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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 KateBap07819 (310 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 IPOMira46304 (290 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 DustinD58026 (410 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 DanielleBouc (330 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 ArianneDuhig (410 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 MatildaMatos (430 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 Elliott59662 (270 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 LloydChristy (710 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 SusannaCaste (310 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 CortezDale67 (290 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 EliWilkerson (270 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 AlenaPeter3 (350 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 LeliaMcCann8 (450 points)

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1 answer 33 views

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 CierraYamada (210 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 Craig9385823 (390 points)

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1 answer 28 views

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 Genevieve35R (270 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 ChelseyHenle (310 points)

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Calculate the standard enthalpy of formation of water (H2O) given the following information: ΔHf° of H2(g) = 0 kJ/molΔHf° of O2(g) = 0 kJ/molΔHf° of H2O2(l) = -188.2 kJ/mol

asked Feb 3 in ThermoChemistry by ArdenHutto33 (230 points)

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1 answer 46 views

Calculate the standard enthalpy of formation of propane (C3H8) given the following data:- Standard enthalpy of formation of CO2(g) = -393.5 kJ/mol- Standard enthalpy of formation of H2O(l) = -285.8 kJ/mol- Standard enthalpy of combustion of propane at constant pressure = -2220.1 kJ/mol

asked Feb 3 in Chemical thermodynamics by JaimieGuerra (490 points)

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1 answer 42 views

Calculate the standard enthalpy of formation of potassium nitrate (KNO3) given the following information:- Heat of combustion of potassium is -468 kJ/mol- Heat of combustion of nitrogen is -940 kJ/mol- Heat of combustion of oxygen is -283.8 kJ/mol- Heat of formation of KNO3 is -383 kJ/mol.

asked Feb 3 in Chemical thermodynamics by TheronDorsch (310 points)

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