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Calculate the enthalpy change of polymerization for the formation of polystyrene from its monomer, styrene, given the following data:- ΔH°f (Styrene) = -25.68 kJ/mol- Bond enthalpies: C-C = 347 kJ/mol; C=C = 611 kJ/mol; C-H = 413 kJ/mol

asked Jan 23 in ThermoChemistry by KirstenLipsc (1.8k 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 of mixing 50 mL of 1 M HCl with 50 mL of 1 M NaOH at 25°C. It is known that the standard enthalpies of formation of HCl and NaOH are -92.3 kJ/mol and -469.2 kJ/mol, respectively. Assume that the heat capacity of the mixture is 4.18 J/g°C and the density of the solution is 1 g/mL.

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

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Calculate the enthalpy change of isomerization for the reaction of cyclopropane to propene given that the standard enthalpy of formation of cyclopropane is -119.1 kJ/mol and the standard enthalpy of formation of propene is -103.8 kJ/mol. Assume that the enthalpy change of vaporization for both compounds is negligible.

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

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Calculate the enthalpy change of isomerization for the conversion of n-butane to isobutane if the heat of combustion of n-butane is -2657.5 kJ/mol and the heat of combustion of isobutane is -2878.8 kJ/mol.

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

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Calculate the enthalpy change of isomerization for the conversion of cis-but-2-ene to trans-but-2-ene, given the standard enthalpy of formation for both isomers. Asssume all other conditions remain constant.

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

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Calculate the enthalpy change of isomerization for the conversion of cis-but-2-ene to trans-but-2-ene if the enthalpy of formation of cis-but-2-ene is -24.7 kJ/mol and the enthalpy of formation of trans-but-2-ene is -28.6 kJ/mol. The heat of combustion of but-2-ene is -2723 kJ/mol.

asked Jan 23 in ThermoChemistry by EttaKee54894 (2.1k points)

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Calculate the enthalpy change of isomerization for the conversion of cis-2-butene to trans-2-butene, given that the heat of combustion of cis-2-butene is -3283.1 kJ/mol and the heat of combustion of trans-2-butene is -3336.8 kJ/mol. Assume that the heat of combustion is representative of the enthalpy of formation.

asked Jan 23 in ThermoChemistry by NFDRoman4328 (1.8k points)

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Calculate the enthalpy change of ionization for magnesium given the following data: Mg(g) → Mg+(g) + e- ΔH1 = +738 kJ/mol Mg+(g) → Mg2+(g) + e- ΔH2 = +1451 kJ/mol

asked Jan 23 in ThermoChemistry by Georgianna69 (2.2k points)

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1 answer 62 views

Calculate the enthalpy change of ionization for hydrogen gas when one mole of H2 gas is ionized to form two moles of H+ ions in the gas phase, given that the enthalpy change of ionization for H(g) is +1312 kJ/mol.

asked Jan 23 in ThermoChemistry by OnaSchnell25 (1.8k points)

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Calculate the enthalpy change of dissolving 5.00 g of NaOH in 100.0 g of water. The temperature of the resulting solution increases from 25.00°C to 31.50°C. The specific heat capacity of the resulting solution is 4.18 J/g°C.

asked Jan 23 in ThermoChemistry by EloisaPtm353 (1.9k points)

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Calculate the enthalpy change of dissolving 10.0 g of sodium hydroxide (NaOH) in 200.0 mL of water at 25°C. Given: the enthalpy of dissolution of NaOH is -44.5 kJ/mol.

asked Jan 23 in ThermoChemistry by JuliannSfd66 (2.0k points)

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Calculate the enthalpy change of dissolving 10 grams of NaCl in 100 mL of water, assuming the resultant solution has a density of 1.0 g/mL and assuming that the heat evolved is absorbed by the water. Given: the enthalpy of hydration of NaCl is -787 kJ/mol.

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

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Calculate the enthalpy change of dissolution when 5 grams of sodium chloride (NaCl) dissolves in 100 mL of water at 25°C. The molar enthalpy of dissolution of sodium chloride is -3.9 kJ/mol.

asked Jan 23 in ThermoChemistry by Milagros70T7 (1.5k points)

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Calculate the enthalpy change of dissolution (in kJ/mol) for NaCl in water, given that 1.00 g of NaCl is dissolved in 50.0 mL of water at 25°C. The density of water is 0.997 g/mL and the specific heat capacity of the solution is assumed to be the same as that of water (4.184 J/gK). The molar mass of NaCl is 58.44 g/mol.

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

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1 answer 65 views

Calculate the enthalpy change of desorption of water from a graphite surface if the initial pressure of water is 10 torr and the final pressure is 1 torr at a constant temperature of 300 K. The surface area of the graphite is 50 cm² and the heat of adsorption of water on the surface is -40 kJ/mol.

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

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Calculate the enthalpy change of desorption for a solid substance using the given data: The mass of the substance is 2.5 g, and the temperature change during desorption is 25 °C. The heat capacity of the substance is 1.5 J/g·°C. The molar mass of the substance is 150 g/mol. Assume that the desorption process takes place at constant pressure.

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

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1 answer 52 views

Calculate the enthalpy change of combustion for the reaction of methane (CH4) when 1.25 moles of methane is completely burnt in excess oxygen gas at standard conditions, given that the enthalpy change of combustion for methane is -890.3 kJ/mol.

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

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Calculate the enthalpy change of combustion for ethane (C2H6) when 5.00 g of ethane is completely burned in excess oxygen gas, given that the standard enthalpy of combustion of ethane is -1560 kJ/mol.

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

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Calculate the enthalpy change of combustion for ethane (C2H6) given that the standard enthalpy of formation for ethane is -84.68 kJ/mol, the standard enthalpy of formation for CO2 is -393.5 kJ/mol, and the standard enthalpy of formation for H2O is -241.8 kJ/mol.

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

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