Recent questions in Chemical thermodynamics

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Calculate the standard enthalpy change for the following reaction at 25°C given the enthalpies of formation (in kJ/mol) of the compounds involved:CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)Hf(CaCO3) = -1206.9 kJ/molHf(CaCl2) = -795.8 kJ/molHf(CO2) = -393.5 kJ/molHf(H2O) = -285.8 kJ/molHf(HCl) = -92.31 kJ/mol

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

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1 answer 29 views

Calculate the standard enthalpy change for the following neutralization reaction where hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH) to form sodium chloride (NaCl) and water (H2O).HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)Given the following tabulated standard enthalpies of formation values: ΔHf°(HCl) = -167 kJ/mol, ΔHf°(NaOH) = -469 kJ/mol, ΔHf°(NaCl) = -411 kJ/mol, ΔHf°(H2O) = -286 kJ/mol.

asked 2 days ago in Chemical thermodynamics by MaurineAbe9 (490 points)

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1 answer 31 views

Calculate the standard enthalpy change for the following neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH):HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)Given: - The standard enthalpy of formation (ΔHf°) of NaCl(aq) is -407.3 kJ/mol.- The standard enthalpy of formation (ΔHf°) of H2O(l) is -285.8 kJ/mol.- The specific heat capacity (c) of the solution is 4.18 J/g°C.- The temperature change (ΔT) during the reaction is 15°C. - The mass (m) of the solution is 50.0 g. What is the standard enthalpy change (ΔH°) for the neutralization reaction between HCl and NaOH?

asked 2 days ago in Chemical thermodynamics by ElbaFedler88 (570 points)

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1 answer 30 views

Calculate the standard enthalpy change for the following chemical reaction involving solutions:2HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2H2O(l)Given the following information:ΔHf° [HNO3(aq)] = -207.5 kJ/molΔHf° [Ba(OH)2(aq)] = -994.0 kJ/molΔHf° [Ba(NO3)2(aq)] = -537.5 kJ/mol

asked 2 days ago in Chemical thermodynamics by LucyGreene29 (490 points)

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1 answer 24 views

Calculate the standard enthalpy change for the dissolution reaction of 10.0 g of NaOH(s) in 100.0 g of water at 25°C, given that the heat absorbed by the solution is 9.14 kJ. (Molar mass of NaOH = 40.00 g/mol and specific heat capacity of water = 4.18 J/g·°C)

asked 2 days ago in Chemical thermodynamics by KathiCannan0 (410 points)

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1 answer 24 views

Calculate the standard enthalpy change for the dissolution of 5g of sodium chloride in 100mL of water at 25°C, given that the molar enthalpy of dissolution of NaCl is -3.9 kJ/mol.

asked 2 days ago in Chemical thermodynamics by ElijahGlaspi (510 points)

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1 answer 26 views

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 2 days ago in Chemical thermodynamics by DixieBeach5 (530 points)

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1 answer 17 views

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 2 days ago in Chemical thermodynamics by LibbyWhittel (430 points)

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1 answer 38 views

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 2 days ago in Chemical thermodynamics by VetaFunk053 (530 points)

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1 answer 27 views

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 2 days ago in Chemical thermodynamics by DonnellDewee (590 points)

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1 answer 19 views

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 2 days ago in Chemical thermodynamics by HalWhitten9 (590 points)

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1 answer 22 views

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 2 days ago in Chemical thermodynamics by HelenaFlemin (430 points)

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1 answer 32 views

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 2 days ago in Chemical thermodynamics by JaniChewning (820 points)

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1 answer 40 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 2 days ago in Chemical thermodynamics by MarinaWsq125 (550 points)

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1 answer 39 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 2 days ago in Chemical thermodynamics by MarielKeble (1.1k points)

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1 answer 27 views

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 2 days ago in Chemical thermodynamics by BrigetteFinc (390 points)

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1 answer 26 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 2 days ago in Chemical thermodynamics by ArcherPcc770 (550 points)

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1 answer 33 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 2 days ago in Chemical thermodynamics by YACCaryn271 (590 points)

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1 answer 30 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 2 days ago in Chemical thermodynamics by CharlotteLer (530 points)

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1 answer 43 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 2 days ago in Chemical thermodynamics by MerriP79566 (510 points)

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Recent questions in Chemical thermodynamics

Recent questions in Chemical thermodynamics

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