A two electron redox reaction has a redox potential E' = 0.58 V. Given Faraday's constant...
The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by the equation Fe(s) + Ni+ (aq) +Fe?+ (aq) + NI(s) FE In K = Express your answer numerically. View Available Hints) where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mole). R (the gas constant) is equal to 8.314 J/(mol-K). and T is the Kelvin temperature. ΟΙ ΑΣΦ h ? KK- Submit Previous Answers *...
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.
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...
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...
Based on the given standard free energy change and electron stoichiometry values below, calculate a corresponding standard cell potential. AG°= -4.5 kJ/mol, n = 1, F = 96485 J/mol O El-0.047 V O Edel = -4.5V El=+0.047V
Review I Constants I Periodic Table The equilibrium constant, K, for a redox reaction is related to the standard potential, E°, by the equation Standard reduction potentials nFE RT In K E° (V) Reduction half-reaction Agt(aq)eAg(s) Cu2+(aq)2eCu(s) 0.80 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. 0.34 Sn4t (aq)4eSn(s) 0.15...
A student made measurements on some electrochemical cells and calculated three quantities 0 The standard reaction free energy AG . The equilibrium constant K at 25.0 °C 0 The cell potential under standard conditions E. His results are listed below Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any Note: If there is a mistake in a row, only one of the three...
Cell Potential and Equilibrium Standard reduction potentials The equilibrium constant, K, for a redox reaction is related to the standard cell potential, Ecel, by the equation Reduction half-reaction (V) Ag+ (aq) + e-→Ag(s) Cu2+ (aq) + 2e-→Cu(s) 0.34 Sn (a) 4e-Sn(s 0.15 2H' (aq) + 2e-→H2 (g) Ni2+ (aq) + 2e-→Ni(s)-0.26 Fe2+ (aq) + 2e-→Fe(s)-0.45 Zn2+ (aq) + 2e-→Zn(s)-0.76 Al3+ (aq) +3e-→Al(s) -1.66 Mg2+ (aq) + 2e-→Mg(s) -2.37 0.80 n FEcell where n is the number of moles of electrons...
Calculate the standard change in Gibbs free energy, AGixn , for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH,CI() = NH(aq) + Cl(aq) AGxn = -7.7 kJ/mol Determine the concentration of NH(aq) if the change in Gibbs free energy, AGrxn , for the reaction is –9.53 kJ/mol. [NH] = 0.72 Consider a general reaction enzyme A(aq) = B(aq) The AG® of the reaction is -4.880 kJ mol-....
CU PIULUOS LO UCCU 30. Based on the given standard free energy change and electron stoichiometry values below, calculate a corresponding standard cell potential. AG°= 12 kJ/mol, n=3 A. Eceu=0.041 V B. Eceu= +0.047 V C. Eceu=-0.041 V D. Eceu= -0.047 V