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Calculate the standard enthalpy change for the dissolution of 5.36 g of NaOH in 100.0 mL of water, given that the molar enthalpy of dissolution for NaOH is -44.5 kJ/mol.

asked 5 days ago in Chemical thermodynamics by DixieBeach5 (530 points)

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Calculate the standard enthalpy change for the dissolution of 5.00 g of solid sodium hydroxide (NaOH) in water, given that the molar enthalpy of dissolution of NaOH is -44.51 kJ/mol. Assume that the specific heat capacity and density of the solution are the same as pure water and that no heat is lost to the surroundings during the dissolution process.

asked 5 days ago in Chemical thermodynamics by LibbyWhittel (430 points)

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Calculate the standard enthalpy change for the dissolution of 5 grams of ammonium chloride (NH4Cl) in water, given that the molar enthalpy of dissolution of NH4Cl is -340.0 kJ/mol. The molar mass of NH4Cl is 53.49 g/mol and the density of water is 1.00 g/mL.

asked 5 days ago in Chemical thermodynamics by VetaFunk053 (530 points)

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Calculate the standard enthalpy change for the dissolution of 3.00 moles of sodium chloride in water, given that the molar enthalpy of solution of sodium chloride is -3.88 kJ/mol.

asked 5 days ago in Chemical thermodynamics by DonnellDewee (590 points)

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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 5 days ago in Chemical thermodynamics by HalWhitten9 (590 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 5 days ago in Chemical thermodynamics by HelenaFlemin (430 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 5 days ago in Chemical thermodynamics by JaniChewning (820 points)

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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 5 days ago in Chemical thermodynamics by MarinaWsq125 (550 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 5 days ago in Chemical thermodynamics by MarielKeble (1.1k 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 5 days ago in Chemical thermodynamics by BrigetteFinc (390 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 5 days ago in Chemical thermodynamics by ArcherPcc770 (550 points)

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1 answer 34 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 5 days ago in Chemical thermodynamics by YACCaryn271 (590 points)

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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 5 days ago in Chemical thermodynamics by CharlotteLer (530 points)

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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 5 days ago in Chemical thermodynamics by MerriP79566 (510 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 5 days ago in Chemical thermodynamics by DessieStopfo (570 points)

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1 answer 36 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 5 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 5 days ago in Chemical thermodynamics by ClarissaMcAl (350 points)

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1 answer 15 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 5 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 5 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 5 days ago in Chemical thermodynamics by EnidKieran6 (490 points)

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