Recent questions in Chemistry

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Calculate the standard Gibbs free energy change for the following chemical reaction at 25°C:2H2(g) + O2(g) → 2H2O(l)The standard Gibbs free energy of formation at 25°C for H2O(l) is -237.2 kJ/mol, H2(g) is 0 kJ/mol, and O2(g) is 0 kJ/mol.

asked Feb 3 in Chemical thermodynamics by SZVRamon1645 (2.4k points)

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Calculate the standard Gibbs free energy change for the electrochemical reaction of zinc and copper ions: Zn(s) + Cu2+(aq) → Cu(s) + Zn2+(aq)Given the following standard electrode potentials: E°(Cu2+(aq) + 2e- → Cu(s)) = 0.34 V E°(Zn2+(aq) + 2e- → Zn(s)) = -0.76 V Assume standard conditions (25°C and 1 atm pressure) and that the concentrations of the copper and zinc ions are both 1 mol/L.

asked Feb 3 in ElectroChemistry by WallaceMaria (2.4k points)

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Calculate the standard Gibbs free energy change for the electrochemical cell reaction using the given half-reactions:Cu^2+(aq) + 2 e^- → Cu(s) E° = +0.34 VSn^4+(aq) + 2 e^- → Sn^2+(aq) E° = +0.15 VConstruct the cell diagram and identify the anode and cathode. Determine the overall cell potential and whether the reaction is spontaneous.

asked Feb 3 in ElectroChemistry by TiaraFitzgib (2.1k points)

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1 answer 157 views

Calculate the standard Gibbs free energy change (ΔG°) for the reaction below at 298 K:2NO(g) + O2(g) → 2NO2(g)Given:ΔG°f(NO2(g)) = -51.29 kJ/molΔG°f(NO(g)) = 86.67 kJ/molΔG°f(O2(g)) = 0 kJ/mol

asked Feb 3 in Physical Chemistry by Milagros70T7 (1.5k points)

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1 answer 143 views

Calculate the standard Gibbs free energy change (ΔG°) for the following electrochemical reaction:Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)Given: - Standard reduction potential for the half-reaction: Cu²⁺(aq) + 2e⁻ → Cu(s) E° = +0.34 V Ag⁺(aq) + e⁻ → Ag(s) E° = +0.80 V

asked Feb 3 in ElectroChemistry by EarleneKnott (1.5k points)

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1 answer 104 views

Calculate the standard Gibbs free energy change (ΔG°) for the electrochemical reaction of the reduction of copper ions (Cu2+) to copper atoms (Cu) using a copper electrode in a solution of copper sulfate (CuSO4) at 25°C. The standard reduction potential of the copper ion is +0.34 V.

asked Feb 3 in ElectroChemistry by CesarSpragg2 (2.1k points)

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1 answer 155 views

Calculate the standard Gibbs free energy change ($\Delta G^{\circ}$) for the following reaction at 298 K:2Fe(s) + 3/2O2(g) → Fe2O3(s) Given: Standard enthalpy of formation of Fe2O3(s) = -822.2 kJ/molStandard enthalpy of formation of Fe(s) = 0 kJ/molStandard entropy change for the reaction = +87.4 J/mol K

asked Feb 3 in Chemical thermodynamics by JackH2065356 (1.1k points)

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Calculate the standard free energy change, ΔG°, for the following redox reaction:2Fe2+ (aq) + H2O2 (aq) → 2Fe3+ (aq) + 2OH- (aq)Given the following half-reactions and their respective standard reduction potentials: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 MacLgq130601 (2.4k points)

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1 answer 113 views

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 CorneliusBur (2.1k points)

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1 answer 130 views

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 EmilyForro67 (1.6k points)

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1 answer 114 views

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 SaraNis63941 (1.4k points)

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1 answer 108 views

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 QJXClarice2 (2.5k points)

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1 answer 137 views

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 DKGStacy090 (2.4k points)

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1 answer 137 views

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 JuanitaShear (2.4k points)

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1 answer 86 views

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 ClementMackr (2.5k points)

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1 answer 130 views

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 QTHGenevieve (1.7k points)

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1 answer 162 views

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 OrvalFrankla (1.9k points)

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1 answer 163 views

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 CheryleCass8 (1.7k points)

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1 answer 133 views

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 HalleySomers (1.8k points)

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1 answer 85 views

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 DaisyThwaite (1.9k points)

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