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Calculate the enthalpy change of adsorption when 2.5 moles of nitrogen gas are adsorbed onto 10 g of activated charcoal at 298 K, given that the pressure of nitrogen gas is 1.0 atm. The molar mass of nitrogen is 28 g/mol, and the initial pressure of nitrogen is 0.5 atm.

asked Jan 23 in ThermoChemistry by CarmellaBibl (2.0k points)

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Calculate the enthalpy change of adsorption for the adsorption of CO gas on activated carbon at 25°C, given that the equilibrium constant for the reaction is 1.5×10^3 L/mol and the molar density of CO is 1.25 g/L. The surface area of activated carbon used is 50 m^2/g, and the initial pressure of CO is 2.5 atm.

asked Jan 23 in ThermoChemistry by TammiTolbert (2.1k points)

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Calculate the enthalpy change involved in the precipitation reaction between 50ml of 0.1 M lead nitrate solution and 50ml of 0.1 M sodium chloride solution at a constant temperature of 25°C. The balanced chemical equation for the reaction is Pb(NO3)2 + 2NaCl → PbCl2 + 2NaNO3. Standard enthalpies of formation for Pb(NO3)2, NaCl, PbCl2, and NaNO3 are -460.56 kJ/mol, -407.33 kJ/mol, -359.57 kJ/mol, and -467.93 kJ/mol respectively.

asked Jan 23 in ThermoChemistry by Bev611336790 (1.8k points)

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Calculate the enthalpy change in kJ/mol for the combustion of butane (C4H10) given that the heat of formation of CO2(g) is -393.5 kJ/mol, the heat of formation of H2O(l) is -285.8 kJ/mol, and the heat of formation of C4H10(g) is -126 kJ/mol. The balanced equation for the combustion of butane is:2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l) + heat.

asked Jan 23 in ThermoChemistry by SelmaHartsoc (1.8k points)

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Calculate the enthalpy change for the reduction of iron (III) oxide using carbon in a thermite reaction if 12.5 grams of iron (III) oxide reacts with excess carbon, and the resulting iron has a mass of 7.5 grams. Assume all heat evolved is absorbed by the iron and that the reaction occurs at constant pressure.

asked Jan 23 in ThermoChemistry by SusannahRose (1.3k points)

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Calculate the enthalpy change for the reaction: 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) given the enthalpies of formation of H2O(g), SO2(g), and H2S(g) are -241.8 kJ/mol, -296.8 kJ/mol, and -20.2 kJ/mol, respectively.

asked Jan 23 in ThermoChemistry by WyattBriones (1.9k points)

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Calculate the enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(l)given that the enthalpy change of formation for water (H2O) is -285.8 kJ/mol.

asked Jan 23 in Chemical thermodynamics by TerrieGaffne (1.6k points)

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Calculate the enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(l) using Hess's law given the following reactions: 2H2(g) + O2(g) → 2H2O(g) ΔH1 = -483.6 kJ/mol 2H2O(g) → 2H2O(l) ΔH2 = -40.7 kJ/mol

asked Jan 23 in ThermoChemistry by KrystleDHage (2.0k points)

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Calculate the enthalpy change for the reaction: 2H₂(g) + O₂(g) → 2H₂O(g) The enthalpy of formation of H₂O is -242 kJ/mol, and the enthalpy of formation of O₂ is 0 kJ/mol.

asked Jan 23 in ThermoChemistry by MercedesLang (2.2k points)

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Calculate the enthalpy change for the reaction: 2H2(g) + O2(g) --> 2H2O(g) given the following enthalpy changes: H2(g) + 1/2O2(g) --> H2O(g) ΔH1 = -286 kJ/molH2(g) + 1/2Cl2(g) --> HCl(g) ΔH2 = -92 kJ/mol Cl2(g) --> 2Cl(g) ΔH3 = +242 kJ/molHCl(g) + 1/2O2(g) --> H2O(g) + Cl2(g) ΔH4 = -184 kJ/mol

asked Jan 23 in Chemical reactions by SheilaSchaef (1.8k points)

