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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 RhysAltman92 (190 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 HelenaGass02 (250 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 BryceWhittel (310 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 RosariaLomba (470 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 LaureneLeves (350 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 ToddMcdowell (370 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 ZaneSeiler9 (350 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 LaraeWicks2 (270 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 RosalindTarl (370 points)

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1 answer 60 views

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 QJCStuart42 (610 points)

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1 answer 54 views

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 ShelleyC9050 (430 points)

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1 answer 76 views

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 AmosDeBernal (510 points)

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1 answer 50 views

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 878041975522 (270 points)

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1 answer 55 views

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 CyrusGeogheg (450 points)

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1 answer 70 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 Julio140610 (130 points)

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1 answer 49 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 GilbertoVall (330 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 BudTruong728 (570 points)

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1 answer 61 views

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 MarshaReiss (330 points)

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1 answer 53 views

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 Phillis17Z51 (310 points)

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1 answer 59 views

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 JerrellBodin (250 points)

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