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Calculate the standard free energy change, ΔG°, for the following redox reaction if the standard reduction potential of Ag⁺/Ag is +0.80 V and the standard reduction potential of Cu²⁺/Cu is +0.34 V:Ag⁺(aq) + Cu(s) → Ag(s) + Cu²⁺(aq)

asked Feb 3 in Chemical thermodynamics by Broderick659 (410 points)

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Calculate the standard free energy change, ΔG°, for the following redox reaction at 298 K:2Fe3+(aq) + 2I-(aq) → 2Fe2+(aq) + I2(s)The standard reduction potential values for Fe3+ and Fe2+ are -0.037 V and -0.44 V respectively, while the standard reduction potential value for I2 is 0.535 V.

asked Feb 3 in Chemical thermodynamics by LawrenceBuck (450 points)

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Calculate the standard free energy change for the redox reaction: Fe2+(aq) + Sn4+(aq) → Fe3+(aq) + Sn2+(aq)Given: E°Fe3+/Fe2+ = 0.771 V E°Sn4+/Sn2+ = 0.150 V R = 8.314 J/K·mol T = 298 K

asked Feb 3 in Chemical thermodynamics by RickieTretho (290 points)

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Calculate the standard free energy change for the redox reaction: 2Fe^3+(aq) + H2(g) --> 2Fe^2+(aq) + 2H^+(aq) Given the following standard reduction potentials: Fe^3+(aq) + e^- --> Fe^2+(aq) E° = +0.771 V 2H^+(aq) + 2e^- --> H2(g) E° = 0.000 V

asked Feb 3 in Chemical thermodynamics by RandalLauren (610 points)

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Calculate the standard free energy change for the reaction of HCl with MnO2 to form MnCl2 and H2O at a temperature of 298 K, given that the standard reduction potentials are E°(MnO2/MnCl2)=-0.13 V and E°(H2O/HCl)=1.23 V.

asked Feb 3 in Chemical thermodynamics by ChristoperGa (630 points)

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Calculate the standard free energy change for the following redox reaction:2HgO(s) → 2Hg(l) + O2(g)Given: ΔG°f (HgO) = -90.83 kJ/molΔG°f (Hg) = 0 kJ/mol ΔG°f (O2) = 0 kJ/mol.

asked Feb 3 in Chemical thermodynamics by EdwinCamidge (450 points)

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Calculate the standard free energy change for the following redox reaction:2Fe^2+ (aq) + H2O2 (aq) + 2H+ (aq) -> 2Fe^3+ (aq) + 2H2O (l) Given the following reduction potentials at standard conditions:Fe3+ (aq) + e- -> Fe2+ (aq) E° = 0.77 VH2O2 (aq) + 2H+ (aq) + 2e- -> 2H2O (l) E° = 1.78 V

asked Feb 3 in Chemical thermodynamics by EddyConnery6 (570 points)

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Calculate the standard free energy change for the following redox reaction: Balanced Chemical Equation: 2Fe3+(aq) +3H2O2(aq) → 2Fe2+(aq) + 3O2(g) + 6H+(aq)Given data: Standard reduction potential of Fe3+/Fe2+ = +0.77 V Standard reduction potential of H2O2/O2 = +0.70 V

asked Feb 3 in Chemical thermodynamics by AlexisHooten (590 points)

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Calculate the standard free energy change for the following redox reaction under standard conditions:2 Fe3+ (aq) + H2 (g) → 2 Fe2+ (aq) + 2 H+ (aq)Given: Standard reduction potential of Fe3+ / Fe2+ = -0.771 V Standard reduction potential of H+ / H2 = 0.00 V

asked Feb 3 in Chemical thermodynamics by JosephDelato (310 points)

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Calculate the standard free energy change for the following redox reaction at 298 K:2 Mg(s) + O2(g) -> 2 MgO(s)(The standard reduction potential for Mg2+/Mg is -2.37 V and for O2/H2O is +1.23 V)

asked Feb 3 in Chemical thermodynamics by DeneseHamble (530 points)

