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Calculate the standard enthalpy of formation for hydrogen peroxide (H2O2) at 298 K, given that the standard enthalpy change of formation for water (H2O) is -285.8 kJ/mol and the standard enthalpy change of formation for oxygen gas (O2) is 0 kJ/mol.

asked 4 days ago in Chemical thermodynamics by MaryanneKuef (390 points)

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Can the unique photophysical properties of lanthanide complexes be harnessed for efficient light harvesting and photocatalysis? Explore the photochemical properties of selected lanthanide complexes to demonstrate their potential applications in these fields.

asked 4 days ago in PhotoChemistry by RyanAskins6 (510 points)

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Calculate the standard free energy change for the following redox reaction:2HgO(s) → 2Hg(l) + O2(g)Given: ΔG°f (HgO) = -90.83 kJ/molΔG°f (Hg) = 0 kJ/mol ΔG°f (O2) = 0 kJ/mol.

asked 4 days ago in Chemical thermodynamics by Latanya48975 (350 points)

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Can the chemical modification of a polymer affect its optical properties and if so, how can we design a polymer with unique optical properties for use in advanced optical materials?

asked 4 days ago in Polymer Chemistry by AnibalTimm8 (550 points)

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Calculate the standard free energy change for the following redox reaction under standard conditions:2 Fe3+ (aq) + H2 (g) → 2 Fe2+ (aq) + 2 H+ (aq)Given: Standard reduction potential of Fe3+ / Fe2+ = -0.771 V Standard reduction potential of H+ / H2 = 0.00 V

asked 4 days ago in Chemical thermodynamics by BennieHeitma (710 points)

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Design a chemical reactor for the production of ethylene oxide through the direct oxidation of ethylene. The reactor should have a production rate of 100 tons per day and maintain a constant temperature of 250°C. Assume a feed composition of 90% ethylene and 10% oxygen. The reactor should also have a conversion efficiency of at least 95%. Compute the necessary reactor volume and the optimal flow rate of ethylene and oxygen to achieve the desired production rate and conversion efficiency.

asked 4 days ago in Chemical engineering by CruzFehon13 (290 points)

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Calculate the standard enthalpy change for the reaction where 3 moles of hydrogen gas react with 1 mole of nitrogen gas to form 2 moles of ammonia gas. Given the following thermochemical equation: N2(g) + 3 H2(g) → 2 NH3(g) ΔH° = −92.4 kJ/mol

asked 4 days ago in Chemical thermodynamics by PenniSalaam4 (430 points)

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Calculate the standard enthalpy change for the reaction of 25.0 mL of 0.100 M HCl with 25.0 mL of 0.100 M NaOH at 25°C, given that the specific heat capacity of the solution is 4.18 J/g°C and the density of the solution is 1.00 g/mL. The balanced chemical equation for the reaction is:HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) Assume the heat of the reaction is absorbed by the solution and the reaction has reached equilibrium.

asked 4 days ago in Chemical thermodynamics by JustineDez22 (470 points)

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Consider the electrochemical cell with the following half-cell reactions: Fe3+ (aq) + e- → Fe2+ (aq) E° = +0.771 V and Cd2+ (aq) + 2e- → Cd (s) E° = -0.403 V What is the overall cell potential, Ecell, under standard conditions? Which species will be reduced at the cathode? Which electrode is the anode? Justify your choices using the given standard reduction potentials.

asked 4 days ago in ElectroChemistry by IolaMunn388 (390 points)

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Calculate the standard entropy change for the reaction: 2SO3(g) + O2(g) → 2SO4(g) Given the following standard entropies of formation: ΔS°f SO3(g) = 256.2 J/K mol ΔS°f O2(g) = 205.0 J/K mol ΔS°f SO4(g) = 296.8 J/K mol

asked 4 days ago in Inorganic Chemistry by AngelinaOrch (490 points)

