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If the equilibrium constant for a two electron redox reaction at 198 °C is 1500, calculate...
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.
Calculate Eocell for a two-electron redox reaction if the equilibrium constant is 4.1 x 1015 at 298 K.
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.
A two electron redox reaction has a redox potential E' = 0.58 V. Given Faraday's constant F = 96,500 J/mol, calculate the standard Gibb's free energy change AG in kJ (to three significant figures) for the reaction.
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.
7. (8 pts) If the equilibrium constant for a three-electron redox reaction at 298 K is 7.0x104 calculate the corresponding ?Go and -cell.
6. Calculate the equilibrium constant (K) for the following redox reaction at 25 ?C. Ecell = -0.71 V 2 Al(s) + 3 Mg2+(aq) --> 2 Al3+(aq) + 3 Mg(s