Mn²+ + 2e - Mn e° = -1.18 V Fe2+ + 2e¯ - Fe e° = -0.44 V a. Determine the overall cell reaction and calculate el: (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it + Ecell b. Calculate AG° and K for the cell reaction at 25°C. AG° = kJ K = c. Calculate ecell at 25°C when Mn2+ = 0.10 M and Fe²+ = 1.5 x 10-5 M. Ecell =

Mn²+ + 2e - Mn e° = -1.18 V Fe2+ + 2e¯ - Fe e° = -0.44 V a. Determine the overall cell reaction and calculate el: (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it + Ecell b. Calculate AG° and K for the cell reaction at 25°C. AG° = kJ K = c. Calculate ecell at 25°C when Mn2+ = 0.10 M and Fe²+ = 1.5 x 10-5 M. Ecell =

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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The overall reaction and equilibrium constant value for a hydrogen-oxygen fuel cell at 298 K is given below. 2 H₂(g) + O₂(g) – 2 H₂O(l) K = 1.34×1083 (a) Calculate 8º and AG° at 298 K for the fuel-cell reaction. V Cº AGº (b) Predict the signs of AH° and ASº for the fuel-cell reaction. AH°: O O O O AS°: positive negative positive negative (c) As temperature increases, does the maximum amount of work obtained from the fuel-cell reaction increase, decrease, or remain the same? Explain. as T increases. Since AS is ---Select--- ŷ as T increases, AG becomes more ---Select--- ŷ Therefore, the maximum work obtained will ---Select--- Need Help? Read It Supporting Materials Periodic Table I Constants & Factors Supplemental Data
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Consider the galvanic cell based on the following half-reactions: Mn2+ + 2e → Mn ɛ° -1.18 V Cd2+ + 2e –→ Cd e° : -0.40 V = a. Determine the overall cell reaction and calculate cell · (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + + E cel b. Calculate AG° and K for the cell reaction at 25°C. AG° kJ K C. Calculate Ecell at 25°C when Ma*] Ca*+ = 1.2 Mn²+ - 0.10 М and x 10-5 М. Ecell =
Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd²+ + 2e →→ Cd (a) Determine the overall cell reaction and calculate º chemPad XX² cell 8° = +0.80 V 8⁰ = -0.40 V V AGO K Help Greek (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. kJ (in V). (Use the lowest possible whole number coefficients. Omit states-of-matter from your answer.) cell (c) Calculate cell (in V) at 25°C when [Ag+ ] = V 1.0×10-4 M and [Cd²+] = 1.0×10-² M.
11. What is AG° for the reaction driving the following voltaic cell? Co (s) | Co²+ (aq) || Mn³+ (aq), Mn²+ (aq) | Pt (s) A. -175 kJ +175 kJ B. -351 kJ +351 kJ C. -527 kJ D. E.
Given the following two half-reactions, determine which overall reaction is spontaneous, and calculate its standard cell potential. Cd2*(aq) + 2 e- Cd(s); E° = -0.403 V Zn2"(aq) + 2 e-Zn(s); E° = -0.763 V O A. Cd(s) + Zn2*(aq) OB. Cd(s) + Zn(s)¯ OC. ca²*(aq) + Zn²*(aq)' Cd2+(aq) + Zn(s); E° = -0.360 V Cd2*(aq) + Zn²+(aq); E° = -1.166 V PCd(s) + Zn(s); E° = +1.166 V O D. Cd2+(aq) + Zn(s) cd(s) + Zn2*(aq); E° = +0.360 V
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG° for the following redox reaction. Round your answer to 4 significant digits. L (s) + 6H,0 (1) +5Zn²™ (aq) → 21IO, (aq)+ 12H" (aq)+ 5Zn (s) |kJ x10
Determine electromotive force for the cell represented by: Fe (s) | FeSO4(0.30 M) || KIO3(0.50 M), l2(s), pH 4.0 | Pt(s) Given: Fe2+ + 2 e --------- Fe (s) Eo = - 0.44 Fe3+ + e ------ Fe2+ Eo = 0.771 V IO3- + 6 H+ + 5e ------ ½ I2(s) + 3 H2O (l) E0 = 1.210 V A. 1.346 V B. 0.166 V C. 1.376 V D. 0.498 V E. 1.660 V
The electrochemical cell notation for the non-standard cell (assumed to be voltaic cell) below is correctly written. Ag(s) | AgCl(s) | Ag (sat'd), Cl- (sat'd) || Ag+ (1.0 M) | Ag(s) The Ksp of AgCl is 1.8x10-¹⁰, Select one: O True O False
The following reaction is non-spontaneous as written when the components are in their standard states, the cell potential is -0.16 V. Which of the following is true? Co(s) + Fe²*(aq) 2 Co²* (aq) + Fe(s) E =-0.16 V A. the reaction is spontaneous if [Co2+/[Fe2+] > 3.91x10-6 В. the reaction is spontaneous if [Co2+]/[Fe2+] -6 C. the reaction is spontaneous if [Co2+/[Fe2*] > 2.56x105 D. the reaction is spontaneous if [Co2*]/[Fe2+] 5
For the galvanic cell: Zn(s) + 2TI*(aq) 2TI(s) + Zn2*(aq) What is E°cel? Standard Electrode Potentials: Zn2*(aq) + 2e Zn(s) E° = -0.76 V TI*(aq) + eTI(s) E° = -0.34 V O 0.42 V O -0.42 V O 1.1 V O -1.1 V