Free-energy change, ΔG∘, is related to cell potential, E∘, by the equation
ΔG∘=−nFE∘
where n is the number of moles of electrons transferred and F=96,500C/(mol e−) is the Faraday constant. When E∘ is measured in volts, ΔG∘ must be in joules since 1 J=1 C⋅V.
Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -679 kJ and ΔS∘ = -195 J/K .
Free-energy change, ΔG∘, is related to cell potential, E∘, by the equation ΔG∘=−nFE∘ where n is...
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...
Cell: Fe(s)| Fe2+(aq, 1M) | Cu2+(aq, 1M) | Cu(S) Calculated Values ΔG° = -nFE° = ΔH° - TΔS° ΔH° = -0.34905 J/C * 2 mols * 96485 C/mol = -67,356.18 J =67.36kJ ΔS° = 0.8597 x 10-3 J/C * 2 mols * 96485 C/mol = 165.89 J ΔG° =-67356.18 J – (298*165.9 J) = -116794.4 J = -116.79 kJ Theoretical Values ΔG⁰ = -(2 mols *96485 C/mol * 1.07 J/C) = -206.48 kJ ΔH⁰ = ΔS⁰ = Cell: Zn(s)| Zn2+(aq,...
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.
Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -627 kJ and ΔS∘ = -153 J/K .
Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -795 kJ and ΔS∘ = -349 J/K .
Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -829 kJ and ΔS∘ = -367 J/K
9. Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -725 kJ and ΔS∘ = -289 J/K .
Part B. Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -609 kJ and ΔS∘ = -373 J/K .
Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -923 kJ and ΔS∘ = -257 J/K . Express your answer to three significant figures and include the appropriate units. Calculate the standard cell potential at 25°C for the reaction X(s) +2Y+ (aq)+X2+ (aq) + 2Y(s) where AH = -923 kJ and AS = -257 J/K. Express your answer to three significant figures and include the appropriate units. View Available Hint(s) CO 2 ? E°...
Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔrH∘ = -799 kJ mol−1 and ΔrS∘ = -359 J K−1 mol−1 .