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Calculate the standard entropy change for the following reaction at 298 K:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) Given the standard entropies of CH4(g), O2(g), CO2(g), and H2O(l) are 186.26 J/K/mol, 205.03 J/K/mol, 213.74 J/K/mol, and 69.95 J/K/mol respectively.

asked 4 days ago in Chemical thermodynamics by Catharine458 (550 points)

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How does changing the temperature of a chemical reaction affect the activation energy barrier in the reaction? Use computational chemistry and molecular modeling to calculate the activation energy barriers for the same reaction at different temperatures and explain the change in activation energy with temperature.

asked 4 days ago in Physical Chemistry by BryceFawsitt (350 points)

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Calculate the standard enthalpy change for the reaction between hydrochloric acid (HCl) and ammonia (NH3) to produce ammonium chloride (NH4Cl) if the reaction is carried out in a solution of water (H2O), given the following information:HCl(aq) + H2O(l) -> H3O+(aq) + Cl-(aq) ΔH1 = -74.8 kJ/mol NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq) ΔH2 = -51.8 kJ/mol NH4Cl(s) → NH4+(aq) + Cl-(aq) ΔH3 = 15.2 kJ/mol Ensure that the answer is in kJ/mol.

asked 4 days ago in Chemical thermodynamics by QOBGertrude3 (350 points)

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Calculate the standard enthalpy change for the reaction between 25 mL of 0.1 M HCl and 25 mL of 0.1 M NaOH, assuming the reaction takes place in aqueous solution and is complete. The temperature of the solutions should be maintained at a constant 25°C during the reaction. (Assume the density of the solutions is 1 g/mL and the specific heat capacity of the solutions is 4.18 J/g°C).

asked 4 days ago in Chemical thermodynamics by OrenSansom9 (490 points)

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Calculate the standard enthalpy change for the fusion reaction of 1 mole of ice at 0°C to 1 mole of liquid water at 0°C. Given the standard enthalpy of fusion of water is 6.02 kJ/mol and the specific heat capacity of water is 4.18 J/(g·°C).

asked 4 days ago in Chemical thermodynamics by Laurence32K (310 points)

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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 4 days ago in Chemical thermodynamics by MireyaReynol (390 points)

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Calculate the standard enthalpy change (∆H°) for the reaction between 50.0 mL of 0.100 M hydrochloric acid (HCl) and 50.0 mL of 0.100 M sodium hydroxide (NaOH), given that the temperature change was -5.01°C and the specific heat capacity of the solution is 4.18 J/g°C. The balanced chemical equation for the reaction is:HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)Note: Assume the density of the solutions is 1.00 g/mL and that the specific heat capacity of the solutions is the same as that of water.

asked 4 days ago in Chemical thermodynamics by JereBrock920 (470 points)

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Calculate the standard enthalpy change for the reaction: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(g) Given the necessary bond enthalpies are: C-H = 411 kJ/molO=O = 495 kJ/molO-H = 463 kJ/molC=O = 799 kJ/mol.

asked 4 days ago in Quantum Chemistry by FriedaGreine (710 points)

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Calculate the standard enthalpy change for the formation of methane (CH4) from its elements carbon (C) and hydrogen (H2) at standard conditions, given the following thermodynamic data: ΔHf(C) = 0 kJ/molΔHf(H2) = 0 kJ/molΔHc(CH4) = -890.3 kJ/mol

asked 4 days ago in Chemical thermodynamics by GordonChoate (470 points)

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Calculate the standard enthalpy of formation (ΔH°f) for butane (C4H10) given the following data:ΔH°f (kJ/mol)C(s) 0H2(g) 0C2H6(g) -84.7C3H8(g) -103.8Note: You may assume that butane undergoes complete combustion to form CO2(g) and H2O(l) and that the standard enthalpies of combustion for C4H10, CO2, and H2O are -2877.2, -393.5, and -285.8 kJ/mol, respectively.

asked 4 days ago in Chemical thermodynamics by RaquelGendro (430 points)

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