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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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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 AdelaideYwt4 (1.6k 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 JordanChun58 (2.3k 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 LXJGinger283 (2.2k 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 AlisiaBarwel (2.1k 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 NicholeBlade (2.1k points)

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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 JannetteBarr (2.2k points)

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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 SusannahCrow (2.4k points)

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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 CooperPallad (1.7k points)

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Calculate the enthalpy change for the oxidation of methane (CH4) to carbon dioxide (CO2) at constant pressure using the following reactions: * C(s) + O2(g) --> CO2(g) ΔH = -393.5 kJ/mol* 2H2(g) + O2(g) --> 2H2O(l) ΔH = -571.6 kJ/molThe enthalpy of formation of CH4(g) is -74.8 kJ/mol.

asked Jan 23 in ThermoChemistry by JaredOliva6 (2.2k points)

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Calculate the enthalpy change for the oxidation of 5 moles of hydrogen gas using the standard enthalpies of formation of water and hydrogen gas.

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

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Calculate the enthalpy change for the oxidation of 25 grams of iron (Fe) to form iron(III) oxide (Fe2O3) using the balanced chemical equation and the given enthalpy of formation values for Fe(s) and Fe2O3(s).

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

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Calculate the enthalpy change for the oxidation of 2 moles of iron, given the standard enthalpy of formation for FeO is -272.2 kJ/mol and that of Fe2O3 is -824 kJ/mol.

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

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1 answer 60 views

Calculate the enthalpy change for the oxidation of 10 moles of carbon monoxide (CO) to carbon dioxide (CO2) using the enthalpy of formation values given below:∆Hf CO = -110.5 kJ/mol ∆Hf CO2 = -393.5 kJ/mol

asked Jan 23 in ThermoChemistry by JadaMeece33 (1.6k points)

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Calculate the enthalpy change for the oxidation of 1 mole of methane gas to form carbon dioxide and water vapor, given the following balanced chemical equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)(enthalpy of formation: ΔHf(CH4)=-74.81 kJ/mol, ΔHf(CO2)=-393.51 kJ/mol, ΔHf(H2O)= -241.83 kJ/mol)

asked Jan 23 in ThermoChemistry by LawrenceShel (1.6k points)

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