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Calculate the standard enthalpy change for the dissolution of 10 g of NaOH in 100 mL of water at 25°C if the molar enthalpy of dissolution is -44.5 kJ/mol.

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

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Calculate the standard enthalpy change for the complete combustion of methane gas (CH4) at 25°C and 1 atm pressure, given that the standard enthalpy of formation for CH4 is -74.9 kJ/mol and the standard enthalpy of formation for water (H2O) is -285.8 kJ/mol.

asked Feb 3 in Chemical thermodynamics by BettinaChirn (290 points)

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Calculate the standard enthalpy change for the complete combustion of methane gas (CH4(g)) at constant pressure, given the balanced equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l). The standard enthalpies of formation of CO2(g), H2O(l), and CH4(g) are -393.5 kJ/mol, -285.8 kJ/mol, and -74.8 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by LachlanFrair (330 points)

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Calculate the standard enthalpy change for the complete combustion of methane (CH4) at constant pressure and 298 K, given that the standard enthalpies of formation for CH4(g) and H2O(l) are -74.8 kJ/mol and -285.8 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by DebraAtkinso (230 points)

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Calculate the standard enthalpy change for the complete combustion of 2 moles of methane gas under standard conditions, where all reactants and products are in their standard states. The balanced chemical equation for the combustion of methane is CH4(g) + 2O2(g) → CO2(g) + 2H2O(l), and the standard enthalpy of formation ΔH°f for methane, carbon dioxide, and water are -74.8 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by CecilB463053 (310 points)

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1 answer 33 views

Calculate the standard enthalpy change for the combustion reaction of octane (C8H18) using the following balanced chemical equation:C8H18 + 12.5O2 →8CO2 + 9H2O Given the standard enthalpies of formation for CO2, H2O, and octane are -394 kJ/mol, -286 kJ/mol, and -249 kJ/mol respectively.

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

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1 answer 44 views

Calculate the standard enthalpy change for the combustion of methane gas using the following reaction: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g). Given the standard enthalpy of formation values for methane, carbon dioxide, and water, calculate the heat released or absorbed during this reaction. Express your answer in kJ/mol.

asked Feb 3 in Chemical thermodynamics by EmilieBobb0 (350 points)

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Calculate the standard enthalpy change for the combustion of methane gas at standard conditions, given the following balanced chemical equation:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)Note: Standard conditions refer to a temperature of 25°C and a pressure of 1 atm.

asked Feb 3 in Chemical thermodynamics by GerardMaes99 (410 points)

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Calculate the standard enthalpy change for the combustion of methane gas (CH4) given the balanced chemical equation:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)The relevant standard enthalpies of formation are:ΔHf°[CH4(g)] = -74.87 kJ/molΔHf°[CO2(g)] = -393.5 kJ/molΔHf°[H2O(l)] = -285.8 kJ/mol

asked Feb 3 in Chemical thermodynamics by EliBrinkman (370 points)

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1 answer 33 views

Calculate the standard enthalpy change for the combustion of methane (CH4) at constant pressure, given that the standard enthalpies of formation are -74.87 kJ/mol for methane and -393.51 kJ/mol for carbon dioxide (CO2), and 2H2(g) + O2(g) → 2H2O(l) has a standard enthalpy change of -571.66 kJ/mol.

asked Feb 3 in Chemical thermodynamics by KathrinPenne (350 points)

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1 answer 16 views

Calculate the standard enthalpy change for the combustion of ethene gas (C2H4(g)) to form carbon dioxide gas (CO2(g)) and water vapor (H2O(g)), given the following thermochemical equations: C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(g) ΔH°=-1411 kJ/mol2H2(g) + O2(g) → 2H2O(g) ΔH°=-484 kJ/mol

asked Feb 3 in Chemical thermodynamics by OpheliaTuggl (190 points)

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1 answer 34 views

Calculate the standard enthalpy change for the combustion of ethane (C2H6) given the balanced chemical equation:C2H6(g) + 3.5 O2(g) → 2CO2(g) + 3H2O(l)Assume all reactants and products are in standard states and use the following standard enthalpy of formation values:ΔHf°(C2H6) = -84.7 kJ/molΔHf°(CO2) = -393.5 kJ/molΔHf°(H2O) = -285.8 kJ/mol

asked Feb 3 in Chemical thermodynamics by RedaDoy9962 (310 points)

