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Calculate the standard potential, Eº, for this reaction from its AGⓇ value. X(s) + y4+ (aq)...
Calculate the standard potential E°, for this reaction from its ΔG° value. X(s)+Y4+(aq)⟶X4+(aq)+Y(s)ΔG°=97.0 kJ
Question 5 of 16 Calculate the standard potential, E“, for this reaction from its AGⓇ value. X(s) + Y3+ (aq) — X3+(aq) + Y(s) AGⓇ = 61.0 kJ E V
Calculate the standard potential, Eº, for this reaction from its equilibrium constant at 298 K. X(s) + y2+(aq) = x2+(aq) + Y(s) K = 9.95 103 E = V
Calculate the standard potential, E®, for this reaction from its equilibrium constant at 298 K. X(s) +Y4+ (aq) = X4+ (aq) + Y(s) K = 7.92 x 10-8 E =
For the reaction 2Al(s) + 3C0(aq) 2A1* (aq) + 3C0(S), AGⓇ is -799 kJ. What is Eº for a standard cell based on this reaction? Seleccione una: a. +2.76 V b. +1.38 v C. +4.14 V d. +8.28 V
Consider the following reaction and its AGⓇ at 25 °C. Mg(s) + Ni2+(aq) — Mg2+(aq) + Ni(s) AG° = -408.0 kJ/mol Calculate the standard cell potential, Ecell, for the reaction. Fo Celi Calculate the equilibrium constant, K, for the reaction.
Consider the following reaction and its AGⓇ at 25.00 °C. Mg(s) + Ni2+ (aq) + Mg2+(aq) + Ni(s) AG° = -408.0 kJ/mol Calculate the standard cell potential, Ecell, for the reaction. Begin = 2.11 Cell Calculate the equilibrium constant, K, for the reaction. K K = =
Calculate the standard cell potential (°) for the reaction X(s) +Y+ (aq) +X+ (aq) +Y(s) if K = 2.88x10-3 Express your answer to three significant figures and include the appropriate units. View Available Hint(s) E' - -.134 V Submit Previous Answers X Incorrect; Try Again; 3 attempts remaining
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where n is the number of moles of electrons transferred and F = 96,500 C/(mol e ) is the Faraday constant. When Eº is measured in volts, AGⓇ must be in joules since 1 J =1C.V. Part A Calculate the standard free-energy change at 25°C for the following reaction: Mg(s) + Fe2+ (aq)Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include...
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE° RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol · K), and T is the Kelvin temperature. Standard reduction potentials Reduction half-reaction E° (V) Ag+ (aq) + e +Ag(s) 0.80 Cu²+ (aq) + 2e + Cu(s) 0.34...