Determine the standard cell potential: A (s) A5 + (ac) || B5 + (ac) | B (s), using the following standard reduction potentials.
reduction reaction E ° (V)
AS + (ac) + 5 e- A (s) -0.362
BS * (ac) + 5 e- → B (s) -0.275
Determine the standard cell potential: A (s) A5 + (ac) || B5 + (ac) | B...
Determine the standard potential (at 25 ° C) of the cell: A (s) | A5 + (ac) || B3 + (ac) | B (s), if [AS +] = 1.91 M and [B³ *] = 0.81 M. Use the following standard reduction potentials. reduction reaction. E ° (V) A5 + (ac) + 5 e- A (s) 0.039 B3 + (ac) + 3 e - B (s) 0.577
Determine the value of AGº for the following reaction if the standard potential of the cell where that reaction occurs is E = +1.08 V. 2 Cr (s) + 3 Cu2+ (ac) → 2 Cr3+ (ac) + 3 Cu (s) A. -2.08 x 102 kJ/mol B. -6.25 x 102 kJ / mol C. -3.13 x 102 kJ/mol D. -4.17 x 102 kJ / mol E. -5.21 x 102 kJ/mol
Use the standard half-cell potentials listed below to calculate the standard cell potential and standard free energy Gº) for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.) k(aq) + e-K(5) E* --2.93 V 12(s) + 2 0 - 2 (aq) E*-+0.54V a. +6.40 V & 670 KJ b. +1.85 V & 487K] C. 3.47 V & 241 Kb d. 3.47 V8 - 6709 e.+5,32 V &-+670K)
Using tabulated standard reduction potentials from your text, calculate the standard cell potential, E degree_cell (always positive for a galvanic cell), based on the following reaction: Cu^2+ (aq) + Mg(s) Mg^2+ (aq) + Cu(s) A galvanic cell based on the above reaction is constructed according to the generic sketch of a galvanic cell shown below:
Calculate the cell potential for the galvanic cell in which the reaction Fe(s)+Au3+(aq)−⇀↽− Fe3+(aq)+Au(s) occurs at 25 ∘C , given that [Fe3+]=0.00150 M and [Au3+]=0.795 M . Refer to the table of standard reduction potentials. E= V
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25�C. (The equation is balanced.) Sn(s) + 2 Ag+(aq) ? Sn2+(aq) + 2 Ag(s) Sn2+(aq) + 2 e- ? Sn(s) E� = -0.14 V Ag+(aq) + e- ? Ag(s) E� = +0.80 V a)-1.08 V b)+1.74 V c)-1.74 V d)+0.94 V e)+1.08 V
Maximum Standard Single Cell Potential Under standard conditions, what is the maximum single cell potential that might be attained using reagents found in the table of standard reduction potentials for common half-reactions, in your text? Note: 7.5 V is not the correct answer
Data Analysis Questions Q1. Complete Table 8.2 below. Using a standard half-cell potential of 0.34 V for Cu2*/Cu, calculate the experimental reduction potentials for Mg, Pb, Sn, and Zn half-cells. Obtain standard reduction potentials from a suitable reference source. Show all of your work below and RANK the metals in terms of oxidizing and reducing ability according to the experimental half-cell potentials. (3.0) Table 8.2 Half-cell reduction reaction (include phase labels) Calculated E (v) Literature E (V) Culaq) + 2e...
First fill in your half cell and cell reactions. F in standard cell potentials as you calculate them. Oxidation at the Anode: The black (.) lead is attached to the electrode, which is the source of electrons. Write the anode half reaction: Reduction at the Cathode: The red lead (+) is attached to the electrode. Write the cathode half reaction: E degree - V. Overall Cell Reaction (Net Ionic equation): Write the overall cell reaction (balance electrons and add together):...
Determine the standard cell potential (in volts) at 25 degree C for the following reaction. You will need to look up the relevant reduction potentials in your textbook. 3 Cu^2+ _(aq) + 2 Al_(s) rightarrow 2 Al^3+ _(aq) + 3 Cu_(s) TRUE or FALSE: The above reaction is non-spontaneous and would need the input of electricity to move forward as an electrolytic cell. True False