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Calculate the electronegativity difference between carbon and hydrogen atoms in methane (CH4). Show the steps involved in the calculation and explain what the value of the electronegativity difference indicates about the bonding between the atoms.

asked Jan 23 in Chemical bonding by LaureneMcAle (1.8k points)

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Calculate the Gibbs free energy change for the chemical reaction: 2H2O (l) → 2H2 (g) + O2 (g)at a temperature of 298 K, given that the standard Gibbs free energies of formation are ΔGf°(H2O) = -237.13 kJ/mol, ΔGf°(H2) = 0 kJ/mol, and ΔGf°(O2) = 0 kJ/mol.

asked Jan 23 in Chemical thermodynamics by ShaunteYun90 (1.4k points)

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Calculate the enthalpy of ionization of hydrogen atom from hydrogen molecule given that the bond dissociation enthalpy of H2 is 432 kJ/mol and the electron affinity of H atom is -72.8 kJ/mol.

asked Jan 23 in ThermoChemistry by DanielleSauc (2.4k points)

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Calculate the enthalpy of adsorption for the adsorption of hydrogen gas onto a nickel surface at 25°C, given that the equilibrium pressure of hydrogen gas is 0.5 atm and the surface coverage is 0.2 monolayers. The heat of dissociation of hydrogen gas is 436 kJ/mol.

asked Jan 23 in ThermoChemistry by Melanie86K41 (1.7k 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 SamMph085344 (2.4k points)

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1 answer 66 views

Calculate the bond energy of carbon-hydrogen bond in methane (CH4) given that the enthalpy change of combustion for methane is -890 kJ/mol and the enthalpy change for breaking carbon-hydrogen bonds is 413 kJ/mol.

asked Jan 23 in Chemical reactions by MckenzieWxs (1.6k points)

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Calculate the amount of heat released when 0.5 moles of propane, C3H8, combust completely in oxygen gas, O2, according to the following balanced equation:C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(l), ∆H = -2220 kJ/mol.

asked Jan 23 in ThermoChemistry by MargueriteWa (1.8k points)

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A container initially contains 0.10 mol of NOBr, 0.10 mol of NO, and 0.10 mol of Br2. If the system reaches equilibrium and the concentration of NOBr is found to be 0.075 M at that point, calculate the concentration of NO and Br2 at equilibrium.

asked Jan 22 in Chemical equilibrium by JodieGartrel (1.8k points)

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1 answer 65 views

Calculate the cell potential for the reaction between a silver electrode and a copper electrode, given that the silver electrode is immersed in a 0.1 M AgNO3 solution and the copper electrode is immersed in a 1.0 M CuSO4 solution at 25°C. (Standard electrode potentials of Ag and Cu electrodes are +0.80 V and +0.34 V, respectively. Carry out the calculation in steps and provide the final answer with appropriate units.)

asked Jan 23 in ElectroChemistry by ChristieJzq (1.7k points)

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Calculate the formal charge of the oxygen atom and the chlorine atom in the perchlorate ion, ClO₄⁻. Show your work and explain how you arrived at your answer.

asked Jan 23 in Inorganic Chemistry by AzucenaGrasb (1.6k points)

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1 answer 52 views

Calculate the equilibrium concentrations of reactants and products for the following reaction at a temperature of 25°C and a pressure of 1 atm:2 NO(g) + Br2(g) ⇌ 2 NOBr(g)Given the initial concentrations are [NO] = 0.20 M, [Br2] = 0.35 M, and [NOBr] = 0.015 M. The equilibrium constant (Kc) for the reaction is 4.8 x 10^2 at 25°C.

asked Jan 23 in Chemical equilibrium by ThaliaSheil (2.0k points)

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1 answer 53 views

Calculate the enthalpy of vaporization for water given the following information: The boiling point of water is 100°C and its specific heat capacity is 4.18 J/g°C. The density of water at its boiling point is 0.958 g/mL and the heat of fusion for water is 40.7 kJ/mol. The molar mass of water is 18.015 g/mol.

asked Jan 23 in ThermoChemistry by KathiFatnown (1.6k points)

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Calculate the entropy change of an ideal monatomic gas at 1 atm and 300 K when it expands isothermally to 5 times its initial volume.

asked Jan 23 in Physical Chemistry by Shawn33B4717 (1.9k points)

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Calculate the entropy change for the following chemical reaction at 25 °C: 2H2(g) + O2(g) → 2H2O(l) Given that the standard molar entropy of H2(g), O2(g), and H2O(l) are 130.68 J/mol·K, 205.03 J/mol·K and 70.01 J/mol·K respectively.

asked Jan 23 in Chemical thermodynamics by CecileBills (2.2k points)

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1 answer 60 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 NicholeBlade (2.1k points)

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1 answer 66 views

Calculate the bond dissociation energy for the C-H bond in methane (CH4) using the following data:- The heat of combustion of methane is -890 kJ/mol.- The enthalpy of formation of CO2 is -393.5 kJ/mol.- The enthalpy of formation of H2O is -285.8 kJ/mol.- The heat of combustion of hydrogen is -286 kJ/mol.

asked Jan 23 in ThermoChemistry by NadiaN491716 (2.1k points)

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1 answer 52 views

Calculate the entropy change (∆S) when a container of volume 1.0 L is filled with 1.0 mol of ideal gas at a temperature of 300 K and a pressure of 1.0 atm, and then the gas is allowed to expand irreversibly to fill a volume of 2.0 L against a constant external pressure of 0.5 atm at the same temperature.

asked Jan 23 in Physical Chemistry by ChloeBodnar (2.0k points)

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Calculate the enthalpy change for the oxidation of 10 moles of carbon monoxide (CO) to carbon dioxide (CO2) using the enthalpy of formation values given below:∆Hf CO = -110.5 kJ/mol ∆Hf CO2 = -393.5 kJ/mol

asked Jan 23 in ThermoChemistry by JadaMeece33 (1.6k points)

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Calculate the enthalpy change of oxidation for the combustion of 1 mole of ethane gas (C₂H₆) in oxygen gas (O₂) to form carbon dioxide gas (CO₂) and water vapor (H₂O), given the following enthalpies of formation: ΔHf(C₂H₆) = -84.7 kJ/mol, ΔHf(CO₂) = -393.5 kJ/mol, ΔHf(H₂O) = -241.8 kJ/mol.

asked Jan 23 in ThermoChemistry by Anglea937174 (1.9k points)

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Calculate the enthalpy change and the entropy change of the reaction where 2 moles of HCl(g) reacts with 1 mole of CaO(s) to produce 1 mole of CaCl2(s) and 1 mole of H2O(l). Given the bond dissociation enthalpies (in kJ/mol) of H-H is 436, Cl-Cl is 243, H-Cl is 431, and O-H is 463. The standard entropies (in J/mol K) of HCl(g) is 186.9, CaO(s) is 38.2, CaCl2(s) is 223.0, and H2O(l) is 69.9.

asked Jan 23 in Inorganic Chemistry by AmandaRku513 (1.8k points)

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