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Calculate the standard enthalpy change for the fusion of solid silver (Ag) at its melting point (961.78°C) to liquid silver (Ag) at the same temperature. Given the standard enthalpy of fusion of solid silver is 11.3 kJ/mol.

asked Feb 3 in Chemical thermodynamics by DonnyTorres9 (410 points)

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Calculate the standard enthalpy change for the fusion of solid hydrogen (H₂) at its melting point of 13.81 K, given that the standard enthalpy of fusion of H₂ is 0.117 kJ/mol.

asked Feb 3 in Chemical thermodynamics by VincentResch (390 points)

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Calculate the standard enthalpy change for the fusion of ice at 0°C to liquid water at 0°C, given that the enthalpy of fusion of ice is 6.01 kJ/mol and the molar mass of water is 18.015 g/mol.

asked Feb 3 in Chemical thermodynamics by HomerDrury6 (490 points)

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Calculate the standard enthalpy change for the fusion of 50 grams of ice at -10°C to liquid water at 10°C. Given the enthalpy of fusion of ice is 6.01 kJ/mol and the specific heat capacity of water is 4.184 J/g°C.

asked Feb 3 in Chemical thermodynamics by ArlenHoule07 (390 points)

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Calculate the standard enthalpy change for the fusion of 25 grams of ice at -10°C to liquid water at 20°C. The specific heat capacity of ice is 2.09 J/g°C, the specific heat capacity of water is 4.18 J/g°C, and the enthalpy of fusion of water is 6.01 kJ/mol.

asked Feb 3 in Chemical thermodynamics by CaseyMorin76 (450 points)

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Calculate the standard enthalpy change for the fusion of 2.5 moles of solid sulfur (S8) at its melting point (388 K) using the given information: ΔHfus = 9.73 kJ/mol ΔSfus = 22.8 J/(mol*K) The molar heat capacity of solid sulfur is 22.75 J/(mol*K) and the heat capacity of the liquid sulfur is 37.05 J/(mol*K).

asked Feb 3 in Chemical thermodynamics by MohammadC566 (350 points)

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Calculate the standard enthalpy change for the fusion of 2.5 moles of ice at 0℃ to form water at 0℃. Given that the molar enthalpy of fusion of ice is 6.01 kJ/mol and the specific heat capacity of water is 4.18 J/g·℃.

asked Feb 3 in Chemical thermodynamics by RosalineFauv (130 points)

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Calculate the standard enthalpy change for the fusion of 100 grams of ice at 0°C to liquid water at 0°C. The specific heat capacity of water is 4.184 J/g°C, the standard enthalpy of fusion of water is 6.01 kJ/mol, and the molar mass of water is 18.015 g/mol. Assume all heat absorbed is used to melt the ice and the temperature remains constant.

asked Feb 3 in Chemical thermodynamics by Jeannine13L7 (430 points)

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Calculate the standard enthalpy change for the fusion of 1 mole of solid water (ice) at 0°C to liquid water at 0°C. Given the enthalpy of fusion of solid water as 6.01 kJ/mol and the specific heat capacity of water as 4.18 J/g°C.

asked Feb 3 in Chemical thermodynamics by SherrylZqx4 (240 points)

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Calculate the standard enthalpy change for the formation of water vapor (H2O (g)) from its elements, given that the standard enthalpy of formation of hydrogen gas (H2(g)) is -241.8 kJ/mol and the standard enthalpy of formation of oxygen gas (O2(g)) is 0 kJ/mol.

asked Feb 3 in Chemical thermodynamics by LouieEmmons4 (430 points)

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Calculate the standard enthalpy change for the formation of one mole of methane (CH4) gas given the following information: - Heat of combustion of methane gas is -890.36 kJ/mol - Heat of formation of water (H2O) liquid is -285.83 kJ/mol - Heat of formation of carbon dioxide (CO2) gas is -393.52 kJ/mol

asked Feb 3 in Chemical thermodynamics by Armando5965 (290 points)

