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Calculate the enthalpy change for the isomerization reaction of butene-1 to cis-2-butene. Given that the standard enthalpy of formation for butene-1 is -19.8 kJ/mol and for cis-2-butene is -20.4 kJ/mol, and the standard enthalpy of combustion for butene-1 is -2876 kJ/mol.

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

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Calculate the enthalpy change for the isomerization of pentene-1 to pentene-2 if 2.5 g of pentene-1 is isomerized using a catalyst and the temperature increases from 25° C to 35° C. The heat capacity of the calorimeter is 15.6 J/deg and the density of the solution is 0.98 g/mL. Assume the heat capacity of the solution is equal to the heat capacity of water (4.18 J/g deg).

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

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Calculate the enthalpy change for the isomerization of n-butane to iso-butane if the standard enthalpy of formation for n-butane is -125.7 kJ/mol and that for iso-butane is -147.4 kJ/mol. The isomerization reaction occurs at a constant pressure of 1 atm and at a temperature of 298 K.

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

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Calculate the enthalpy change for the isomerization of butene-1 to butene-2 given that the standard enthalpy of formation of butene-1 is -25.3 kJ/mol and the standard enthalpy of formation of butene-2 is -23.6 kJ/mol. The reaction is carried out at a constant pressure of 1 atm and a temperature of 298 K.

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

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Calculate the enthalpy change for the isomerization of butene-1 to butene-2 given that the heat of combustion of butene-1 and butene-2 are -2874 kJ/mol and -2854 kJ/mol respectively. Assume all reactants and products are in the gaseous state and that the reaction is carried out at constant pressure.

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

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Calculate the enthalpy change for the isomerization of butene to isobutene given that the enthalpy of combustion for butene is -2671.2 kJ/mol and the enthalpy of combustion for isobutene is -2678.6 kJ/mol. Assume that the molar enthalpy of formation of CO2 and H2O are -393.5 kJ/mol and -241.8 kJ/mol, respectively.

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

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Calculate the enthalpy change for the isomerization of But-1-ene to But-2-ene using the given bond enthalpies: C-C single bond (347 kJ/mol), C-H bond (413 kJ/mol), C=C double bond (611 kJ/mol), and the enthalpy of formation of But-1-ene (-4.8 kcal/mol) and But-2-ene (-0.9 kcal/mol).

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

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Calculate the enthalpy change for the ionization of sodium chloride given that the enthalpy of formation of NaCl is -411 kJ/mol, and the ionization energy of Na and Cl are 496 kJ/mol and 349 kJ/mol respectively.

asked Jan 23 in ThermoChemistry by Juliana93U49 (2.3k points)

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Calculate the enthalpy change for the ionization of magnesium, given that it requires 738 kJ/mol to remove an electron from a gaseous magnesium atom, and that the ionization energy for a second electron is 1450 kJ/mol.

asked Jan 23 in ThermoChemistry by XLNDorris808 (1.7k points)

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Calculate the enthalpy change for the ionization of magnesium using the following information: - The first ionization energy of magnesium is 738 kJ/mol. - The second ionization energy of magnesium is 1450 kJ/mol.

asked Jan 23 in ThermoChemistry by JewelFison69 (1.8k points)

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Calculate the enthalpy change for the ionization of hydrogen atom if the ionization energy required is 1312 kJ/mol.

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

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Calculate the enthalpy change for the ionization of 1 mol of hydrogen chloride gas at standard conditions, given that the enthalpy change for the reaction HCl(g) → H+(aq) + Cl-(aq) is -74.8 kJ/mol.

asked Jan 23 in ThermoChemistry by GrettaKavel6 (2.2k points)

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Calculate the enthalpy change for the hydrolysis of sucrose given the following information: Sucrose (C12H22O11) reacts with water to form glucose (C6H12O6) and fructose (C6H12O6). Delta H for the reaction is -190 kJ/mol. The enthalpy of formation for sucrose is -2227 kJ/mol, the enthalpy of formation for glucose is -1274 kJ/mol, and the enthalpy of formation for fructose is -1266 kJ/mol.

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

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Calculate the enthalpy change for the hydrolysis of sucrose given that 10.0 g of sucrose was completely hydrolyzed in excess water. The reaction takes place at 25°C and 1 atm pressure. The following reaction is involved: C12H22O11(s) + H2O(l) → 12C(s) + 11H2O(l) The enthalpy of formation of C12H22O11(s) is -2226.8 kJ/mol and the enthalpy of formation of H2O(l) is -285.8 kJ/mol.

asked Jan 23 in ThermoChemistry by ShaunteYun90 (1.4k points)

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Calculate the enthalpy change for the hydrolysis of 50 grams of sucrose (C12H22O11) when dissolved in 500 ml of water at 25°C. The molar mass of sucrose is 342.3 g/mol and the enthalpy change per mole of sucrose is -564.8 kJ/mol.

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

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Calculate the enthalpy change for the hydrolysis of 5.5 grams of sucrose (C12H22O11) using the standard enthalpy of formation values of the products and reactants. Assume the reaction takes place at constant pressure and temperature of 25°C.

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

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Calculate the enthalpy change for the hydrolysis of 5 moles of methyl acetate using the given bond enthalpies: C-O (360 kJ/mol), C=O (740 kJ/mol), O-H (460 kJ/mol), and C-H (410 kJ/mol).

asked Jan 23 in ThermoChemistry by ScottyWild8 (1.4k points)

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Calculate the enthalpy change for the hydrolysis of 2 moles of sucrose (C12H22O11) into glucose (C6H12O6) and fructose (C6H12O6), given the enthalpy change of hydrolysis for glucose and fructose are -2801 and -2802 kJ/mol respectively.

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

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Calculate the enthalpy change for the hydrolysis of 2 moles of sucrose (C12H22O11) into glucose (C6H12O6) and fructose (C6H12O6) given the following information:- Enthalpy of formation of glucose = -1273 kJ/mol- Enthalpy of formation of fructose = -1260 kJ/mol- Enthalpy of formation of sucrose = -2226 kJ/mol

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

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Calculate the enthalpy change for the hydrolysis of 2 moles of sucrose (C12H22O11) in aqueous solution given that the heat capacity of the solution is 4.18 J/g.K, the initial and final temperatures of the solution are 22.0°C and 28.0°C respectively. The molar mass of sucrose is 342.3 g/mol.

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

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