Recent questions without an upvoted answer

0 votes

1 answer 44 views

Calculate the standard enthalpy change (∆H°) and standard entropy change (∆S°) for the reaction between solid aluminum and gaseous oxygen to form solid aluminum oxide, given the following balanced chemical equation:4Al(s) + 3O2(g) → 2Al2O3(s) The standard enthalpies of formation of Al(s), O2(g), and Al2O3(s) are -394.4 kJ/mol, 0 kJ/mol, and -1675.7 kJ/mol, respectively. The standard entropy change for the reaction of O2(g) to form Al2O3(s) is -159.6 J/K·mol.

asked 5 days ago in Inorganic Chemistry by AdelaidaH499 (530 points)

0 votes

1 answer 35 views

Calculate the standard enthalpy change (∆H) for the vaporization of 25.0 g of water at its boiling point (100°C) and 1 atm pressure assuming the heat capacity of water to be constant. Given: The heat of vaporization for water is 40.7 kJ/mol and the molar mass of water is 18.015 g/mol.

asked 5 days ago in Chemical thermodynamics by OsvaldoCorte (390 points)

0 votes

1 answer 37 views

Calculate the standard enthalpy change ($\Delta H^\circ$) for the dissolution of 10.0 g of sodium hydroxide (NaOH) in 100.0 mL of water assuming that the specific heat capacity of the solution is 4.18 J g$^{-1}$ K$^{-1}$ and that the initial and final temperatures are 25.0$^\circ$C and 35.0$^\circ$C, respectively. The molar mass of NaOH is 40.0 g mol$^{-1}$.

asked 5 days ago in Chemical thermodynamics by WilliamsBorn (230 points)

0 votes

1 answer 38 views

Calculate the standard enthalpy and standard entropy change at 298 K for the following reaction: 2Fe(s) + 3/2O2(g) → Fe2O3(s) Given that the standard enthalpies of formation for Fe(s), O2(g), and Fe2O3(s) are 0 kJ/mol, 0 kJ/mol, and -826 kJ/mol respectively. Also, the standard molar entropy of Fe2O3(s) is 87.4 J/K/mol.

asked 5 days ago in Inorganic Chemistry by EvanMoye5887 (510 points)

0 votes

1 answer 40 views

Calculate the standard enthalpy and entropy change for the reaction, given the following information:2 H2(g) + O2(g) → 2 H2O(g)∆H°f [H2O(g)] = -241.8 kJ/mol∆H°f [H2(g)] = 0 kJ/mol∆H°f [O2(g)] = 0 kJ/mol∆S° [H2O(g)] = 188.8 J/Kmol∆S° [H2(g)] = 130.7 J/Kmol∆S° [O2(g)] = 205.2 J/KmolAssuming that all heat capacities are independent of temperature, calculate ∆S°rxn and ∆H°rxn for this reaction.

asked 5 days ago in Inorganic Chemistry by HugoHogg5769 (430 points)

0 votes

1 answer 41 views

Calculate the standard enthalpy and entropy change for the reaction that occurs when 1 mole of Fe2O3 is formed from its elements in their standard state, using the following given data:Fe(s) + 1.5 O2(g) → Fe2O3(s) ΔH°f = -824.2 kJ/mol ΔS° = 87.4 J/mol·K

asked 5 days ago in Inorganic Chemistry by MadgeLemberg (310 points)

0 votes

1 answer 36 views

Calculate the standard electrode potential of the half-cell reaction Ag+ + e- → Ag, given that the standard reduction potential of Ag+ is 0.80 V.

asked 5 days ago in ElectroChemistry by PilarMcIntos (450 points)

0 votes

1 answer 33 views

Calculate the standard electrode potential of the following reaction: Cu2+(aq) + 2e- ⇌ Cu(s) Given that the standard reduction potential of Cu2+(aq) is +0.34 V and the standard electrode potential of hydrogen electrode is 0.00 V.

asked 5 days ago in Chemical thermodynamics by MohammadC566 (390 points)

0 votes

1 answer 34 views

Calculate the standard electrode potential of the following cell: Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s) Given: Eº(Zn2+(aq)/Zn(s)) = -0.76 V and Eº(Cu2+(aq)/Cu(s)) = +0.34 V.

