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Calculate the standard enthalpy change for the reaction between calcium oxide (CaO) and water (H2O) to form calcium hydroxide (Ca(OH)2), given that all species are in their standard state and that the balanced chemical equation is:CaO(s) + H2O(l) → Ca(OH)2(s)The standard enthalpies of formation of CaO(s), H2O(l) and Ca(OH)2(s) are -635.1 kJ/mol, -285.8 kJ/mol, and -986.2 kJ/mol respectively.

asked 4 days ago in Chemical thermodynamics by RyanAskins6 (510 points)

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Calculate the standard enthalpy change for the reaction between Aquapentamminecobalt(III) chloride and sodium hydroxide to form Aquapentamminecobalt(III) hydroxide and sodium chloride if the initial concentration of Co(NH3)5Cl3 is 0.1 M and the reaction takes place at 25°C.

asked 4 days ago in Chemical thermodynamics by PartheniaF00 (570 points)

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Calculate the standard enthalpy change for the reaction between 50.0 mL of 0.200 M HCl(aq) and 50.0 mL of 0.300 M NaOH(aq) at 25°C. The heat capacity of the calorimeter is 9.60 J/°C and the temperature change observed is 4.00°C. Also, assume that the density of both solutions is 1.00 g/mL and that the heat capacity and density of the final solution are the same as that of water.

asked 4 days ago in Chemical thermodynamics by InaLewers025 (330 points)

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Calculate the standard enthalpy change for the reaction between 50 mL of 1.0 M HCl and 50 mL of 1.0 M NaOH at 25°C given that the temperature of the resultant solution is 31.2°C and the specific heat capacity of the solution is 4.184 J/g°C.

asked 4 days ago in Chemical thermodynamics by DanielleBouc (490 points)

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Calculate the standard enthalpy change for the reaction between 50 ml of 0.2 M HCl (aq) and 50 ml of 0.2 M NaOH (aq) at 25°C, given that the specific heat capacity of the combined solution is 4.18 J/g °C and the density of the combined solution is 1.0 g/mL.

asked 4 days ago in Chemical thermodynamics by EtsukoBoston (430 points)

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Calculate the standard enthalpy change for the reaction between 25 mL of 0.1 M HCl and 25 mL of 0.1 M NaOH, assuming the reaction takes place in aqueous solution and is complete. The temperature of the solutions should be maintained at a constant 25°C during the reaction. (Assume the density of the solutions is 1 g/mL and the specific heat capacity of the solutions is 4.18 J/g°C).

asked 4 days ago in Chemical thermodynamics by OrenSansom9 (490 points)

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Calculate the standard enthalpy change for the reaction between 2.00 moles of liquid ethanol (C2H5OH) and 3.50 moles of gaseous oxygen (O2) to form carbon dioxide (CO2) gas and liquid water (H2O) at 25°C and standard pressure. The balanced chemical equation for the reaction is C2H5OH + 3O2 → 2CO2 + 3H2O. (The molar enthalpies of formation for C2H5OH, CO2, and H2O are -277.6 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol, respectively.)

asked 4 days ago in Chemical thermodynamics by MarilouArnde (440 points)

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Calculate the standard enthalpy change for the reaction between [Fe(H2O)6]2+ and 2Cl- ions to produce [FeCl4]2- complex ion given that the enthalpy of formation for [FeCl4]2- is -392 kJ/mol and the enthalpies of hydration for Fe2+ and Cl- ions are -340 kJ/mol and -381 kJ/mol, respectively.

asked 4 days ago in Chemical thermodynamics by ZHAJeanne624 (650 points)

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Calculate the standard enthalpy change for the reaction between [Co(en)2Cl2]Cl and NaNO2 to form [Co(en)2(NO2)2]Cl and NaCl, given the following information: [Co(en)2Cl2]Cl and [Co(en)2(NO2)2]Cl have a ΔHf° of -288 kJ/mol and -136 kJ/mol, respectively. The ΔHf° of NaNO2 and NaCl are -463.2 kJ/mol and -411.2 kJ/mol, respectively. Assume that the reaction is conducted at a constant pressure and temperature of 298 K.

asked 4 days ago in Chemical thermodynamics by JenniferLink (550 points)

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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 4 days ago in Chemical thermodynamics by KatjaMilerum (630 points)

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Calculate the standard enthalpy change for the reaction A(s) + 2B(g) → 3C(l) + D(g) given the following data:• ΔHf° for A(s) is -100 kJ/mol• ΔHf° for C(l) is -50 kJ/mol• ΔS° for the reaction is 450 J/K•mol• ΔS° for D(g) is 200 J/K•mol

asked 4 days ago in Inorganic Chemistry by ShayPicot468 (530 points)

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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 4 days ago in Chemical thermodynamics by PatrickSherr (470 points)

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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 4 days ago in Chemical thermodynamics by JermaineMaue (320 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 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 4 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 4 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 4 days ago in Chemical thermodynamics by KarineTerry (690 points)

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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 4 days ago in Chemical thermodynamics by YYGKarry1452 (620 points)

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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 4 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 4 days ago in Chemical thermodynamics by VedaHoar6953 (730 points)

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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 4 days ago in Chemical thermodynamics by DortheaConsi (770 points)

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