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Calculate the enthalpy change for the polymerization of ethylene to polyethylene if it is known that the heat of combustion of ethylene is -1411 kJ/mol and the enthalpy of formation of polyethylene is -248 kJ/mol. Assume that the reaction occurs at constant pressure and temperature of 25°C.

asked Jan 23 in ThermoChemistry by IHSKellye65 (330 points)

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Calculate the enthalpy change for the polymerization of 2-methyl-1,3-butadiene (MBC) if 1 mole of MBC is polymerized in a perfectly insulated container at a constant temperature of 25°C. The reaction equation for the polymerization of MBC is given as:nC5H8 (MBC) → (C5H8) (Polymer)Given the bond dissociation energies (in kJ/mol) for the following bonds:C-C bond = 348C-H bond = 413Assume that the enthalpy change of vaporization of MBC is negligible.

asked Jan 23 in ThermoChemistry by StephaniaU34 (250 points)

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Calculate the enthalpy change for the oxidation of methane gas (CH4) to carbon dioxide (CO2) and water (H2O) using the following balanced chemical equation:CH4 (g) + 2O2 (g) -> CO2 (g) + 2H2O (l)The standard enthalpy of formation of methane, carbon dioxide, and water are -74.81 kJ/mol, -393.5 kJ/mol, and -285.83 kJ/mol respectively.

asked Jan 23 in ThermoChemistry by DaisyCarolan (430 points)

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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 KiaLovegrove (250 points)

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1 answer 56 views

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 GudrunCollea (210 points)

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1 answer 54 views

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 KelleBraden2 (310 points)

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1 answer 74 views

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 ByronVanwink (230 points)

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1 answer 57 views

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 HelenStidham (270 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 EbonyVanderb (390 points)

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1 answer 52 views

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 JanineGeach (190 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 HaleyXtk6504 (530 points)

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1 answer 52 views

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 ArleenNielso (730 points)

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1 answer 56 views

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 DaltonMcDone (270 points)

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1 answer 60 views

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 Raquel762307 (350 points)

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1 answer 59 views

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 QFFNeil45469 (410 points)

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1 answer 50 views

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 ShannanPatti (250 points)

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1 answer 73 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 DennisDaly04 (190 points)

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1 answer 58 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 LillieIst935 (310 points)

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1 answer 67 views

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 SerenaColema (290 points)

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1 answer 53 views

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 ThaliaFihell (230 points)

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