asked 5 days ago in ElectroChemistry by RhodaVue438 (570 points)

0 votes

1 answer 34 views

Calculate the standard electrode potential of the following cell reaction at 25°C: Cu(s) | Cu2+ (0.01 M) || Zn2+ (1.0 M) | Zn(s)

asked 5 days ago in ElectroChemistry by Frank7401499 (310 points)

0 votes

1 answer 32 views

Calculate the standard electrode potential of the electrode in the given electrochemical cell: Fe3+(aq) + 3e- → Fe(s) E°= -0.04V Ag+(aq) + e- → Ag(s) E°= 0.80V

asked 5 days ago in ElectroChemistry by StarlaStroud (530 points)

0 votes

1 answer 27 views

Calculate the standard electrode potential of the copper electrode if the standard electrode potential of the zinc electrode is -0.76 V and the standard cell potential is 1.10 V for the cell reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s). Use the equation Eºcell=Eº cathode - Eº anode where Eºcell is the standard cell potential, Eºcathode is the standard potential for the reduction half-reaction, and Eºanode is the standard potential for the oxidation half-reaction.

asked 5 days ago in ElectroChemistry by FedericoWess (450 points)

0 votes

1 answer 29 views

Calculate the standard electrode potential of copper electrode if the Cu2+ ion concentration is 1.0 M and the electrode is at 25°C. The half-cell reaction is Cu2+(aq) + 2e- → Cu(s).

asked 5 days ago in ElectroChemistry by MerriP79566 (510 points)

0 votes

1 answer 22 views

Calculate the standard electrode potential of an electrode that is in contact with a solution containing 0.1 M copper (II) ions and its concentration of Cu2+ ions is in equilibrium with a hydrogen electrode at 1 atm hydrogen pressure and pH = 0.

asked 5 days ago in ElectroChemistry by JaydenOutlaw (790 points)

0 votes

1 answer 48 views

Calculate the standard electrode potential of a silver electrode (Ag) in contact with a solution containing 1.0 M AgNO3 and a hydrogen electrode (Pt) in contact with a solution containing 1.0 M HCl, given that the reduction potential of Ag+/Ag is +0.80V and the reduction potential of H+/H2 is 0.00V at 298K.

asked 5 days ago in ElectroChemistry by RussFries886 (430 points)

0 votes

1 answer 25 views

Calculate the standard electrode potential of a half-cell containing F2(g) and F- ion at 25°C. The reduction potential for F2(g) is 2.87 V and the standard reduction potential for F- ion is -2.87 V.

asked 5 days ago in ElectroChemistry by RichelleHale (610 points)

0 votes

1 answer 35 views

Calculate the standard electrode potential for the redox reaction: Al(s) + Fe2+(aq) → Fe(s) + Al3+(aq) at 298K, given that the standard reduction potential for Fe2+/Fe is -0.44V and Al3+/Al is -1.66V.

asked 5 days ago in Chemical thermodynamics by CristineKula (710 points)

0 votes

1 answer 29 views

Calculate the standard electrode potential for the redox reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)if the standard electrode potentials for Zn2+/Zn and Cu2+/Cu half-cells are -0.76V and +0.34V, respectively.

asked 5 days ago in Chemical thermodynamics by CliffAachen7 (490 points)

0 votes

1 answer 22 views

Calculate the standard electrode potential for the redox reaction: Fe3+(aq) + e- → Fe2+(aq) given that the standard reduction potential for the Fe3+(aq)/Fe2+(aq) couple is +0.77 V.

asked 5 days ago in Chemical thermodynamics by Eulah68Z087 (650 points)

0 votes

1 answer 27 views

Calculate the standard electrode potential for the redox reaction: Fe3+(aq) + e- → Fe2+(aq) Given that the standard electrode potential for the reduction of Fe3+(aq) to Fe2+(aq) is +0.771 V and the standard electrode potential for the reduction of H+(aq) to H2(g) is 0.000 V.

asked 5 days ago in Chemical thermodynamics by AngelineWood (470 points)

Recent questions without an upvoted answer

Categories