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Calculate the standard enthalpy change for the formation of methane gas (CH4) from its elements carbon (solid, graphite) and hydrogen gas (H2) given the following data:ΔHf° (C(graphite)) = 0 kJ/molΔHf° (H2(g)) = 0 kJ/molΔHc° (CH4(g)) = -890.4 kJ/mol

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

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1 answer 27 views

Calculate the standard enthalpy change for the formation of methane (CH4) given the following equations:C(s) + O2(g) ⟶ CO2(g); ΔH = -393.5 kJ/mol2H2(g) + O2(g) ⟶ 2H2O(l); ΔH = -571.6 kJ/mol

asked Feb 3 in Chemical thermodynamics by EstebanKenne (210 points)

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Calculate the standard enthalpy change for the formation of methane (CH4) from its elements carbon (C) and hydrogen (H2) at standard conditions, given the following thermodynamic data: ΔHf(C) = 0 kJ/molΔHf(H2) = 0 kJ/molΔHc(CH4) = -890.3 kJ/mol

asked Feb 3 in Chemical thermodynamics by TinaStamps81 (650 points)

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1 answer 22 views

Calculate the standard enthalpy change for the formation of ethylene oxide (C2H4O) given the following reaction:C2H4(g) + 1.5 O2(g) -> C2H4O(g)Given the standard enthalpy of formation of C2H4(g) = 52.5 kJ/mol and that of O2(g) = 0 kJ/mol, determine the standard enthalpy of formation of C2H4O(g).

asked Feb 3 in Chemical thermodynamics by LLIRhys20886 (230 points)

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1 answer 31 views

Calculate the standard enthalpy change for the formation of ethylene glycol (C2H6O2) from its elements given that the standard enthalpies of formation of carbon dioxide, water, and ethylene glycol are -393.5 kJ/mol, -285.8 kJ/mol, and -421.1 kJ/mol respectively.

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

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Calculate the standard enthalpy change for the formation of carbon dioxide (CO2) from its elements, given the following standard enthalpies of formation:ΔHf°(CO2) = -393.5 kJ/molΔHf°(C) = 0 kJ/molΔHf°(O2) = 0 kJ/mol

asked Feb 3 in Chemical thermodynamics by MiaTryon261 (190 points)

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Calculate the standard enthalpy change for the formation of carbon dioxide (CO2) from its elements carbon (C) and oxygen (O2) given the following information:- The standard enthalpy change for the combustion of carbon to form carbon dioxide is -394 kJ/mol.- The standard enthalpy change for the combustion of hydrogen gas (H2) to form water (H2O) is -286 kJ/mol.- The standard enthalpy change for the reaction of oxygen gas (O2) with hydrogen gas (H2) to form water (H2O) is -572 kJ/mol.Note: All values are at standard temperature and pressure (298 K and 1 atm).

asked Feb 3 in Chemical thermodynamics by LeviW4659934 (230 points)

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Calculate the standard enthalpy change for the formation of ammonium chloride (NH4Cl) from its constituent elements, nitrogen (N2), hydrogen (H2), and chlorine (Cl2), given the following information:Reaction equation: N2(g) + 4H2(g) + 2Cl2(g) → 2NH4Cl(s)Standard enthalpy of formation for NH4Cl: -314.4 kJ/molStandard enthalpy of formation for N2(g): 0 kJ/molStandard enthalpy of formation for H2(g): 0 kJ/molStandard enthalpy of formation for Cl2(g): 0 kJ/mol Express your answer in kilojoules per mole (kJ/mol).

asked Feb 3 in Chemical thermodynamics by DianHolliday (430 points)

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Calculate the standard enthalpy change for the formation of ammonia gas from nitrogen gas and hydrogen gas using Hess's Law, given the following equations and their corresponding enthalpy changes:N2(g) + 3H2(g) → 2NH3(g) ∆H = -92.4 kJ/molN2(g) → 2N(g) ∆H = 941 kJ/molH2(g) → 2H(g) ∆H = 436 kJ/mol

asked Feb 3 in ThermoChemistry by JustinKasper (310 points)

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