Recent questions in ThermoChemistry

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Calculate the enthalpy change for the oxidation of methane (CH4) to carbon dioxide (CO2) at constant pressure using the following reactions: * C(s) + O2(g) --> CO2(g) ΔH = -393.5 kJ/mol* 2H2(g) + O2(g) --> 2H2O(l) ΔH = -571.6 kJ/molThe enthalpy of formation of CH4(g) is -74.8 kJ/mol.

asked Jan 23 in ThermoChemistry by StephanyHerr (350 points)

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Calculate the enthalpy change for the oxidation of 5 moles of hydrogen gas using the standard enthalpies of formation of water and hydrogen gas.

asked Jan 23 in ThermoChemistry by AlvaroZyl417 (470 points)

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Calculate the enthalpy change for the oxidation of 25 grams of iron (Fe) to form iron(III) oxide (Fe2O3) using the balanced chemical equation and the given enthalpy of formation values for Fe(s) and Fe2O3(s).

asked Jan 23 in ThermoChemistry by BerryPalmer6 (310 points)

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Calculate the enthalpy change for the oxidation of 2 moles of iron, given the standard enthalpy of formation for FeO is -272.2 kJ/mol and that of Fe2O3 is -824 kJ/mol.

asked Jan 23 in ThermoChemistry by GDZWillis962 (390 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 AbrahamMaruf (550 points)

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Calculate the enthalpy change for the oxidation of 1 mole of methane gas to form carbon dioxide and water vapor, given the following balanced chemical equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)(enthalpy of formation: ΔHf(CH4)=-74.81 kJ/mol, ΔHf(CO2)=-393.51 kJ/mol, ΔHf(H2O)= -241.83 kJ/mol)

asked Jan 23 in ThermoChemistry by TuyetSticht2 (310 points)

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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 YasminKoerst (390 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 RetaRicher65 (450 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 QOBGertrude3 (350 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 SamaraQ8653 (410 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 LesleyStyers (670 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 Cortney96786 (330 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 SharylHastin (310 points)

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1 answer 50 views

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 Shirley80008 (530 points)

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1 answer 57 views

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 KarriWalpole (810 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 LelandCreswi (350 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 MarcelO27806 (350 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 DanialOsburn (410 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 ArcherPcc770 (550 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 DanielleCand (330 points)

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