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Calculate the standard enthalpy change (ΔH°), standard entropy change (ΔS°) and standard Gibbs free energy change (ΔG°) of the reaction:2A(g) + 3B(g) → C(g) + 2D(g)given thatΔH°f[A(g)] = 200 kJ mol^-1Δ H°f [B(g)] = 100 kJ mol^-1Δ H°f [C(g)] = 400 kJ mol^-1Δ H°f [D(g)] = 0 kJ mol^-1ΔH°= -400 kJ mol^-1Temperature (T) = 298 KThe student needs to use their knowledge in quantum chemistry and thermodynamics to calculate the thermodynamic properties of the given reaction.

asked Feb 3 in Quantum Chemistry by MireyaFlaher (1.6k points)

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Calculate the standard enthalpy change (ΔH°) for the reduction of iron(III) oxide (Fe2O3) to iron (Fe) given the following balanced chemical equation:2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g)The enthalpy of formation for Fe2O3(s) is -824.2 kJ/mol and the enthalpy of formation for CO2(g) is -393.5 kJ/mol. All other substances are in their standard state.

asked Feb 3 in ThermoChemistry by AlphonsoKirk (2.1k points)

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1 answer 166 views

Calculate the standard enthalpy change (ΔH°) for the reaction:2H2(g) + O2(g) → 2H2O(g)given the following bond energies:H-H = 436 kJ/mol, O=O = 498 kJ/mol, H-O = 463 kJ/mol

asked Feb 3 in Quantum Chemistry by BeverlyNavar (1.8k points)

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1 answer 181 views

Calculate the standard enthalpy change (ΔH°) for the reaction where 50.0 mL of 2.0 M hydrochloric acid reacts with 50.0 mL of 2.0 M sodium hydroxide to form 50.0 mL of 2.0 M sodium chloride and water, given that the density of the solutions is 1.00 g/mL and the specific heat capacity of the solutions is 4.18 J/g·°C.

asked Feb 3 in Chemical thermodynamics by MichaelBirds (2.0k points)

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1 answer 126 views

Calculate the standard enthalpy change (ΔH°) for the reaction where 1 mol of solid sodium hydroxide (NaOH) dissolves in excess water to produce 1 mol of aqueous solution and releases heat. Given that the standard enthalpy of formation (ΔH°f) for NaOH(s) is -425.6 kJ/mol, the heat capacity of the aqueous solution is 4.18 J/gK, and the change in temperature (ΔT) is observed to be 8.0°C for 250 g of the solution.

asked Feb 3 in Chemical thermodynamics by MeredithFeg5 (1.6k points)

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1 answer 134 views

Calculate the standard enthalpy change (ΔH°) for the reaction of combustion of 1 mole of ethanol (C2H5OH) given that the standard enthalpy of formation (ΔH°f) for ethanol and carbon dioxide (CO2) are -277.7 kJ/mol and -393.5 kJ/mol respectively, and the standard enthalpy of formation (ΔH°f) for water (H2O) is -285.8 kJ/mol. The balanced chemical equation for the reaction is as follows:C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (l)

asked Feb 3 in Chemical thermodynamics by JacquelynWil (1.7k points)

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Calculate the standard enthalpy change (ΔH°) for the phase transition reaction of ice to water, given that the enthalpy of fusion for ice is 6.01 kJ/mol and the specific heat capacity of water is 4.18 J/g·°C. Express your answer in kJ/mol.

asked Feb 3 in Chemical thermodynamics by CletaF793120 (2.8k points)

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1 answer 143 views

Calculate the standard enthalpy change (ΔH°) for the following reaction involving the coordination compound [Fe(H2O)6]2+:[Fe(H2O)6]2+(aq) + 2Cl-(aq) → [FeCl2(H2O)4](aq) + 2H2O(l) Given: ΔH°f [FeCl2(H2O)4](aq) = -334 kJ/mol ΔH°f [Fe(H2O)6]2+(aq) = -393 kJ/mol ΔH°f H2O(l) = -286 kJ/mol Note: The superscript ° denotes standard conditions (i.e. 1 atm and 25°C) and the superscript f denotes standard enthalpy of formation.

asked Feb 3 in Chemical thermodynamics by CharmainHers (1.6k points)

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1 answer 87 views

Calculate the standard enthalpy change (ΔH°) for the following reaction at 298 K:2SO₂(g) + O₂(g) → 2SO₃(g)given the following standard enthalpy of formation values:ΔH°f (SO₂(g)) = -296.8 kJ/molΔH°f (O₂(g)) = 0 kJ/molΔH°f (SO₃(g)) = -395.7 kJ/mol

asked Feb 3 in Chemical thermodynamics by OliviaMilton (2.0k points)

