7. (8 pts) If the equilibrium constant for a three-electron redox reaction at 298 K is...
If the equilibrium constant for a one-electron redox reaction at 298 K is 7.9×104, calculate the corresponding ΔG∘ and E∘cell. A. ΔG∘= ? kJ B. E∘cell= ? V Please explain this problem to me. Thanks.
If the equilibrium constant for a two-electron redox reaction at 298 K is 1.4×10−4, calculate the corresponding ΔG∘ and E∘cel under standard conditions.
Calculate Eocell for a two-electron redox reaction if the equilibrium constant is 4.1 x 1015 at 298 K.
Calculate ΔG∘rxn and E∘cell for a redox reaction with n = 1 that has an equilibrium constant of K = 25. (Temperature is 298 K.
If the equilibrium constant for a two electron redox reaction at 198 °C is 1500, calculate the ΔG° and E0red.
If the equilibrium constant for a two electron redox reaction at 198 oC is 1500, calculate the ΔG° and E0red.
If the equilibrium constant for a two electron redox reaction at 198 oC is 1500, calculate the ΔG° and E0red.
If the equilibrium constant for a two electron redox reaction at 198 oC is 1500, calculate the ΔG° and E0red.
cell = 0.74 V. Calculate the equilibrium constant, K. For the following redox reaction at 25 °C, E° Cd(s) + Cu 2+ (aq) → Cd 2+ (aq) + Cu(s)
The equilibrium constant, K, for a redox reaction is related to the standard potential, E∘, by the equation lnK=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. Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 5.51×10−3.