Recent questions in Chemical thermodynamics

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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 2 days ago in Chemical thermodynamics by DessieStopfo (570 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 2 days ago in Chemical thermodynamics by TamelaHollim (490 points)

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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 2 days ago in Chemical thermodynamics by ClarissaMcAl (350 points)

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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 2 days ago in Chemical thermodynamics by DerrickLavin (470 points)

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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 2 days ago in Chemical thermodynamics by Kimberly5191 (510 points)

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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 2 days ago in Chemical thermodynamics by EnidKieran6 (490 points)

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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 2 days ago in Chemical thermodynamics by PatriceWebbe (230 points)

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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 2 days ago in Chemical thermodynamics by DylanEnglish (370 points)

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Calculate the standard enthalpy change (ΔH°) for the reaction where 50.0 mL of 2.0 M hydrochloric acid reacts with 50.0 mL of 2.0 M sodium hydroxide to form 50.0 mL of 2.0 M sodium chloride and water, given that the density of the solutions is 1.00 g/mL and the specific heat capacity of the solutions is 4.18 J/g·°C.

asked 2 days ago in Chemical thermodynamics by RoryDelacruz (210 points)

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Calculate the standard enthalpy change (ΔH°) for the reaction where 1 mol of solid sodium hydroxide (NaOH) dissolves in excess water to produce 1 mol of aqueous solution and releases heat. Given that the standard enthalpy of formation (ΔH°f) for NaOH(s) is -425.6 kJ/mol, the heat capacity of the aqueous solution is 4.18 J/gK, and the change in temperature (ΔT) is observed to be 8.0°C for 250 g of the solution.

asked 2 days ago in Chemical thermodynamics by RheaNazario (530 points)

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Calculate the standard enthalpy change (ΔH°) for the reaction of combustion of 1 mole of ethanol (C2H5OH) given that the standard enthalpy of formation (ΔH°f) for ethanol and carbon dioxide (CO2) are -277.7 kJ/mol and -393.5 kJ/mol respectively, and the standard enthalpy of formation (ΔH°f) for water (H2O) is -285.8 kJ/mol. The balanced chemical equation for the reaction is as follows:C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (l)

asked 2 days ago in Chemical thermodynamics by LonBaskett07 (460 points)

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1 answer 43 views

Calculate the standard enthalpy change (ΔH°) for the phase transition reaction of ice to water, given that the enthalpy of fusion for ice is 6.01 kJ/mol and the specific heat capacity of water is 4.18 J/g·°C. Express your answer in kJ/mol.

asked 2 days ago in Chemical thermodynamics by EusebiaSweat (670 points)

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Calculate the standard enthalpy change (ΔH°) for the following reaction involving the coordination compound [Fe(H2O)6]2+:[Fe(H2O)6]2+(aq) + 2Cl-(aq) → [FeCl2(H2O)4](aq) + 2H2O(l) Given: ΔH°f [FeCl2(H2O)4](aq) = -334 kJ/mol ΔH°f [Fe(H2O)6]2+(aq) = -393 kJ/mol ΔH°f H2O(l) = -286 kJ/mol Note: The superscript ° denotes standard conditions (i.e. 1 atm and 25°C) and the superscript f denotes standard enthalpy of formation.

asked 2 days ago in Chemical thermodynamics by ElliottGalla (330 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 2 days ago in Chemical thermodynamics by LAFFelicitas (190 points)

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Calculate the standard enthalpy change (ΔH°) for the following reaction at 25°C, given that the enthalpies of formation for the reactants and products are:HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)ΔH°f[HCl (aq)] = -92.31 kJ/molΔH°f[NaOH (aq)] = -469.49 kJ/molΔH°f[NaCl (aq)] = -407.29 kJ/molΔH°f[H2O (l)] = -285.83 kJ/mol

asked 2 days ago in Chemical thermodynamics by DelilaM1159 (470 points)

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Calculate the standard enthalpy change (ΔH°) for the combustion reaction of ethanol (C2H5OH) if the heat evolved is 1367.6 kJ and the molar mass of ethanol is 46.07 g/mol.

asked 2 days ago in Chemical thermodynamics by DaniloMichel (910 points)

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Calculate the standard enthalpy change (in kJ/mol) for the reaction of hydrochloric acid (HCl) and sodium hydroxide (NaOH) to form sodium chloride (NaCl) and water (H2O), given the following balanced chemical equation:HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)Assume the reaction takes place under standard conditions (298 K and 1 atm pressure) and that all solutions have a concentration of 1.0 M. The standard enthalpies of formation for HCl (aq), NaOH (aq), NaCl (aq), and H2O (l) are -92.31 kJ/mol, -469.14 kJ/mol, -407.76 kJ/mol, and -285.83 kJ/mol, respectively.

asked 2 days ago in Chemical thermodynamics by KandaceGrey4 (570 points)

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Calculate the standard enthalpy change (in kJ/mol) for the neutralization reaction of hydrochloric acid (HCl) and sodium hydroxide (NaOH) using the following information: HCl (aq) + NaOH (aq) → NaCl (aq) + H2O(l)ΔHf° (kJ/mol): HCl (aq) = -167.2 NaOH (aq) = -469.2 NaCl (aq) = -407.3 H2O(l) = -285.8

asked 2 days ago in Chemical thermodynamics by MaxCampa199 (290 points)

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Calculate the standard enthalpy change (in kJ/mol) for the following reaction involving solutions: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)Given the following enthalpy values:NaOH(aq): -469.2 kJ/mol HCl(aq): -167.2 kJ/mol NaCl(aq): -411.2 kJ/mol H2O(l): -285.8 kJ/mol

asked 2 days ago in Chemical thermodynamics by CyrusPremo0 (430 points)

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Calculate the standard enthalpy change (in kJ/mol) for the dissolution of 3.50 g of potassium hydroxide (KOH) in 250.0 mL of water at 25°C, given that the molar heat of solution of KOH is -57.61 kJ/mol.

asked 2 days ago in Chemical thermodynamics by LoisPenny954 (570 points)

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