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Calculate the enthalpy of ionization of magnesium using the following data: the first ionization energy of Mg is 738 kJ/mol and the lattice energy of MgCl₂ is -2495 kJ/mol.

asked Jan 23 in ThermoChemistry by Marlene31P52 (2.5k points)

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Calculate the enthalpy of ionization of magnesium if 50 mL of 0.1 M HCl solution is added to 1 g of magnesium powder at 25°C, and the change in temperature is -10°C. The specific heat capacity of the solution is 4.18 J•g-1•K-1.

asked Jan 23 in ThermoChemistry by MollieBalke (2.3k points)

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Calculate the enthalpy of ionization of magnesium if 4.8 g of magnesium reacts completely with hydrochloric acid to form 224 mL of hydrogen gas at standard temperature and pressure (STP). The heat released during the reaction is -412 kJ/mol.

asked Jan 23 in ThermoChemistry by AudreaV25265 (2.0k points)

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Calculate the enthalpy of ionization of hydrogen gas (H₂) given that it requires 1312 kJ/mol to ionize a single hydrogen atom (H) in the gas phase.

asked Jan 23 in ThermoChemistry by DanaPittmann (1.5k 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 ionization for the reaction Mg(g) → Mg⁺(g) + e⁻ given that the ionization potential of Mg is 735 kJ/mol and the electron affinity of Mg⁺ is -195 kJ/mol.

asked Jan 23 in ThermoChemistry by PenneyMaxey5 (2.0k points)

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Calculate the enthalpy of ionization for sodium ion (Na+) given that the first ionization energy of sodium (Na) is 495.8 kJ/mol and the second ionization energy is 4562 kJ/mol.

asked Jan 23 in ThermoChemistry by MaynardErb58 (2.0k points)

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Calculate the enthalpy of formation of water (H2O) given the enthalpies of formation of hydrogen gas (H2) and oxygen gas (O2) are -286 kJ/mol and 0 kJ/mol, respectively.

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

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Calculate the enthalpy of formation of sodium chloride from its constituent elements, given the following thermochemical equations:2Na (s) + 1/2 O2 (g) -> Na2O (s) ΔH° = -414.1 kJ/mol Na2O (s) + 1/2 Cl2 (g) -> NaCl (s) ΔH° = -411.2 kJ/mol

asked Jan 23 in ThermoChemistry by DevonHamlett (2.3k points)

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Calculate the enthalpy of formation of So₃(g) using the given thermochemical equations:2SO₂(g) + O₂(g) → 2SO₃(g) ∆H = -197 kJ/mol2SO₂(g) + 2O₂(g) → 2SO₃(g) ∆H = -792 kJ/mol

asked Jan 23 in ThermoChemistry by BradCoz53277 (1.9k points)

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Calculate the enthalpy of formation of NaCl(s) using the following information:1. The enthalpy change of formation of Na(g) is +108.5 kJ/mol.2. The enthalpy change of formation of Cl2(g) is 0 kJ/mol.3. The enthalpy change of vaporization of Na is +97.42 kJ/mol.4. The enthalpy change of dissociation of Cl2 is +242.76 kJ/mol.

asked Jan 23 in ThermoChemistry by MarcellaR325 (2.2k points)

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Calculate the enthalpy of formation of carbon dioxide given the following data:C(s) + O2(g) → CO2(g) ΔH° = -393.5 kJ/molC(s) + 2H2(g) → CH4(g) ΔH° = -74.8 kJ/mol2H2(g) + O2(g) → 2H2O(l) ΔH° = -571.6 kJ/mol

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

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Calculate the enthalpy of formation for glucose (C6H12O6) at standard conditions, given the following enthalpies of formation for its constituent elements: C(graphite) = 0 kJ/mol H2(g) = 0 kJ/mol O2(g) = 0 kJ/mol Hint: Use Hess's Law and standard enthalpies of formation to solve the problem.

asked Jan 23 in ThermoChemistry by EdgardoHinch (2.2k points)

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Calculate the enthalpy of desorption of hydrogen gas (H2) from a platinum surface, given that the temperature of the surface is 298 K and the pressure of H2 gas above the surface is 1 atm. The adsorption enthalpy of H2 on Pt is -43300 J/mol. (Assume ideal gas behavior for H2.)

asked Jan 23 in ThermoChemistry by TahliaEvatt8 (2.2k points)

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1 answer 64 views

Calculate the enthalpy of desorption of CO2 from sodium hydroxide (NaOH) pellets given the following information: - The heat of absorption of CO2 by NaOH pellets is -20.9 kJ/mol.- The standard enthalpy of formation of Na2CO3 is -1130 kJ/mol.- The standard enthalpy of formation of water is -286 kJ/mol.- The standard enthalpy of formation of NaOH is -425 kJ/mol. Assuming that the desorption process is the reverse of the absorption process, determine the enthalpy change for the reaction: Na2CO3(s) + H2O(l) → 2NaOH(s) + CO2(g).

asked Jan 23 in ThermoChemistry by HenryBorella (2.2k points)

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1 answer 66 views

Calculate the enthalpy of desorption of carbon dioxide (CO2) from a surface if the surface coverage is 0.025 mol/m² and the temperature is 298 K. The enthalpy of adsorption for CO2 on the surface is -35.8 kJ/mol. The equilibrium constant (K) for the reaction is 2.99 x 10⁶ at 298 K.

asked Jan 23 in ThermoChemistry by VerleneSchut (1.7k points)

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Calculate the enthalpy of desorption for water vapor adsorbed on activated carbon, given that the heat of adsorption is -50 kJ/mol and the boiling point of water is 100°C.

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

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Calculate the enthalpy of desorption for water molecules from the surface of a silica gel at a temperature of 25°C using the following information:- The vapor pressure of water at 25°C is 3.17 kPa.- The surface area of the silica gel is 25 cm².- The mass of the silica gel used in the experiment is 2.5 g.

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

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Calculate the enthalpy of desorption for the process of magnesium oxide (MgO) surface drying at a temperature of 500 K, given that the equilibrium pressure of water vapor above the dried MgO is 0.056 atm and the enthalpy of adsorption of water on MgO is -44.48 kJ/mol.

asked Jan 23 in ThermoChemistry by KarolinBalse (1.5k points)

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Calculate the enthalpy of combustion of methane if 2.56 g of methane was burnt completely in a bomb calorimeter containing excess oxygen, causing a temperature rise of 4.58 °C in the calorimeter, which has a heat capacity of 1.26 kJ/°C. The balanced chemical equation for the combustion of methane is as follows: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) + energy.

asked Jan 23 in ThermoChemistry by MaxwellDuff3 (1.9k points)

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