 H2O + 2 eH2 + 2 OHCe3+ + 3 e― Ce2.8701.229-0.828-2.335Enter electrons as e. Use the smallest integer coefficients possible. If a box is not needed leave it blank.Half-reaction at anode:Half-reaction at cathode:→+

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Answered: An aqueous CeF3 solution is…

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 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 =
A student wanted to measure the concentration of cobalt(II) ion in an aqueous solution. For the cathode half-reaction, she used a silver electrode with a 0.51 M solution of AgNO3. For the anode half-reaction, she used a cobalt electrode dipped into the aqueous solution. If the cell gave a potential of 1.043 V at 25 °C, what was the concentration of Co2+ in the solution? Half-reaction E° (V) Ag*(aq) + e- Ag(s) +0.7996 Co2+(aq) + 2 e- -0.28 Co(s) Your Answer: Answer units
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)
Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- → La (s) E° = -2.37 V Na+ (aq) + e- → Na (s) E° = -2.71 V 1.8 x 10-6 5.7 x 10-18 5.6 x 105 1.7 x 1017
A galvanic cell is constructed as follows. One half-cell consists of a platinum wire immersed in a solution containing 1.00 M Sn2+ and 1.00 M Sn4+. The other half-cell has a thallium rod immersed in a solution of 1.00 M Tl+. What is the equilibrium constant at 25° C?(Eo= Tl+ / Tl = −0.34 V.)? What is the cell voltage if the Tl+ concentration is increased 6−fold?
A standard hydrogen electrode has a half-cell reduction potential of zero at 25 C. Calculate the potential of the half-cell when the pH is 3.8 and the pressure of H2 is 4.6 bar.
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. An aqueous ScCl3 solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C Ch(g) + 2 e → 2 Cl'(aq) 1.360 02(g) + 4 H30*(aq) + 4 e» 6 H2O() 1.229 2 H2O(1) + 2 e– H2(g) + 2 OH (aq) -0.828 Sc*(aq) + 3 e - Sc(s) -2.080 Half-reaction at anode: Half-reaction at cathode: (b) What is the expected decomposition potential? V +
Is there a minimum or maximum standard reduction potential that the half-reaction can have. Then write the balanced equation

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