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Calculate the standard free energy change (ΔG°) for the following redox reaction at 298K:Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) (Given: E°cell = 1.10V, F = 96,500 J/V.mol)

asked Feb 3 in Chemical thermodynamics by TraciCoomes1 (1.9k 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 Feb 3 in Chemical thermodynamics by ScottyWild8 (1.4k points)

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Calculate the standard free energy change (ΔG°) for the following reaction at 25°C: 2Fe2+(aq) + Cu2+(aq) -> 2Fe3+(aq) + Cu+(aq) (Standard reduction potentials: Fe3+(aq) + e- -> Fe2+(aq) E° = 0.77 V Cu2+(aq) + e- -> Cu+(aq) E° = 0.16 V)

asked Feb 3 in Chemical thermodynamics by LovieCastles (2.3k points)

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Calculate the standard free energy change (∆G°) for the reaction: 2CH4(g) + 3O2(g) → 2CO2(g) + 2H2O(l) at 298 K, given that the standard enthalpy change (∆H°) of the reaction is -890.4 kJ mol^-1 and the standard entropy change (∆S°) of the reaction is +292.2 J K^-1 mol^-1. Is the reaction spontaneous or non-spontaneous under standard conditions?

asked Feb 3 in Physical Chemistry by JaysonPlott5 (1.6k points)

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Calculate the standard free energy change (∆G°) for the following redox reaction at 25°C:2 Fe³⁺(aq) + 3 H₂(g) → 2 Fe(s) + 6 H⁺(aq)

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

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Calculate the standard entropy change of the following reaction: 2Fe(s) + 3Cl2(g) → 2FeCl3(s) Given that the standard enthalpy change for this reaction is -400 kJ/mol at 298 K and the standard molar entropy of FeCl3(s) is 95 J/mol K.

asked Feb 3 in Inorganic Chemistry by AudreaV25265 (2.0k points)

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Calculate the standard entropy change for the reaction: 2H2 (g) + O2 (g) -> 2H2O (g) given the standard enthalpy of formation of H2O (g) is -241.8 kJ/mol at 298 K.

asked Feb 3 in Inorganic Chemistry by CalvinHornin (1.6k points)

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Calculate the standard entropy change for the reaction: 2SO3(g) + O2(g) → 2SO4(g) Given the following standard entropies of formation: ΔS°f SO3(g) = 256.2 J/K mol ΔS°f O2(g) = 205.0 J/K mol ΔS°f SO4(g) = 296.8 J/K mol

asked Feb 3 in Inorganic Chemistry by GlenCaringto (2.1k points)

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Calculate the standard entropy change for the reaction of 2 moles of nitrogen gas reacting with 5 moles of oxygen gas to produce 2 moles of nitrogen monoxide gas at a constant pressure of 1 bar and 298 K. Given the standard molar entropy of nitrogen gas, oxygen gas, and nitrogen monoxide gas to be 191.6 J K-1 mol-1, 205.0 J K-1 mol-1, and 210.6 J K-1 mol-1, respectively.

asked Feb 3 in Chemical thermodynamics by JudithMackni (2.3k points)

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Calculate the standard entropy change for the reaction below at a temperature of 298 K:CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) The standard molar entropies are as follows: S(CH4) = 186.3 J K^-1 mol^-1S(O2) = 205.0 J K^-1 mol^-1S(CO2) = 213.7 J K^-1 mol^-1S(H2O) = 188.8 J K^-1 mol^-1

asked Feb 3 in Chemical thermodynamics by HenryCharles (2.0k points)

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Calculate the standard entropy change for the reaction 2H2(g) + O2(g) → 2H2O(g) given the standard entropy values of H2(g) = 130.6 J/mol K, O2(g) = 205.0 J/mol K, and H2O(g) = 188.8 J/mol K. Also, determine whether the reaction is spontaneous or not at 298 K.

asked Feb 3 in Inorganic Chemistry by LuzMccrary7 (2.5k points)

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Calculate the standard entropy change for the following reaction at 298 K:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) Given the standard entropies of CH4(g), O2(g), CO2(g), and H2O(l) are 186.26 J/K/mol, 205.03 J/K/mol, 213.74 J/K/mol, and 69.95 J/K/mol respectively.

asked Feb 3 in Chemical thermodynamics by EmerySynan65 (1.8k points)

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Calculate the standard enthalpy of reduction for the following reaction: Fe2O3 (s) + 3 H2(g) → 2 Fe(s) + 3 H2O(g)Given: ΔH°f for Fe2O3 (s) = -824.2 kJ/mol ΔH°f for H2O(g) = -241.8 kJ/molΔH°f for Fe(s) = 0 kJ/mol

asked Feb 3 in ThermoChemistry by PeteWirtz263 (2.1k points)

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Calculate the standard enthalpy of precipitation for the reaction: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) given that the standard enthalpies of formation for AgNO3(aq), NaCl(aq), AgCl(s), and NaNO3(aq) are -123.2 kJ/mol, -407.3 kJ/mol, -127.0 kJ/mol, and -467.3 kJ/mol, respectively.

asked Feb 3 in ThermoChemistry by NickolasShum (1.9k points)

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Calculate the standard enthalpy of hydrolysis for the following reaction: AlCl3 + 3H2O → Al(OH)3 + 3HCl Given that the standard enthalpies of formation for AlCl3(-696.5 kJ/mol), Al(OH)3(-1277.1 kJ/mol), and HCl(-92.3 kJ/mol) are known.

asked Feb 3 in ThermoChemistry by DelilahKyte3 (1.8k points)

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Calculate the standard enthalpy of hydrolysis for Na2CO3 when 2.5 moles of water react with 1 mole of Na2CO3, given that the heat of reaction is -843.2 kJ/mol.

asked Feb 3 in ThermoChemistry by LillianaY16 (1.7k points)

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Calculate the standard enthalpy of formation, ΔH°f, of carbon dioxide (CO2) gas given the following thermochemical equations: C(s) + O2(g) → CO2(g) ΔH°rxn = -393.5 kJ/mol C(s) + O2(g) → CO(g) ΔH°rxn = -110.5 kJ/mol CO(g) + 1/2 O2(g) → CO2(g) ΔH°rxn = -283.0 kJ/mol Assume that all reactants and products are in their standard states.

asked Feb 3 in ThermoChemistry by Karine04K24 (2.0k points)

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Calculate the standard enthalpy of formation of water using Hess's law and the following data:2H2(g) + O2(g) -> 2H2O(g) ΔH°rxn = -484 kJ/molH2(g) + 1/2O2(g) -> H2O(l) ΔH°rxn = -286 kJ/mol

asked Feb 3 in Chemical thermodynamics by MaximoVardon (1.9k points)

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Calculate the standard enthalpy of formation of water if you know that the standard enthalpy of combustion of hydrogen is -286 kJ/mol and the standard enthalpy of combustion of oxygen is -394 kJ/mol.

asked Feb 3 in Chemical thermodynamics by ZellaSeamon3 (1.6k points)

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Calculate the standard enthalpy of formation of water (H2O) given the following information:- The standard enthalpy of formation of hydrogen gas (H2) is 0 kJ/mol- The standard enthalpy of formation of oxygen gas (O2) is 0 kJ/mol- The standard enthalpy of combustion of hydrogen gas is -286 kJ/mol- The standard enthalpy of combustion of carbon (C) is -394 kJ/mol- The standard enthalpy of combustion of methane gas (CH4) is -890 kJ/mol

asked Feb 3 in ThermoChemistry by ChiKellett4 (1.5k points)

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