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1 answer 39 views

Calculate the standard enthalpy change for the combustion of ethane (C2H6) gas to form carbon dioxide (CO2) gas and water (H2O) vapor at 298 K and 1 atm. The balanced chemical equation for the reaction is: C2H6(g) + 3.5 O2(g) → 2 CO2(g) + 3H2O(g) Given that the standard enthalpy of formation for C2H6(g) is -84.68 kJ/mol, CO2(g) is -393.51 kJ/mol, and H2O(g) is -241.82 kJ/mol.

asked Feb 3 in Chemical thermodynamics by JennaFairfax (470 points)

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1 answer 30 views

Calculate the standard enthalpy change for the combustion of 1 mole of propane gas (C3H8) at standard conditions using the following balanced chemical equation: C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(l)Given the standard enthalpy of formation values at 298K for C3H8(g), CO2(g), and H2O(l) as -103.8, -393.5, and -285.8 kJ/mol respectively, calculate the standard enthalpy change for the combustion reaction.

asked Feb 3 in Chemical thermodynamics by Margot259311 (930 points)

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1 answer 30 views

Calculate the standard enthalpy change for the combustion of 1 mole of methane gas (CH4) under standard conditions given the following balanced chemical equation:CH4(g) + 2O2(g)→CO2(g) + 2H2O(g)(Standard conditions: temperature of 298K and pressure of 1 bar)

asked Feb 3 in Chemical thermodynamics by MiriamOtis62 (690 points)

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1 answer 26 views

Calculate the standard enthalpy change and the standard entropy change for the reaction: 2HCl(g) + Mg(s) → MgCl2(s) + H2(g) Given the following standard enthalpy of formation values: - HCl(g) = -92.31 kJ/mol - MgCl2(s) = -641.8 kJ/mol - H2(g) = 0 kJ/mol - Mg(s) = 0 kJ/mol Also given the following standard molar entropy values:- HCl(g) = 186.9 J/Kmol - MgCl2(s) = 138.53 J/Kmol - H2(g) = 130.7 J/Kmol - Mg(s) = 32.85 J/Kmol

asked Feb 3 in Inorganic Chemistry by KeeleyGame0 (290 points)

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1 answer 42 views

Calculate the standard enthalpy change and entropy change for the reaction: 2Fe(s) + 3/2O2(g) -> Fe2O3(s) Given the standard enthalpies of formation of Fe(s), O2(g), and Fe2O3(s) are -0.44 kJ/mol, 0 kJ/mol, and -826 kJ/mol, respectively. Also, the standard molar entropy of Fe2O3(s) is 87.4 J/(mol K).

asked Feb 3 in Inorganic Chemistry by MitchNina52 (290 points)

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1 answer 23 views

Calculate the standard enthalpy change (ΔH°), standard entropy change (ΔS°) and standard Gibbs free energy change (ΔG°) of the reaction:2A(g) + 3B(g) → C(g) + 2D(g)given thatΔH°f[A(g)] = 200 kJ mol^-1Δ H°f [B(g)] = 100 kJ mol^-1Δ H°f [C(g)] = 400 kJ mol^-1Δ H°f [D(g)] = 0 kJ mol^-1ΔH°= -400 kJ mol^-1Temperature (T) = 298 KThe student needs to use their knowledge in quantum chemistry and thermodynamics to calculate the thermodynamic properties of the given reaction.

asked Feb 3 in Quantum Chemistry by Cathern38144 (570 points)

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1 answer 38 views

Calculate the standard enthalpy change (ΔH°) for the reduction of iron(III) oxide (Fe2O3) to iron (Fe) given the following balanced chemical equation:2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g)The enthalpy of formation for Fe2O3(s) is -824.2 kJ/mol and the enthalpy of formation for CO2(g) is -393.5 kJ/mol. All other substances are in their standard state.

asked Feb 3 in ThermoChemistry by HughLarge668 (550 points)

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1 answer 46 views

Calculate the standard enthalpy change (ΔH°) for the reaction:2H2(g) + O2(g) → 2H2O(g)given the following bond energies:H-H = 436 kJ/mol, O=O = 498 kJ/mol, H-O = 463 kJ/mol

asked Feb 3 in Quantum Chemistry by ErmelindaHur (510 points)

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