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Calculate the standard free energy change for the following redox reaction at 298 K:Mg(s) + 2H+(aq) -> Mg2+(aq) + H2(g)Given: Eºred for Mg2+/Mg = -2.37 V & Eºred for H+/H2 = 0 V.

asked Feb 3 in Chemical thermodynamics by Manie9252773 (490 points)

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Calculate the standard free energy change for the following redox reaction at 25°C:2Fe(s) + 3/2 O2(g) -> Fe2O3(s)Given the following half-reactions and their standard reduction potentials at 25°C:Fe2O3(s) + 3H2O(l) + 2e- -> 2Fe(OH)3(s) E°= -0.33VO2(g) + 4H+(aq) + 4e- -> 2H2O(l) E°= +1.23VFe(OH)3(s) -> Fe3+(aq) + 3OH-(aq) E°= -0.25V

asked Feb 3 in Chemical thermodynamics by GitaDangelo (450 points)

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Calculate the standard free energy change (ΔG°) for the redox reaction:Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s) Given that the standard reduction potentials of Cu2+(aq)/Cu(s) and Ag+(aq)/Ag(s) are +0.34V and +0.80V, respectively.

asked Feb 3 in Chemical thermodynamics by BrandenBreez (360 points)

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Calculate the standard free energy change (ΔG°) for the following redox reaction: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g)Given: ΔG°f (Zn2+) = -153.9 kJ/mol ΔG°f (H+) = 0 kJ/mol ΔG°f (H2) = 0 kJ/mol ΔG°f (Zn) = 0 kJ/mol

asked Feb 3 in Chemical thermodynamics by CherylYoul4 (350 points)

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Calculate the standard free energy change (ΔG°) for the following redox reaction at 298K:Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) (Given: E°cell = 1.10V, F = 96,500 J/V.mol)

asked Feb 3 in Chemical thermodynamics by GlennaPark6 (550 points)

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Calculate the standard free energy change (ΔG°) for the following redox reaction at 298 K, given that E°cell = 0.91 V:Zn(s) + 2 Ag+(aq) → Zn2+(aq) + 2 Ag(s)

asked Feb 3 in Chemical thermodynamics by TrevorMcClin (310 points)

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Calculate the standard free energy change (ΔG°) for the following reaction at 25°C: 2Fe2+(aq) + Cu2+(aq) -> 2Fe3+(aq) + Cu+(aq) (Standard reduction potentials: Fe3+(aq) + e- -> Fe2+(aq) E° = 0.77 V Cu2+(aq) + e- -> Cu+(aq) E° = 0.16 V)

asked Feb 3 in Chemical thermodynamics by DeangeloGree (150 points)

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Calculate the standard free energy change (∆G°) for the reaction: 2CH4(g) + 3O2(g) → 2CO2(g) + 2H2O(l) at 298 K, given that the standard enthalpy change (∆H°) of the reaction is -890.4 kJ mol^-1 and the standard entropy change (∆S°) of the reaction is +292.2 J K^-1 mol^-1. Is the reaction spontaneous or non-spontaneous under standard conditions?

asked Feb 3 in Physical Chemistry by BradKeeney1 (420 points)

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Calculate the standard free energy change (∆G°) for the following redox reaction at 25°C:2 Fe³⁺(aq) + 3 H₂(g) → 2 Fe(s) + 6 H⁺(aq)

asked Feb 3 in Chemical thermodynamics by JaquelineQue (350 points)

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Calculate the standard entropy change of the following reaction: 2Fe(s) + 3Cl2(g) → 2FeCl3(s) Given that the standard enthalpy change for this reaction is -400 kJ/mol at 298 K and the standard molar entropy of FeCl3(s) is 95 J/mol K.

asked Feb 3 in Inorganic Chemistry by DarwinSanjua (370 points)

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