Recent questions in ThermoChemistry

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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 CandiceLabou (580 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 ElaneLavarac (590 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 CaitlinLaros (490 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 Elisabeth544 (190 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 HughLarge668 (590 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 JohnettePass (430 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 MerryJonas8 (310 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 LillieHussai (530 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 CarriKdt2125 (290 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 TeresaSchran (410 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 LincolnElsto (390 points)

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1 answer 60 views

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 EleanoreWitc (230 points)

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1 answer 48 views

Calculate the enthalpy change for the precipitation reaction between 50.0 mL of 0.150 M silver nitrate solution and excess sodium chloride solution if the temperature change was measured to be -5.47°C. The molar mass of AgNO3 is 169.87 g/mol, and the density of the silver nitrate solution is 1.05 g/mL. The reaction is as follows: AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq).

asked Jan 23 in ThermoChemistry by MickiWedgwoo (490 points)

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Calculate the enthalpy change for the precipitation reaction between 25.0 mL of 0.100 M silver nitrate (AgNO3) and excess calcium chloride (CaCl2) solution at 25°C. The balanced equation for the reaction is:AgNO3(aq) + CaCl2(aq) → AgCl(s) + Ca(NO3)2(aq)Assume the density of the solutions is equal to 1.00 g/mL and the solutions have the same specific heat as water (4.18 J/g°C).

asked Jan 23 in ThermoChemistry by JannetteVdl (650 points)

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Calculate the enthalpy change for the polymerization reaction of ethylene to form polyethylene using the bond dissociation energies listed below: C-H bond energy = 413 kJ/mol C=C bond energy = 602 kJ/mol Assume that the polymerization reaction proceeds via breaking of the C=C bond followed by formation of the C-C bond in polyethylene.

asked Jan 23 in ThermoChemistry by PMBJamila017 (350 points)

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Calculate the enthalpy change for the polymerization of propylene to polypropylene, given the enthalpy of formation of propylene is -103.8 kJ/mol and the enthalpy of formation of polypropylene is -45.4 kJ/mol. Assume the reaction occurs at constant pressure and temperature.

asked Jan 23 in ThermoChemistry by AaronSoul138 (470 points)

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Calculate the enthalpy change for the polymerization of polyethylene using the following information: ΔHf° of ethylene (-20.4 kJ/mol) and polyethylene (-1024 kJ/mol); the reaction equation: nC2H4 (g) → [-CH2-CH2-]n (s)

asked Jan 23 in ThermoChemistry by ZVWShalanda (590 points)

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1 answer 51 views

Calculate the enthalpy change for the polymerization of ethylene to polyethylene if it is known that the heat of combustion of ethylene is -1411 kJ/mol and the enthalpy of formation of polyethylene is -248 kJ/mol. Assume that the reaction occurs at constant pressure and temperature of 25°C.

asked Jan 23 in ThermoChemistry by AlisonEastwo (660 points)

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1 answer 54 views

Calculate the enthalpy change for the polymerization of 2-methyl-1,3-butadiene (MBC) if 1 mole of MBC is polymerized in a perfectly insulated container at a constant temperature of 25°C. The reaction equation for the polymerization of MBC is given as:nC5H8 (MBC) → (C5H8) (Polymer)Given the bond dissociation energies (in kJ/mol) for the following bonds:C-C bond = 348C-H bond = 413Assume that the enthalpy change of vaporization of MBC is negligible.

asked Jan 23 in ThermoChemistry by BlakeHuffman (570 points)

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1 answer 51 views

Calculate the enthalpy change for the oxidation of methane gas (CH4) to carbon dioxide (CO2) and water (H2O) using the following balanced chemical equation:CH4 (g) + 2O2 (g) -> CO2 (g) + 2H2O (l)The standard enthalpy of formation of methane, carbon dioxide, and water are -74.81 kJ/mol, -393.5 kJ/mol, and -285.83 kJ/mol respectively.

asked Jan 23 in ThermoChemistry by ShaunTulloch (470 points)

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