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Calculate the standard electrode potential (E°) for the redox reaction of the following half-reactions:Cu2+(aq) + 2e- → Cu(s) E° = +0.34 VFe3+(aq) + e- → Fe2+(aq) E° = +0.77 V

asked 4 days ago in Chemical thermodynamics by DawnAbraham (490 points)

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Calculate the standard enthalpy of formation of carbon dioxide (CO2) using the following information:C(graphite) + O2(g) -> CO2(g), ΔH° = -393.5 kJ/molC(graphite) + 2H2(g) -> CH4(g), ΔH° = -74.8 kJ/mol2H2(g) + O2(g) -> 2H2O(l), ΔH° = -572.0 kJ/mol

asked 4 days ago in ThermoChemistry by ZoeDodd3859 (770 points)

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Calculate the standard change in entropy for the reaction below using the given standard enthalpy and temperature information: 3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g) ΔH° = -770.2 kJ T = 298 K

asked 4 days ago in Inorganic Chemistry by WarnerThaxto (490 points)

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Calculate the standard enthalpy change for the reaction: CH3OH (l) + 3/2 O2 (g) -> CO2 (g) + 2H2O (l) given the standard enthalpies of formation for CH3OH (l), CO2 (g) and H2O (l) as -238.6 kJ/mol, -393.5 kJ/mol and -285.8 kJ/mol respectively.

asked 4 days ago in Chemical thermodynamics by SofiaDenison (730 points)

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Calculate the standard enthalpy change for the precipitation reaction of 50.0 grams of barium chloride and 75.0 grams of potassium sulfate to form solid barium sulfate and aqueous potassium chloride, given that the heat of formation of solid barium sulfate is -1474 kJ/mol and aqueous potassium chloride is -436 kJ/mol.

asked 4 days ago in Chemical thermodynamics by DortheaConsi (770 points)

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Calculate the standard enthalpy change for the reaction: C6H12O6 (s) + 6O2 (g) → 6CO2 (g) + 6H2O (l)Given the following standard enthalpies of formation: ΔHf(C6H12O6 (s)) = -1273 kJ/molΔHf(CO2 (g)) = -393.5 kJ/molΔHf(H2O (l)) = -285.8 kJ/mol

asked 4 days ago in Chemical thermodynamics by NoellaMccrea (450 points)

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What is the effect of changing the concentration of reactants on the rate of a chemical reaction at equilibrium?

asked 5 days ago in Chemical kinetics by TeodoroN8379 (390 points)

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Calculate the standard enthalpy change (ΔH°) for the following reaction at 298 K:2SO₂(g) + O₂(g) → 2SO₃(g)given the following standard enthalpy of formation values:ΔH°f (SO₂(g)) = -296.8 kJ/molΔH°f (O₂(g)) = 0 kJ/molΔH°f (SO₃(g)) = -395.7 kJ/mol

asked 4 days ago in Chemical thermodynamics by LAFFelicitas (190 points)

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Can the mechanical properties of ceramics be improved for use in high-temperature applications by adjusting the manufacturing parameters, such as sintering temperature and time?

asked 4 days ago in Materials Chemistry by BudCrider29 (550 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 4 days ago in Chemical thermodynamics by JaniNolen204 (270 points)

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Calculate the standard enthalpy of formation (∆Hf) of water (H2O) given the following information: 2H2(g) + O2(g) → 2H2O(l); ∆H = -572 kJ/mol and the standard enthalpy of formation of O2 is 0 kJ/mol.

asked 4 days ago in ThermoChemistry by WendyHenning (490 points)

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Design a novel biodegradable polymer and investigate its synthesis using sustainable and green chemistry practices.

asked 4 days ago in Polymer Chemistry by EvieWiegand (470 points)

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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 4 days ago in Chemical thermodynamics by WilliamsBorn (230 points)

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Calculate the standard enthalpy change for the reaction where 250 mL of 2M HCl is mixed with 500 mL of 1M NaOH, assuming that the specific heat capacity of the resulting solution is 4.18 J/g°C and the density of the solution is 1.00 g/mL. (Hint: The balanced chemical equation for the reaction is HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l))

asked 4 days ago in Chemical thermodynamics by ForrestFine0 (550 points)

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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 4 days ago in ElectroChemistry by PilarMcIntos (450 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 4 days ago in Chemical thermodynamics by JaymeBolick (330 points)

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Calculate the standard enthalpy change of the formation reaction for carbon dioxide (CO2) given the standard enthalpies of formation for carbon monoxide (CO) and oxygen gas (O2) as -110.5 kJ/mol and -249.2 kJ/mol, respectively.

asked 4 days ago in Chemical thermodynamics by MistyNewland (430 points)

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Calculate the vibrational frequencies and predict the infrared spectrum of methane (CH4) using quantum chemical methods.

asked 4 days ago in Quantum Chemistry by CooperLovegr (370 points)

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Calculate the vibrational frequencies and infrared spectra for a molecule of carbon dioxide (CO2) using quantum chemistry methods.

asked 4 days ago in Quantum Chemistry by LidiaScoggin (210 points)

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Calculate the standard enthalpy change for the following reaction at 298 K: 2NaHCO3(s) + MgCl2(aq) → MgCO3(s) + 2NaCl(aq) + H2O(l)Given the following standard enthalpies of formation: ΔHf°(NaHCO3) = -950.7 kJ/molΔHf°(MgCl2) = -641.8 kJ/molΔHf°(MgCO3) = -1128.2 kJ/molΔHf°(NaCl) = -411.2 kJ/molΔHf°(H2O) = -285.8 kJ/mol

asked 4 days ago in Chemical thermodynamics by Carrie69T008 (390 points)

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