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1 answer 116 views

Calculate the standard enthalpy change (ΔH°) for the following reaction at 25°C, given that the enthalpies of formation for the reactants and products are:HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)ΔH°f[HCl (aq)] = -92.31 kJ/molΔH°f[NaOH (aq)] = -469.49 kJ/molΔH°f[NaCl (aq)] = -407.29 kJ/molΔH°f[H2O (l)] = -285.83 kJ/mol

asked Feb 3 in Chemical thermodynamics by Ashleigh66X2 (1.9k points)

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1 answer 176 views

Calculate the standard enthalpy change (ΔH°) for the combustion reaction of ethanol (C2H5OH) if the heat evolved is 1367.6 kJ and the molar mass of ethanol is 46.07 g/mol.

asked Feb 3 in Chemical thermodynamics by RudyMms5536 (1.8k points)

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1 answer 95 views

Calculate the standard enthalpy change (ΔH°) and standard entropy change (ΔS°) for the decomposition reaction of calcium carbonate (CaCO3) at 298 K:CaCO3(s) → CaO(s) + CO2(g)

asked Feb 3 in Inorganic Chemistry by MoniqueBrins (1.9k points)

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Calculate the standard enthalpy change (in kJ/mol) for the reaction of hydrochloric acid (HCl) and sodium hydroxide (NaOH) to form sodium chloride (NaCl) and water (H2O), given the following balanced chemical equation:HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)Assume the reaction takes place under standard conditions (298 K and 1 atm pressure) and that all solutions have a concentration of 1.0 M. The standard enthalpies of formation for HCl (aq), NaOH (aq), NaCl (aq), and H2O (l) are -92.31 kJ/mol, -469.14 kJ/mol, -407.76 kJ/mol, and -285.83 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by JacquelynDos (1.7k points)

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Calculate the standard enthalpy change (in kJ/mol) for the neutralization reaction of hydrochloric acid (HCl) and sodium hydroxide (NaOH) using the following information: HCl (aq) + NaOH (aq) → NaCl (aq) + H2O(l)ΔHf° (kJ/mol): HCl (aq) = -167.2 NaOH (aq) = -469.2 NaCl (aq) = -407.3 H2O(l) = -285.8

asked Feb 3 in Chemical thermodynamics by RachelMcCann (2.2k points)

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1 answer 142 views

Calculate the standard enthalpy change (in kJ/mol) for the following reaction involving solutions: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)Given the following enthalpy values:NaOH(aq): -469.2 kJ/mol HCl(aq): -167.2 kJ/mol NaCl(aq): -411.2 kJ/mol H2O(l): -285.8 kJ/mol

asked Feb 3 in Chemical thermodynamics by MuhammadNuna (2.1k points)

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1 answer 135 views

Calculate the standard enthalpy change (in kJ/mol) for the following chemical reaction at 298 K:2SO2(g) + O2(g) → 2SO3(g)Given the standard enthalpies of formation (∆Hf°) at 298 K for SO2(g), O2(g), and SO3(g) are -296.8 kJ/mol, 0 kJ/mol, and -396.0 kJ/mol, respectively.

asked Feb 3 in Physical Chemistry by ClarkPuig93 (2.0k points)

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1 answer 132 views

Calculate the standard enthalpy change (in kJ/mol) for the dissolution of 3.50 g of potassium hydroxide (KOH) in 250.0 mL of water at 25°C, given that the molar heat of solution of KOH is -57.61 kJ/mol.

asked Feb 3 in Chemical thermodynamics by CharleneLemu (1.7k points)

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1 answer 124 views

Calculate the standard enthalpy change (∆H°) of combustion for methane gas (CH4) given that the heat of formation (∆Hf°) for methane is -74.87 kJ/mol and the heat of formation (∆Hf°) for carbon dioxide (CO2) is -393.51 kJ/mol, and the heat of formation (∆Hf°) for water (H2O) is -285.83 kJ/mol.

asked Feb 3 in Chemical thermodynamics by StanGjo3033 (1.9k points)

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1 answer 115 views

Calculate the standard enthalpy change (∆H°) for the vaporization of 10 grams of water at 100°C, given that the molar heat of vaporization of water is 40.7 kJ/mol.

asked Feb 3 in Chemical thermodynamics by MelbaTulloch (2.2k points)

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1 answer 191 views

Calculate the standard enthalpy change (∆H°) for the reaction: NaOH(aq) + HCl(aq) -> NaCl(aq) + H2O(l) given the following information: - The enthalpy change of neutralization of HCl(aq) with NaOH(aq) is -55.9 kJ/mol. - The enthalpy of formation of NaCl(s) is -411.2 kJ/mol.- The enthalpy of vaporization of water (H2O) is 40.7 kJ/mol.Assume that the specific heat capacity of the water is 4.18 J/g K and the density of the solution is 1 g/mL.

asked Feb 3 in Chemical thermodynamics by PeggyBednall (1.9k points)

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