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Calculate the standard enthalpy change for the dissolution of 3 mol of potassium chloride (KCl) in 1000 mL of water, given that the molar enthalpy of dissolution is -17.4 kJ/mol.

asked Feb 3 in Chemical thermodynamics by IvaHaugh7017 (2.1k points)

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Calculate the standard enthalpy change for the dissolution of 10 grams of potassium hydroxide (KOH) in 100 mL of water. Given that the molar enthalpy of dissolution of solid KOH is -57.61 kJ/mol and the density of water is 1 g/mL.

asked Feb 3 in Chemical thermodynamics by EdwardoO6191 (2.5k points)

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Calculate the standard enthalpy change for the dissolution of 10 grams of NaCl in water at 25°C, given that the molar enthalpy of dissolution of NaCl is -3.9 kJ/mol.

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

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1 answer 138 views

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 AhmadEho9450 (1.6k points)

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1 answer 182 views

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 BradyFlo6479 (2.5k 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 KandisBeckwi (1.6k points)

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1 answer 130 views

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 DarbyKieran3 (2.0k points)

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1 answer 133 views

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 IsabelleTitu (1.8k points)

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1 answer 109 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 GarnetGenove (2.2k points)

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1 answer 151 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 BettyWalsh4 (2.0k points)

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1 answer 122 views

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 LeesaJ55672 (1.9k points)

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1 answer 174 views

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 ChadLarocque (2.2k points)

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1 answer 132 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 ChuWegener2 (2.1k points)

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1 answer 114 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 YvetteLink0 (2.0k points)

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1 answer 120 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 SaraNis63941 (1.4k points)

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1 answer 125 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 CierraSpicer (1.4k points)

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1 answer 129 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 SelinaOmar8 (2.0k points)

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1 answer 173 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 Joey98948916 (1.5k points)

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1 answer 123 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 DUPMathias4 (2.1k points)

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1 answer 190 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 AdeleStrothe (2.1k points)

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