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Calculate the standard enthalpy change for the fusion of 2.5 moles of solid sulfur (S8) at its melting point (388 K) using the given information: ΔHfus = 9.73 kJ/mol ΔSfus = 22.8 J/(mol*K) The molar heat capacity of solid sulfur is 22.75 J/(mol*K) and the heat capacity of the liquid sulfur is 37.05 J/(mol*K).

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

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Calculate the standard enthalpy change for the fusion of 2.5 moles of ice at 0℃ to form water at 0℃. Given that the molar enthalpy of fusion of ice is 6.01 kJ/mol and the specific heat capacity of water is 4.18 J/g·℃.

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

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Calculate the standard enthalpy change for the fusion of 100 grams of ice at 0°C to liquid water at 0°C. The specific heat capacity of water is 4.184 J/g°C, the standard enthalpy of fusion of water is 6.01 kJ/mol, and the molar mass of water is 18.015 g/mol. Assume all heat absorbed is used to melt the ice and the temperature remains constant.

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

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Calculate the standard enthalpy change for the fusion of 1 mole of solid water (ice) at 0°C to liquid water at 0°C. Given the enthalpy of fusion of solid water as 6.01 kJ/mol and the specific heat capacity of water as 4.18 J/g°C.

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

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Calculate the standard enthalpy change for the formation of water vapor (H2O (g)) from its elements, given that the standard enthalpy of formation of hydrogen gas (H2(g)) is -241.8 kJ/mol and the standard enthalpy of formation of oxygen gas (O2(g)) is 0 kJ/mol.

asked Feb 3 in Chemical thermodynamics by DeenaTrundle (2.2k points)

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Calculate the standard enthalpy change for the formation of one mole of methane (CH4) gas given the following information: - Heat of combustion of methane gas is -890.36 kJ/mol - Heat of formation of water (H2O) liquid is -285.83 kJ/mol - Heat of formation of carbon dioxide (CO2) gas is -393.52 kJ/mol

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

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Calculate the standard enthalpy change for the formation of methane gas (CH4) from its elements carbon (solid, graphite) and hydrogen gas (H2) given the following data:ΔHf° (C(graphite)) = 0 kJ/molΔHf° (H2(g)) = 0 kJ/molΔHc° (CH4(g)) = -890.4 kJ/mol

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

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Calculate the standard enthalpy change for the formation of methane (CH4) given the following equations:C(s) + O2(g) ⟶ CO2(g); ΔH = -393.5 kJ/mol2H2(g) + O2(g) ⟶ 2H2O(l); ΔH = -571.6 kJ/mol

asked Feb 3 in Chemical thermodynamics by JanisButterf (2.1k points)

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Calculate the standard enthalpy change for the formation of methane (CH4) from its elements carbon (C) and hydrogen (H2) at standard conditions, given the following thermodynamic data: ΔHf(C) = 0 kJ/molΔHf(H2) = 0 kJ/molΔHc(CH4) = -890.3 kJ/mol

asked Feb 3 in Chemical thermodynamics by K29986283214 (2.0k points)

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Calculate the standard enthalpy change for the formation of ethylene oxide (C2H4O) given the following reaction:C2H4(g) + 1.5 O2(g) -> C2H4O(g)Given the standard enthalpy of formation of C2H4(g) = 52.5 kJ/mol and that of O2(g) = 0 kJ/mol, determine the standard enthalpy of formation of C2H4O(g).

asked Feb 3 in Chemical thermodynamics by JannetteBarr (2.2k points)

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Calculate the standard enthalpy change for the formation of ethylene glycol (C2H6O2) from its elements given that the standard enthalpies of formation of carbon dioxide, water, and ethylene glycol are -393.5 kJ/mol, -285.8 kJ/mol, and -421.1 kJ/mol respectively.

asked Feb 3 in Chemical thermodynamics by ChiKellett4 (1.5k points)

