Recent questions in Chemical thermodynamics

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Calculate the standard enthalpy change for the reaction 2 SO2(g) + O2(g) → 2 SO3(g), given the following standard enthalpy of formation: ΔHf° (SO2) = -296.8 kJ/mol, ΔHf° (SO3) = -396.2 kJ/mol.

asked 2 days ago in Chemical thermodynamics by JermaineMaue (320 points)

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1 answer 26 views

Calculate the standard enthalpy change for the precipitation reaction: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)given that the standard enthalpy of formation for AgCl(s) is -127.0 kJ/mol, and for NaNO3(aq) is -467.14 kJ/mol. The molar enthalpy of solution of NaCl and AgNO3 are -3.9 kJ/mol and -19.9 kJ/mol respectively.

asked 2 days ago in Chemical thermodynamics by NoemiBlamey (350 points)

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Calculate the standard enthalpy change for the precipitation reaction: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) Given that the standard enthalpy of formation (∆Hf) for AgNO3(aq), NaCl(aq), AgCl(s), and NaNO3(aq) are -123.1 kJ/mol, -407.3 kJ/mol, -127.0 kJ/mol, and -467.3 kJ/mol respectively.

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

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Calculate the standard enthalpy change for the precipitation reaction that takes place when 25.0 mL of 0.250 M barium chloride (BaCl2) and 50.0 mL of 0.100 M sodium sulfate (Na2SO4) react to form a precipitate of barium sulfate (BaSO4). The density of each solution is 1.00 g/mL and the specific heat capacity is 4.18 J/g°C. Assume a constant temperature of 25°C.

asked 2 days ago in Chemical thermodynamics by KarineTerry (690 points)

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1 answer 33 views

Calculate the standard enthalpy change for the precipitation reaction that occurs when 100 mL of 0.2 M lead nitrate solution reacts with 100 mL of 0.1 M sodium iodide solution to form solid lead iodide and aqueous sodium nitrate. The balanced chemical equation for the reaction is:Pb(NO3)2(aq) + 2 NaI(aq) → PbI2(s) + 2 NaNO3(aq)Given: - Molar mass of Pb(NO3)2 = 331.20 g/mol - Molar mass of NaI = 149.89 g/mol - Density of 0.2 M lead nitrate solution = 1.055 g/mL - Density of 0.1 M sodium iodide solution = 1.04 g/mL - Specific heat capacity of the reaction mixture is 4.18 J/(g · °C) - The initial temperature of the reaction mixture and the surroundings is 25 °C.

asked 2 days ago in Chemical thermodynamics by YYGKarry1452 (620 points)

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1 answer 24 views

Calculate the standard enthalpy change for the precipitation reaction of solid silver chloride (AgCl) from the aqueous solution with the precipitation agent, hydrochloric acid (HCl). Given the molar enthalpies of formation of AgCl(s) and HCl(g) are -127.01 kJ/mol and -92.31 kJ/mol, respectively. The balanced equation for the reaction is: AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)

asked 2 days ago in Chemical thermodynamics by FinlayBaumga (450 points)

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Calculate the standard enthalpy change for the precipitation reaction of copper(II) sulfate and sodium hydroxide, given the following balanced chemical equation:CuSO4(aq) + 2NaOH(aq) → Cu(OH)2(s) + Na2SO4(aq)Assume the reaction takes place under standard conditions and the necessary species are present in their standard states. Round your answer to two decimal places.

asked 2 days ago in Chemical thermodynamics by VedaHoar6953 (730 points)

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1 answer 29 views

Calculate the standard enthalpy change for the precipitation reaction of 50.0 grams of barium chloride and 75.0 grams of potassium sulfate to form solid barium sulfate and aqueous potassium chloride, given that the heat of formation of solid barium sulfate is -1474 kJ/mol and aqueous potassium chloride is -436 kJ/mol.

asked 2 days ago in Chemical thermodynamics by DortheaConsi (770 points)

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1 answer 33 views

Calculate the standard enthalpy change for the precipitation reaction between lead(II) nitrate and sodium chloride to form lead(II) chloride and sodium nitrate. The balanced chemical equation for the reaction is:Pb(NO3)2 (aq) + 2NaCl (aq) → PbCl2 (s) + 2NaNO3 (aq)

asked 2 days ago in Chemical thermodynamics by RWTIona27307 (670 points)

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Calculate the standard enthalpy change for the precipitation reaction between aqueous silver nitrate (AgNO3) and aqueous sodium chloride (NaCl) to form solid silver chloride (AgCl) and aqueous sodium nitrate (NaNO3), given the following balanced chemical equation:AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq) Assume that the reaction takes place under standard conditions (25°C and 1 atm) and that all solutions are at 1 M concentration.

asked 2 days ago in Chemical thermodynamics by MiloMoeller (310 points)

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1 answer 25 views

Calculate the standard enthalpy change for the precipitation reaction between 70.0 mL of 0.500 M lead(II) nitrate solution and excess sodium iodide solution at 25°C, if the resulting precipitate is PbI2 and the specific heat capacity of the solution is 4.18 J g^-1°C^-1.

