Recent questions in Chemistry

0 votes

1 answer 30 views

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 4 days ago in Chemical bonding by CandraDawbin (530 points)

0 votes

1 answer 30 views

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 4 days ago in ElectroChemistry by XMNLesli9153 (430 points)

0 votes

1 answer 42 views

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 4 days ago in ElectroChemistry by Fred30X73439 (450 points)

0 votes

1 answer 29 views

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 4 days ago in ElectroChemistry by CarleyMcdono (410 points)

0 votes

1 answer 37 views

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 4 days ago in Chemical thermodynamics by AzucenaWinga (390 points)

0 votes

1 answer 40 views

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 4 days ago in ElectroChemistry by BereniceStre (370 points)

0 votes

1 answer 33 views

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 4 days ago in ElectroChemistry by Korey4848809 (530 points)

0 votes

1 answer 31 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 4 days ago in Physical Chemistry by DJKScotty15 (590 points)

0 votes

1 answer 24 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 4 days ago in ElectroChemistry by CortezJustus (330 points)

0 votes

1 answer 22 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 4 days ago in ElectroChemistry by SheldonWhitf (430 points)

0 votes

1 answer 33 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 4 days ago in Chemical thermodynamics by MollieMaddox (810 points)

0 votes

1 answer 32 views

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 4 days ago in Chemical thermodynamics by RoxieVenable (350 points)

0 votes

1 answer 28 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 4 days ago in Chemical thermodynamics by TillyFiorini (730 points)

0 votes

1 answer 32 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 4 days ago in Chemical thermodynamics by OlivePidgeon (410 points)

0 votes

1 answer 30 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 4 days ago in Chemical thermodynamics by AnastasiaDwi (370 points)

0 votes

1 answer 40 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 4 days ago in Chemical thermodynamics by SheldonW2345 (590 points)

0 votes

1 answer 20 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 4 days ago in Chemical thermodynamics by LowellBoerne (270 points)

0 votes

1 answer 36 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 4 days ago in Chemical thermodynamics by Latanya48975 (350 points)

0 votes

1 answer 7 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 4 days ago in Chemical thermodynamics by JarrodMorgan (290 points)

0 votes

1 answer 28 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 4 days ago in Chemical thermodynamics by JaniNolen204 (270 points)

Categories