Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350 K....
7. Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350K(a) \(\quad A g^{\prime}(a q)+M g(s) \leftrightharpoons A g(s)+M g^{2 *}(a q)\)(b) \(\mathrm{Cu}^{2 \cdot}(\mathrm{aq})+\mathrm{OH}(\mathrm{aq}) \div \mathrm{Cu}^{+1}(\mathrm{aq})+\mathrm{O}_{3}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(1)\)(c) \(\quad \mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})+\mathrm{Fe}^{+1}(\mathrm{aq}) \leftrightarrows \mathrm{Fe}^{-2}(\mathrm{aq})+\mathrm{Mg}(\mathrm{s})+\mathrm{OH}^{-1}(\mathrm{aq})\)8. Complete the following table and comment on the spontancity each reaction.
can you find this answer at 350K? I know how to find it at
standard conditions! Thanks!
7. Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350 K. AG = -nfeo Ag+ (aq) + Mg(s) S Ag(s) + Mg(aq) (a)
2. Calculate the standard cell potential for each of the following redox reactions, and then predict whether each will occur spontaneously as written. a. Sr(s) + Fe2+(aq) → Sr2+ (aq) + Fe(s) b. 2Cr(s) + 3Cd2+ (aq) → 2Cr3+ (aq) + 3Cd(s) 3. Calculate the standard cell potential, Eºcell, for each of the voltaic cells in Part II of the experiment. a. Zn(s) | Zn2+ (aq, 1.0 M) || Cu2+ (aq, 1.0 M) Cu(s) b. Zn(s) | Zn2+(aq, 1.0 M)...
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...
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...
A voltaic cell employs the following redox reactions. 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions. (a) [Fe3+]= 1.0×10−3 M ; [Mg2+]= 2.05 M (b) [Fe3+]= 2.05 M ; [Mg2+]= 1.0×10−3 M
The standard reaction Gibbs energy for the redox process listed below is -206 kJ mol-1. Calculate the standard cell potential. MnO4-(aq) + NO(g) ⟺ MnO2(s) + NO3-(aq) Given these two half-rxns: MnO4-(aq) + 4 H+(aq) + 3 e-⇔ MnO2(s) + 2 H2O(l) NO(g) + 2 H2O(l) ⇔ NO3-(aq) + 4 H+(aq) + 3 e-
Consider the following redox reactions. For each reaction, calculate the standard cell potential. See Table 12-2 from your book for a list of standard reduction potentials (or lecture notes CH12). A. Ag+ + Fe2+à Fe3+ + Ag(s) B. Zn2+ + Ni(s) à Ni2+ + Zn(s) C. 2Al3+ + 3Cu(s) à 2Al(s) + 3Cu2+
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...
When the following redox reaction is carried out in a voltaic cell, the standard cell potential, E°cell, is 0.93 V. What is ΔG° for this reaction at a temperature of 298.15 K? Pb(s) + 2 Ag+(aq) → Pb2+(aq) + Ag(s) A. -180 kJ B. -90 kJ C. 90 kJ D. 180 kJ