7. Determine the cell potential (in V to two decimal places) for the following electrochemica cell: 2+ Cu(s) | Cu²+ (aq, 0.02 M) || Cu²+ (aq, 0.50 M) | Cu(s) A: 0.04

1) Write the two half reactions and the overall reaction and determine the standard cell potential 2) Is this cell more or less spontaneous at the nonstandard conditions?

In a standard electrochemical cell, A4+ is reduced to solid A, while gaseous Z2 is oxidized to Z3-. Calculate the standard cell potential (in V) if its equilibrium constant is 2.23x1054 (Use R = 8.314 J/mol-K; F = 96485 C/mol) Express your answer with 3 decimal places and do not encode the units. If negative, include the sign in your encoded answer.

Calculate the actual cell potential (E) at 25.0 oC for the following redox reaction when the ionconcentrations are: [Br−] = 0.0500 M, [Cr2O72−] = 0.100 M, [H+] = 0.0100 M, and [Cr3+] = 0.0250 M.(HINT: Liquid-phase species do not appear in reaction quotient (Q) expressions.) 6 Br− + Cr2O72− + 14 H+ 2 Cr3+ + 7 H2O(l) + 3 Br2(l)

Which of the following statements is true for the electrochemical cell below at 25oC? Cu(s)|Cu2+(aq, 1.5 M)||Ag+(aq, 0.25 M)|Ag(s) The standard cell potential, E0cell, is equal to 0 at equilibrium. When the cell reaches equilibrium, the reaction quotient, Q, is equal to the equilibrium constant, K, and the cell will no longer work. Ecell can be determined by using the standard half-cell potentials alone. This cell is operating under standard conditions.

Calculate the non-standard cell potential (in V) for the following reaction at 65.86 ℃ with the following concentrations: [Mg+2Mg+2] = 1.00×10−71.00×10-7 M; [Cu+2Cu+2] = 5.522 MCu+2Cu+2(aq) + Mg(s) --> Cu(s) + Mg+2Mg+2(aq)

Calculate the cell potential of the following cell at 25°C. Cr(s} | C* (1.0 X'10° M) || Ni²* (1.5 M) IÑI (s) 6.

Write the overall cell reaction for the galvanic cell given below. Pt(s) | Sn2+(aq), Sn4+(aq) || Fe3+(aq) | Fe(s)

what is the standard cell potential (in Volts) for a a galvanic cell that can do 567 kJ of work. The number of electrons tranferred in the rxn is 4.

Calculate Ecell for the following electrochemical cell at 25 °CPt(s) | Fe3+(aq, 0.100 M), Fe2+(aq, 0.040 M) || Cl–(aq, 0.50 M) | AgCl(s) | Ag(s)given the following standard reduction potentials.   AgCl(s) + e– → Ag(s) + Cl–(aq) E° = +0.222 V   Fe3+(aq) + e– → Fe2+(aq) E° = +0.771 V