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Calculate the enthalpy change for the reaction: 2H2O(l) → 2H2(g) + O2(g) given the following bond enthalpies: H-H (436 kJ/mol), O=O (498 kJ/mol), H-O (463 kJ/mol). Is the reaction exothermic or endothermic?

asked Jan 23 in Chemical thermodynamics by JanisButterf (2.1k points)

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Calculate the enthalpy change for the reaction: 2H2 (g) + O2 (g) → 2H2O (l) given that the standard enthalpy of formation for water is -285.8 kJ/mol, and standard enthalpies of formation of H2 (g) and O2 (g) are 0 kJ/mol.

asked Jan 23 in Chemical thermodynamics by KaraMcRae960 (2.5k points)

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Calculate the enthalpy change for the reaction of burning 1 mole of methane using Hess's Law, given the following information:1) Enthalpy of formation for methane = -74.8 kJ/mol2) Enthalpy of combustion for methane = -890.3 kJ/mol3) Enthalpy of formation for water = -285.8 kJ/mol4) Enthalpy of formation for carbon dioxide = -393.5 kJ/mol

asked Jan 23 in ThermoChemistry by HiramFarrell (1.7k points)

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Calculate the enthalpy change for the reaction of 2.5 g of hydrogen gas with excess oxygen gas to produce water, given that the enthalpy of formation of water is -285.83 kJ/mol and the molar mass of hydrogen gas is 2.02 g/mol.

asked Jan 23 in ThermoChemistry by SamMph085344 (2.4k points)

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Calculate the enthalpy change for the reaction below using the given bond dissociation energies:2HBr (g) + Cl2 (g) -> 2HCl (g) + Br2 (g)Bond dissociation energies:H-H = 436 kJ/molBr-Br = 193 kJ/molH-Br = 366 kJ/molCl-Cl = 242 kJ/molH-Cl = 431 kJ/mol

asked Jan 23 in Chemical reactions by AugustBranno (2.5k points)

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Calculate the enthalpy change for the reaction below using Hess's Law: 2CO(g) + O2(g) -> 2CO2(g), delta H = -566 kJ/mol Given the following reactions and their corresponding enthalpy changes: CO(g) + 1/2O2(g) -> CO2(g), delta H = -283 kJ/molC(s) + O2(g) -> CO2(g), delta H = -393.5 kJ/mol

asked Jan 23 in ThermoChemistry by HalinaAlderm (1.9k points)

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Calculate the enthalpy change for the reaction below using Hess's Law and the given thermochemical equations:2H2(g) + O2(g) -> 2H2O(g) deltaH1 = -484 kJ/molH2(g) + 1/2O2(g) -> H2O(g) deltaH2 = -242 kJ/mol 2H2O(g) -> 2H2(g) + O2(g) deltaH3 = +484 kJ/mol

asked Jan 23 in ThermoChemistry by SueCasteel38 (1.4k points)

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Calculate the enthalpy change for the process of desorption of carbon dioxide from a zeolite adsorbent at a temperature of 298 K, given that the heat of adsorption for carbon dioxide on the same zeolite at the same temperature is -40 kJ/mol.

asked Jan 23 in ThermoChemistry by GarnetFjo447 (1.8k points)

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Calculate the enthalpy change for the precipitation reaction that occurs when 50.0 mL of 0.100 M AgNO3 (aq) and 25.0 mL of 0.100 M NaCl (aq) are mixed together. The final temperature of the solution is 25.0°C, and the initial temperature of both solutions was 25.0°C. The heat capacity of the solution is 4.18 J/(g °C) and the density of each solution is 1.00 g/mL. Assume that the reaction goes to completion and that the density and specific heat capacity of the resulting solution are the same as those of pure water.

asked Jan 23 in ThermoChemistry by WilburnMcCor (1.8k points)

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Calculate the enthalpy change for the precipitation reaction of barium chloride and sodium sulfate, given that the initial concentrations of the two solutions are 0.2 M and are mixed in a coffee cup calorimeter. The final temperature observed is 25°C and the heat capacity of the coffee cup is 10 J/°C.

asked Jan 23 in ThermoChemistry by ErikaStephen (2.4k points)

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