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Calculate the standard potential of a Daniell cell if the concentration of copper ions and zinc ions in their respective half-cells is 1.0 M and the temperature of the cell is 25°C. The standard reduction potentials of copper and zinc electrodes are +0.34 V and -0.76 V respectively.

asked Feb 3 in Physical Chemistry by AlycePulley2 (450 points)

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Calculate the standard molar entropy change for the reaction: 2 SO2(g) + O2(g) → 2 SO3(g) at 298 K, given the following standard molar entropies: ΔS°(SO2(g)) = 248.2 J K^-1 mol^-1 ΔS°(O2(g)) = 205.0 J K^-1 mol^-1 ΔS°(SO3(g)) = 256.2 J K^-1 mol^-1

asked Feb 3 in Quantum Chemistry by TiaPritt9171 (190 points)

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Calculate the standard molar entropy change (∆S°) at 298 K for the reaction: 2H2 (g) + O2 (g) → 2H2O (l) given that the standard molar enthalpy change (∆H°) for this reaction is -572 kJ/mol.

asked Feb 3 in Quantum Chemistry by FrancescoB73 (450 points)

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Calculate the standard molar enthalpy change for the following reaction using quantum chemistry and compare it with the literature value: 2H2(g) + O2(g) -> 2H2O(g) Literature Value: -572 kJ/mol

asked Feb 3 in Quantum Chemistry by SuzanneTabor (390 points)

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Calculate the standard heat of mixing when 50 mL of 1 M HCl is mixed with 100 mL of 1 M NaOH at 25°C. The standard heat of neutralization of 1 M HCl and 1 M NaOH is -57.32 kJ/mol.

asked Feb 3 in ThermoChemistry by Antoinette08 (370 points)

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Calculate the standard heat of formation of water (H2O) using the bond dissociation energies of H2 and O2 and the standard heat of combustion of methane (CH4).

asked Feb 3 in Chemical bonding by MyrtleW57555 (250 points)

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Calculate the standard heat of formation (in kJ/mol) of water (H2O) given the following bond energies: H-H = 436 kJ/mol, O=O = 498 kJ/mol, H-O = 463 kJ/mol.

asked Feb 3 in Chemical bonding by JesusBittner (210 points)

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Calculate the standard Gibbs free energy change, ΔG°, for the electrochemical reaction of 2 moles of aluminum (Al) being oxidized to form 3 moles of aluminum oxide (Al2O3) in a standard state. Given that E°cell for the reaction is 1.66 V and the standard potential for the reduction of Al3+ ions to Al is -1.66 V.

asked Feb 3 in ElectroChemistry by MarcelaDeros (410 points)

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Calculate the standard Gibbs free energy change for the reaction that occurs when a cell consisting of a nickel electrode and a silver electrode is connected, given that the nickel electrode is immersed in a solution containing 0.010 M Ni2+ ions and the silver electrode is immersed in a solution containing 0.20 M Ag+ ions. The standard reduction potential for the Ni2+/Ni half-cell is -0.25 V and for the Ag+/Ag half-cell is +0.80 V.

asked Feb 3 in ElectroChemistry by CoraDown5757 (590 points)

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Calculate the standard Gibbs free energy change for the following electrochemical reaction at 25°C:Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s) Given: E°cell = 0.46 V, F = 96,500 C/mol, R = 8.314 J/K·mol, and the standard reduction potentials at 25°C are Cu²⁺(aq) + 2e⁻ → Cu(s) (E°red = 0.34 V) and Ag⁺(aq) + e⁻ → Ag(s) (E°red = 0.80 V).

asked Feb 3 in ElectroChemistry by JulianeGlynn (450 points)

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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 HXWEvie0029 (490 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 BrockTimmons (410 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 ElijahGlaspi (470 points)

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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 TrevorPerdri (430 points)

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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 Sadye01D9381 (150 points)

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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 LXKVilma3586 (350 points)

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1 answer 35 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 CecilB463053 (330 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 MillieFowlke (550 points)

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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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