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Calculate the standard enthalpy change for the formation of carbon dioxide (CO2) from its elements, given the following standard enthalpies of formation:ΔHf°(CO2) = -393.5 kJ/molΔHf°(C) = 0 kJ/molΔHf°(O2) = 0 kJ/mol

asked Feb 3 in Chemical thermodynamics by MarcellaMack (1.7k points)

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Calculate the standard enthalpy change for the formation of carbon dioxide (CO2) from its elements carbon (C) and oxygen (O2) given the following information:- The standard enthalpy change for the combustion of carbon to form carbon dioxide is -394 kJ/mol.- The standard enthalpy change for the combustion of hydrogen gas (H2) to form water (H2O) is -286 kJ/mol.- The standard enthalpy change for the reaction of oxygen gas (O2) with hydrogen gas (H2) to form water (H2O) is -572 kJ/mol.Note: All values are at standard temperature and pressure (298 K and 1 atm).

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

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Calculate the standard enthalpy change for the formation of ammonium chloride (NH4Cl) from its constituent elements, nitrogen (N2), hydrogen (H2), and chlorine (Cl2), given the following information:Reaction equation: N2(g) + 4H2(g) + 2Cl2(g) → 2NH4Cl(s)Standard enthalpy of formation for NH4Cl: -314.4 kJ/molStandard enthalpy of formation for N2(g): 0 kJ/molStandard enthalpy of formation for H2(g): 0 kJ/molStandard enthalpy of formation for Cl2(g): 0 kJ/mol Express your answer in kilojoules per mole (kJ/mol).

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

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Calculate the standard enthalpy change for the formation of ammonia gas from nitrogen gas and hydrogen gas using Hess's Law, given the following equations and their corresponding enthalpy changes:N2(g) + 3H2(g) → 2NH3(g) ∆H = -92.4 kJ/molN2(g) → 2N(g) ∆H = 941 kJ/molH2(g) → 2H(g) ∆H = 436 kJ/mol

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

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Calculate the standard enthalpy change for the formation of 2 moles of water vapor (H2O(g)) if the combustion of 1 mole of methane gas (CH4(g)) results in the formation of 2 moles of water vapor and 1 mole of carbon dioxide gas (CO2(g)). Given that the standard enthalpy change of combustion of methane is -890.4 kJ/mol.

asked Feb 3 in Chemical thermodynamics by OrenDarwin6 (1.9k points)

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Calculate the standard enthalpy change for the following reaction:2Fe(s) + 3/2O2(g) → Fe2O3(s)Given that the standard enthalpy of formation of Fe2O3(s) is -824 kJ/mol and the standard enthalpy of formation of Fe(s) and O2(g) are 0 kJ/mol.

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

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Calculate the standard enthalpy change for the following reaction: [CoCl(NH3)5]2+ (aq) + 4H2O (l) → [Co(H2O)6]2+ (aq) + 2Cl- (aq) + 5NH3 (g)Given that the standard enthalpy of formation of [Co(H2O)6]2+ (aq) is -1518.5 kJ/mol, [CoCl(NH3)5]2+ (aq) is -426.9 kJ/mol, and the enthalpy of vaporization of water is 44.0 kJ/mol.

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

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Calculate the standard enthalpy change for the following reaction: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) given the following standard enthalpy of formation values: ΔHf°[Fe2O3(s)] = -824.2 kJ/mol ΔHf°[CO(g)] = -110.5 kJ/mol ΔHf°[Fe(s)] = 0 kJ/mol ΔHf°[CO2(g)] = -393.5 kJ/mol

asked Feb 3 in Chemical thermodynamics by AdelaideYwt4 (1.6k points)

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Calculate the standard enthalpy change for the following reaction: 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) Given the following information: - The standard enthalpy of formation of NaOH(aq) is -469.20 kJ/mol - The standard enthalpy of formation of H2SO4(aq) is -814.50 kJ/mol - The standard enthalpy of formation of Na2SO4(aq) is -1388.10 kJ/mol Note: Make sure to balance the equation and use Hess's Law if necessary.

asked Feb 3 in Chemical thermodynamics by VenusU65079 (1.8k points)

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