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

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1 answer 31 views

Calculate the standard enthalpy change for the phase transition reaction, where 1 mole of solid water (ice) is transformed into 1 mole of liquid water at a constant pressure of 1 atm and a temperature of 298 K. Given the specific heat capacity of ice is 2.108 J g^-1 K^-1 and the specific heat capacity of water is 4.184 J g^-1 K^-1. The molar enthalpy of fusion of water is 6.01 kJ/mol.

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

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1 answer 28 views

Calculate the standard enthalpy change for the phase transition reaction where 100.0 grams of solid water (ice) at -10.0 °C is heated to form 100.0 grams of liquid water at 10.0 °C, given the specific heat capacities of ice and water are 2.09 J/g·°C and 4.18 J/g·°C, respectively, and the enthalpy of fusion of water is 6.01 kJ/mol.

asked 2 days ago in Chemical thermodynamics by JermaineHoag (250 points)

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1 answer 32 views

Calculate the standard enthalpy change for the phase transition reaction of solid water (ice) at -10°C into liquid water at 25°C if the enthalpy of fusion of ice is 6.01 kJ/mol and the specific heat capacity of ice and liquid water are 2.09 J/g°C and 4.18 J/g°C, respectively.

asked 2 days ago in Chemical thermodynamics by ReganBrady59 (390 points)

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1 answer 32 views

Calculate the standard enthalpy change for the phase transition reaction of solid iodine to iodine vapor using the following information:- Standard enthalpy of fusion of solid iodine = 15.52 kJ/mol- Standard enthalpy of vaporization of iodine = 41.57 kJ/mol- Heat capacity of solid iodine = 54.44 J/mol*K- Heat capacity of iodine vapor = 27.32 J/mol*K- Melting point of iodine = 386.85 K- Boiling point of iodine = 457.4 K

asked 2 days ago in Chemical thermodynamics by JustineDez22 (470 points)

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Calculate the standard enthalpy change for the phase transition reaction of solid carbon dioxide (dry ice) to gaseous carbon dioxide at 298 K and 1 atm pressure, given that the standard enthalpy of sublimation of solid carbon dioxide is 25.2 kJ/mol.

asked 2 days ago in Chemical thermodynamics by RudyD6073718 (250 points)

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1 answer 15 views

Calculate the standard enthalpy change for the phase transition reaction of solid carbon dioxide (dry ice) at -78.5°C to gaseous carbon dioxide at 1 atm and 25°C, given the following information: The standard enthalpy of fusion of solid carbon dioxide is 8.4 kJ/mol and the standard enthalpy of vaporization of gaseous carbon dioxide is 22.1 kJ/mol.

asked 2 days ago in Chemical thermodynamics by MilanKight97 (690 points)

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1 answer 24 views

Calculate the standard enthalpy change for the phase transition reaction of solid carbon dioxide (dry ice) at -78.5°C to gaseous carbon dioxide at 1 atm and 25°C given that the enthalpy of formation of solid carbon dioxide and gaseous carbon dioxide are -393.5 kJ/mol and -393.5 kJ/mol, respectively.

asked 2 days ago in Chemical thermodynamics by RenaUxo07372 (470 points)

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1 answer 32 views

Calculate the standard enthalpy change for the phase transition reaction of solid calcium carbonate (CaCO3) to gaseous carbon dioxide (CO2) at 298 K, given the following formation enthalpies: ΔHf°(CaCO3) = -1206.9 kJ/mol ΔHf°(CO2) = -393.5 kJ/mol Also, assume that the specific heat capacity of CaCO3 is 0.82 J/g·K and that of CO2 is 0.85 J/g·K.

asked 2 days ago in Chemical thermodynamics by QSALea374924 (330 points)

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Calculate the standard enthalpy change for the phase transition reaction of solid ammonium nitrate (NH4NO3) to gaseous NH3 and NO2, given that the standard enthalpy of formation for solid NH4NO3 is -365.5 kJ/mol, the standard enthalpy of formation for NH3(g) is -46.1 kJ/mol, and the standard enthalpy of formation for NO2(g) is 33.2 kJ/mol.

asked 2 days ago in Chemical thermodynamics by IleneMarou56 (430 points)

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