Recent questions in Chemical thermodynamics

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Calculate the standard enthalpy change for the reaction below, given the standard enthalpy of formation values: 2CO(g) + O2(g) → 2CO2(g)ΔH°f (CO) = -110.5 kJ/molΔH°f (O2) = 0 kJ/molΔH°f (CO2) = -393.5 kJ/mol

asked Feb 3 in Chemical thermodynamics by Damon31M1921 (2.4k points)

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1 answer 86 views

Calculate the standard enthalpy change for the reaction 2H2(g) + O2(g) ⟶ 2H2O(g), given that the standard enthalpies of formation of H2(g), O2(g), and H2O(g) are 0 kJ/mol, 0 kJ/mol, and -242 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by JamisonKwan8 (1.7k points)

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1 answer 68 views

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 Feb 3 in Chemical thermodynamics by KyleWaddy213 (1.9k points)

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1 answer 58 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 Feb 3 in Chemical thermodynamics by MoniqueBrins (1.9k points)

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1 answer 74 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 (∆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 Feb 3 in Chemical thermodynamics by ClaritaTrive (2.4k 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 Feb 3 in Chemical thermodynamics by MonikaQuirk7 (2.0k points)

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1 answer 67 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 Feb 3 in Chemical thermodynamics by MaynardErb58 (2.0k points)

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1 answer 45 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 Feb 3 in Chemical thermodynamics by Estella80D9 (2.2k points)

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1 answer 58 views

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 Feb 3 in Chemical thermodynamics by YRPAbe659621 (2.3k points)

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1 answer 71 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 Feb 3 in Chemical thermodynamics by JordanChun58 (2.3k points)

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1 answer 80 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 Feb 3 in Chemical thermodynamics by DeanneMack98 (2.1k points)

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1 answer 61 views

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 Feb 3 in Chemical thermodynamics by CaitlynHoran (1.8k points)

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1 answer 67 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 Feb 3 in Chemical thermodynamics by ElsieBidmead (2.1k points)

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1 answer 44 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 Feb 3 in Chemical thermodynamics by RemonaRainey (1.6k points)

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1 answer 136 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 Feb 3 in Chemical thermodynamics by ElidaHaskins (1.7k points)

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1 answer 76 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 Feb 3 in Chemical thermodynamics by MerissaGxv8 (1.7k points)

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1 answer 82 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 Feb 3 in Chemical thermodynamics by ElkeMary0923 (1.7k points)

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1 answer 79 views

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 Feb 3 in Chemical thermodynamics by KaraMcRae960 (2.5k points)

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1 answer 62 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 Feb 3 in Chemical thermodynamics by NataliaCaple (2.1k points)

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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 Feb 3 in Chemical thermodynamics by KariMcCleary (1.5k points)

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