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Calculate the standard enthalpy change for the reaction: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) Given the following information: ΔHf° [NaOH(aq)] = -469.1 kJ/mol ΔHf° [HCl(aq)] = -167.2 kJ/mol ΔHf° [NaCl(aq)] = -407.3 kJ/mol ΔHf° [H2O(l)] = -286 kJ/mol

asked Feb 3 in Chemical thermodynamics by MacLgq130601 (2.4k points)

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Calculate the standard enthalpy change for the formation of methane gas (CH4) from its elements carbon (solid, graphite) and hydrogen gas (H2) given the following data:ΔHf° (C(graphite)) = 0 kJ/molΔHf° (H2(g)) = 0 kJ/molΔHc° (CH4(g)) = -890.4 kJ/mol

asked Feb 3 in Chemical thermodynamics by OctavioDyaso (2.3k points)

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How does changing the concentration of the reactants affect the rate of reaction and the sustainability of the reaction?

asked Feb 3 in Chemical kinetics by JaimeFuqua07 (2.0k points)

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Calculate the standard enthalpy change for the phase transition reaction of solid carbon dioxide (dry ice) to gaseous carbon dioxide at 298 K and 1 atm pressure, given that the standard enthalpy of sublimation of solid carbon dioxide is 25.2 kJ/mol.

asked Feb 3 in Chemical thermodynamics by KaraMcRae960 (2.5k points)

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Calculate the standard enthalpy change for the formation of ammonia gas from nitrogen gas and hydrogen gas using Hess's Law, given the following equations and their corresponding enthalpy changes:N2(g) + 3H2(g) → 2NH3(g) ∆H = -92.4 kJ/molN2(g) → 2N(g) ∆H = 941 kJ/molH2(g) → 2H(g) ∆H = 436 kJ/mol

asked Feb 3 in ThermoChemistry by CarmellaBibl (2.0k points)

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Calculate the standard enthalpy change (∆H) for the vaporization of 25.0 g of water at its boiling point (100°C) and 1 atm pressure assuming the heat capacity of water to be constant. Given: The heat of vaporization for water is 40.7 kJ/mol and the molar mass of water is 18.015 g/mol.

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

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Calculate the polarization of a copper-silver galvanic cell in which the concentration of copper ions is 0.5 M, the concentration of silver ions is 0.1 M, and the cell is operating at a temperature of 25°C. The potential difference of the cell is measured to be 0.75 V.

asked Feb 3 in ElectroChemistry by VioletteM27 (2.1k points)

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Calculate the standard enthalpy and entropy change for the reaction, given the following information:2 H2(g) + O2(g) → 2 H2O(g)∆H°f [H2O(g)] = -241.8 kJ/mol∆H°f [H2(g)] = 0 kJ/mol∆H°f [O2(g)] = 0 kJ/mol∆S° [H2O(g)] = 188.8 J/Kmol∆S° [H2(g)] = 130.7 J/Kmol∆S° [O2(g)] = 205.2 J/KmolAssuming that all heat capacities are independent of temperature, calculate ∆S°rxn and ∆H°rxn for this reaction.

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

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Calculate the standard entropy change of the following reaction: 2Fe(s) + 3Cl2(g) → 2FeCl3(s) Given that the standard enthalpy change for this reaction is -400 kJ/mol at 298 K and the standard molar entropy of FeCl3(s) is 95 J/mol K.

asked Feb 3 in Inorganic Chemistry by AudreaV25265 (2.0k 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 Feb 3 in Chemical thermodynamics by FletaStepp73 (2.0k points)

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How does changing the volume affect the equilibrium position of a chemical reaction? Provide an example of a reaction and calculate the new equilibrium concentrations when the volume is decreased by a certain factor.

asked Feb 3 in Chemical equilibrium by VioletteM27 (2.1k points)

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Describe the steps involved in the preparation of 2,4-dichlorobenzoic acid from benzoic acid and chlorine gas, including the chemical reactions that occur during the process, the reagents required, the conditions required for each step, and the yields of each intermediate and final product.

asked Feb 3 in Chemical synthesis by NoeX25113136 (1.9k points)

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Consider an electrochemical cell with a copper metal electrode immersed in a solution of copper sulfate, and a platinum electrode in a solution of hydrogen sulfate. The current is measured at 25°C while the cell potential is varied. The following data is obtained for the anodic and cathodic currents:Anodic current:Cell potential (V): 0.20 0.30 0.40 0.50 0.60Current (mA): 1.01 1.80 3.04 4.58 6.25Cathodic current:Cell potential (V): -0.20 -0.30 -0.40 -0.50 -0.60Current (mA): -1.00 -1.79 -3.02 -4.54 -6.19Calculate the anodic and cathodic Tafel slopes for this electrochemical cell.

asked Feb 3 in ElectroChemistry by DebbraCarder (2.3k points)

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1 answer 58 views

Calculate the specific heat capacity of water if it absorbs 400 J of energy and its temperature rises by 20°C.

asked Feb 3 in Chemical thermodynamics by DKGStacy090 (2.4k points)

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Calculate the standard enthalpy of formation of propane (C3H8) given the following data:- Standard enthalpy of formation of CO2(g) = -393.5 kJ/mol- Standard enthalpy of formation of H2O(l) = -285.8 kJ/mol- Standard enthalpy of combustion of propane at constant pressure = -2220.1 kJ/mol

asked Feb 3 in Chemical thermodynamics by NicholasTwm2 (2.0k points)

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1 answer 64 views

How does changing the molecular geometry affect the electronic excited states and optical properties of a molecule?

asked Feb 3 in Quantum Chemistry by RogerDenning (2.4k points)

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Calculate the resistance of an electrochemical cell constructed by using a copper electrode in a 1M copper (II) sulfate solution and a zinc electrode in a 1M zinc sulfate solution. The measured potential difference of the cell is 1.45 volts. The area of each electrode is 10cm² and the length of wire connecting the electrodes is 30cm with a cross-sectional area of 1 mm². The conductivity of copper (II) sulfate and zinc sulfate solutions at the given concentration is 98.3% and 89.9% respectively. What is the resistance (in ohms) of the electrochemical cell?

asked Feb 3 in ElectroChemistry by JeremyCanady (2.1k points)

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Calculate the standard enthalpy change for the sublimation of iodine solid to iodine gas at 298 K with the following given data: - Standard enthalpy of fusion of iodine: 15.52 kJ/mol- Standard molar entropy of iodine solid: 62.7 J/K/mol- Standard molar entropy of iodine gas: 260.6 J/K/mol

asked Feb 3 in Chemical thermodynamics by ArlenBieber1 (1.9k points)

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1 answer 62 views

How does changing the surface chemistry of a solid surface affect the adsorption of proteins, and how can this knowledge be applied to improve biomaterials design for medical implants?

asked Feb 3 in Surface Chemistry by WillieAlgera (1.5k points)

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1 answer 48 views

Calculate the standard Gibbs free energy change for the following electrochemical reaction at 25°C:Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s) Given: E°cell = 0.46 V, F = 96,500 C/mol, R = 8.314 J/K·mol, and the standard reduction potentials at 25°C are Cu²⁺(aq) + 2e⁻ → Cu(s) (E°red = 0.34 V) and Ag⁺(aq) + e⁻ → Ag(s) (E°red = 0.80 V).

asked Feb 3 in ElectroChemistry by CassieClopto (2.4k points)

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