Given the following half-reactions and their standard reduction potentials,2CIO,- + 12H+ + 10e Cl, + 6H2OEao,- = 1.47 VS,0,2- + 2e= 2S0,2-Eo = 2.01 Vcalculate the following:(a) E° cell for the reaction:E° cell(b) AG° for the cell reaction:x 10kJ(c) the value of K. for the cell reaction:x 10

E0ClO32- =1.47 V E0S2O82- = 2.01 V E0 cell = E0S2O82- -E0ClO32- = 2.01 - 1.47 = 0.54 V

Given the following half-reactions and their standard reduction potentials, 2CIO;- + 12H* + 10e Cl,+ 6H2O Eao- = 1.47 V %3D S,0,2- + 2e=2S0,- Eo = 2.01 V calculate the following: (a) E° cell for the reaction: E° cell V %3D (b) AG° for the cell reaction: x 10 (c) the value of K, for the cell reaction: x 10

Given the following half-reactions and their standard reduction potentials, 2CIO;- + 12H* + 10e Cl,+ 6H2O Eao- = 1.47 V %3D S,0,2- + 2e=2S0,- Eo = 2.01 V calculate the following: (a) E° cell for the reaction: E° cell V %3D (b) AG° for the cell reaction: x 10 (c) the value of K, for the cell reaction: x 10

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...

See similar textbooks

Similar questions

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.
A redox reaction used in an electrochemical cell has a negative standard free energy change, AGxn- Which statement about the redox reaction is true? O Ecel is positive; K 1 E'cel is negative; K 1 'cell
What statement about a galvanic cell constructed with Cu*/Cu and Fe2*/Fe is correct? Standard reduction E°red, V potentials Cu* + e ---> Cu +0.52 Fe2+ + 2e ---> Fe |-0.44 O Fe2*(aq) is reduced at the cathode. O Fe(s) will reduce Cu*(aq). Fe(s) is a stronger oxidizing agent than Cu(s). O The standard cell potential (E°cell) is +1.40 V.
If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 2 significant digits.
Consider the following cell: | Zn (s) | Ca2* (aq) , SO3²- (aq) || Hg²+ (aq) , F' (aq) | Pt (s) | al Indiate the Oxidizing Agent bindicate the ReducingAge Gont e Wnte he narreattions that occurs ai the cathode d) Write the half reactions that occurs at the anode e) Write the overall net cell reaction f) Calculate the cell potential g) Indicate if electricity is produced or consumed by the cell h) Indicate if the cell is galvanic or electrolytic
What mass of Fe(s) may be deposited from an aqueous FeCl2 solution if a current of 2.50 A is applied to the solution for 365 s? (ε°red(Fe2+/Fe) = -0.447 V, F = 96485 C/mol)
ii. A galvanic system consists of Ni/Ni2+ and Co/Co²+ half-cells. Determine which half-cell is getting reduced, which one is getting oxidized and the electrochemi- cal cell potential Ecell if a) [Co²+] = 0.1 mol L-¹, [Ni²+] = 1 mol L-¹ and b) [Co²+] = 1 mol L-¹, [Ni²+] = 0.005 mol L´¹.
You are given the following three half-reactions
Given the following standard reduction half reactions calculate the standard cell potential (E°cell) to 2 decimal places. O2(g) + 4H+ + 4e" 1 4H* (aq) 2H20L) ; E°red. = 1.23 V A13+ (aq) + Зе Al(s) ; E°red. = -1.66 V