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How does changing the temperature affect the conformational properties and behavior of a polymer chain in a Monte Carlo simulation?

asked Feb 3 in Computational Chemistry by VHBMorgan997 (450 points)

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Calculate the standard electrode potential for the reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) Given that the standard electrode potentials for the half-reactions are: Zn2+(aq) + 2e- → Zn(s) Etheta = -0.76 V Cu2+(aq) + 2e- → Cu(s) Etheta = 0.34 V

asked Feb 3 in ElectroChemistry by HenriettaDul (410 points)

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1 answer 29 views

Calculate the standard enthalpy change for the complete combustion of methane gas (CH4(g)) at constant pressure, given the balanced equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l). The standard enthalpies of formation of CO2(g), H2O(l), and CH4(g) are -393.5 kJ/mol, -285.8 kJ/mol, and -74.8 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by Brian0571409 (530 points)

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Calculate the standard enthalpy change for the melting of 10 grams of ice at -10°C to liquid water at 20°C, given the specific heat capacity of water is 4.18 J/g°C and the enthalpy of fusion of water is 6.01 kJ/mol.

asked Feb 3 in Chemical thermodynamics by VCSKarol0571 (350 points)

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1 answer 35 views

Calculate the number of electrons transferred when a solution containing 0.25 M Ni(NO3)2 is electrolyzed using a current of 0.50 A for 2.0 hours. The reaction taking place is Ni2+ (aq) + 2e- --> Ni (s).

asked Feb 3 in ElectroChemistry by DexterKier30 (330 points)

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1 answer 40 views

How does changing the ligands of a coordination compound affect its photochemical properties? Provide three specific examples with explanations.

asked Feb 3 in PhotoChemistry by BrendaBurche (390 points)

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1 answer 25 views

Calculate the standard enthalpy of formation of carbon dioxide from its elements under standard conditions given the following information:- The standard enthalpy of combustion of carbon to CO2 is -393.5 kJ/mol- The standard enthalpy of combustion of hydrogen to H2O is -285.8 kJ/mol- The standard enthalpy of formation of water is -241.8 kJ/mol.Note: The standard enthalpy of formation of an element in its standard state is zero.

asked Feb 3 in ThermoChemistry by RafaelaReddy (470 points)

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1 answer 29 views

Calculate the standard enthalpy change for the combustion of 1 mole of propane gas (C3H8) at standard conditions using the following balanced chemical equation: C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(l)Given the standard enthalpy of formation values at 298K for C3H8(g), CO2(g), and H2O(l) as -103.8, -393.5, and -285.8 kJ/mol respectively, calculate the standard enthalpy change for the combustion reaction.

asked Feb 3 in Chemical thermodynamics by JosephineAyc (470 points)

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1 answer 24 views

Calculate the standard Gibbs free energy change (ΔG°) for the following electrochemical reaction:Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)Given: - Standard reduction potential for the half-reaction: Cu²⁺(aq) + 2e⁻ → Cu(s) E° = +0.34 V Ag⁺(aq) + e⁻ → Ag(s) E° = +0.80 V

asked Feb 3 in ElectroChemistry by BurtonSteger (370 points)

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1 answer 40 views

How does changing the geometry of a molecule affect its excited state properties, such as the energy levels and transition probabilities, as predicted by quantum chemical calculations?

asked Feb 3 in Computational Chemistry by Celia30F8145 (570 points)

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1 answer 23 views

Chemistry student, can you predict the products and balance the following double replacement chemical reaction: NaCl + AgNO3?

asked Feb 3 in Chemical reactions by RafaelBeards (450 points)

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1 answer 31 views

Calculate the standard enthalpy change (∆H°) for the reaction of the coordination compound [Co(NH3)6]Cl3 (aq) with NaOH (aq) to produce [Co(NH3)6](OH)3 (aq) and NaCl (aq). Given, the standard enthalpy of formation (∆H°f) for [Co(NH3)6]Cl3, [Co(NH3)6](OH)3 and NaCl are -784.8 kJ/mol, -1273.6 kJ/mol and -411.2 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by AlfredoHuber (350 points)

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1 answer 40 views

How does changing the geometry and size of a molecule affect its electronic excited states and optical properties, and how can this information be accurately calculated using quantum chemistry methods?

asked Feb 3 in Quantum Chemistry by BarrettVep43 (250 points)

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1 answer 26 views

Calculate the standard enthalpy change for the reaction: 2NaOH (s) + H2SO4 (aq) → Na2SO4 (aq) + 2H2O (l)given that the standard enthalpy of formation of Na2SO4 (aq) is -1385 kJ/mol, and the standard enthalpies of formation of NaOH (s), H2SO4 (aq) and H2O (l) are -425 kJ/mol, -814 kJ/mol and -286 kJ/mol respectively.

asked Feb 3 in Chemical thermodynamics by TeresaFiorin (490 points)

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1 answer 31 views

Calculate the standard enthalpy change (∆H°) for the dissolution reaction of 5.00 grams of sodium chloride (NaCl) in 100.0 mL of water, given that the final temperature of the solution was 25.0°C and the heat capacity of the solution was 4.18 J/g°C. The molar mass of NaCl is 58.44 g/mol and the density of water is 1.00 g/mL.

asked Feb 3 in Chemical thermodynamics by TerrellWnq0 (170 points)

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1 answer 34 views

Calculate the power output for a Zinc-Copper electrochemical cell operating at standard conditions with a Zinc electrode that measures 10 cm by 12 cm and a Copper electrode that measures 8 cm by 10 cm. The current flowing through the circuit is 0.5 A. The standard reduction potentials for the half-reactions are +0.76 V for Cu2+/Cu and -0.76 V for Zn2+/Zn.

asked Feb 3 in ElectroChemistry by KingCopland (310 points)

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1 answer 28 views

Calculate the standard enthalpy change for the formation of ethylene glycol (C2H6O2) from its elements given that the standard enthalpies of formation of carbon dioxide, water, and ethylene glycol are -393.5 kJ/mol, -285.8 kJ/mol, and -421.1 kJ/mol respectively.

asked Feb 3 in Chemical thermodynamics by EuniceTalari (150 points)

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1 answer 28 views

Calculate the standard enthalpy change for the formation of carbon dioxide (CO2) from its elements, given the following standard enthalpies of formation:ΔHf°(CO2) = -393.5 kJ/molΔHf°(C) = 0 kJ/molΔHf°(O2) = 0 kJ/mol

asked Feb 3 in Chemical thermodynamics by SalvadorSchr (290 points)

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1 answer 27 views

Calculate the standard enthalpy change for the phase transition reaction of solid carbon dioxide (dry ice) at -78.5°C to gaseous carbon dioxide at 1 atm and 25°C given that the enthalpy of formation of solid carbon dioxide and gaseous carbon dioxide are -393.5 kJ/mol and -393.5 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by Ofelia983738 (690 points)

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1 answer 25 views

Calculate the standard enthalpy change of the oxidation of hydrogen gas (H2) to form water (H2O) at 298 K, given that the standard enthalpy of formation of water is -285.8 kJ/mol and the bond dissociation enthalpy of the H-H bond is 436 kJ/mol.

asked Feb 3 in ThermoChemistry by LaurenDelpra (210 points)

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