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Calculate the standard enthalpy of formation of methane gas (CH4) given the standard enthalpies of formation for carbon dioxide (CO2) (-393.5 kJ/mol) and water vapor (H2O) (-241.8 kJ/mol).

asked Feb 3 in ThermoChemistry by LeroyBothwel (1.9k points)

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Calculate the standard enthalpy of formation of methane gas (CH4) given the following data:- ∆H°combustion of methane = -890.36 kJ/mol - ∆H°formation of H2O (l) = -285.8 kJ/mol - ∆H°formation of CO2 (g) = -393.5 kJ/mol

asked Feb 3 in ThermoChemistry by ColumbusU230 (2.4k points)

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Calculate the standard enthalpy of formation of methane (CH4) given the following enthalpy data: C(graphite) + 2H2(g) → CH4(g) ΔH° = -74.8 kJ/mol ΔH°f[C(graphite)] = 0 kJ/molΔH°f[H2(g)] = 0 kJ/mol (Hint: Use Hess's Law and the fact that the standard enthalpy of formation of an element in its most stable state is zero.)

asked Feb 3 in ThermoChemistry by TBHMelaine51 (2.2k points)

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Calculate the standard enthalpy of formation of methane (CH4) given that the standard enthalpies of formation for CO2 and H2O are -393.5 kJ/mol and -285.8 kJ/mol, respectively.

asked Feb 3 in ThermoChemistry by CecileHollin (2.3k points)

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Calculate the standard enthalpy of formation of hydrogen fluoride (HF) given the following reactions and enthalpy change values:2H2(g) + O2(g) → 2H2O(g) ΔH° = -484 kJH2(g) + Cl2(g) → 2HCl(g) ΔH° = -184 kJ1/2 F2(g) + H2(g) → HF(g) ΔH° = -273 kJ.

asked Feb 3 in ThermoChemistry by AundreaWhitf (1.8k points)

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Calculate the standard enthalpy of formation of glucose (C6H12O6) given that the standard enthalpies of combustion for glucose, carbon, and hydrogen are -2803.6 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol, respectively.

asked Feb 3 in ThermoChemistry by MireyaFlaher (1.6k points)

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1 answer 115 views

Calculate the standard enthalpy of formation of ethane (C2H6) given the following bond energies (in kJ/mol):C-C: 347C-H: 413 Note: The equation for the formation of ethane is:C(graphite) + 3H2(g) -> C2H6(g)

asked Feb 3 in ThermoChemistry by MaricelaBevi (1.9k points)

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Calculate the standard enthalpy of formation of carbon dioxide gas (CO2) given the following information: C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ/mol H2(g) + 1/2O2(g) → H2O(l) ΔH = -285.8 kJ/mol 2C(s) + 2H2(g) + 5/2O2(g) → 2CO2(g) + 2H2O(l) ΔH = -890.4 kJ/mol

asked Feb 3 in ThermoChemistry by BonnieSayre (2.1k points)

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Calculate the standard enthalpy of formation of carbon dioxide from its elements under standard conditions given the following information:- The standard enthalpy of combustion of carbon to CO2 is -393.5 kJ/mol- The standard enthalpy of combustion of hydrogen to H2O is -285.8 kJ/mol- The standard enthalpy of formation of water is -241.8 kJ/mol.Note: The standard enthalpy of formation of an element in its standard state is zero.

asked Feb 3 in ThermoChemistry by WilfredoWren (2.1k points)

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Calculate the standard enthalpy of formation of Carbon dioxide (CO2), given the enthalpies of formation of Carbon monoxide (CO) and Oxygen gas (O2) as -110.5 kJ/mol and 0 kJ/mol, respectively.

asked Feb 3 in ThermoChemistry by MichelleHall (2.0k points)

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Calculate the standard enthalpy of formation of carbon dioxide (CO2) using the following information:C(graphite) + O2(g) -> CO2(g), ΔH° = -393.5 kJ/molC(graphite) + 2H2(g) -> CH4(g), ΔH° = -74.8 kJ/mol2H2(g) + O2(g) -> 2H2O(l), ΔH° = -572.0 kJ/mol

asked Feb 3 in ThermoChemistry by AleidaSeifer (1.7k points)

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Calculate the standard enthalpy of formation of carbon dioxide (CO2) using the following data:C(graphite) + O2(g) → CO2(g) ΔH° = -393.5 kJ/mol2H2(g) + O2(g) → 2H2O(l) ΔH° = -572.0 kJ/molHint: Use Hess's law to calculate the standard enthalpy of formation of CO2.

asked Feb 3 in ThermoChemistry by PartheniaBar (2.2k points)

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1 answer 125 views

Calculate the standard enthalpy of formation of C2H6(g) given the following information: C(s) + O2(g) → CO2(g); ΔH° = -393.5 kJ/mol H2(g) + 1/2 O2(g) → H2O(l); ΔH° = -285.8 kJ/mol 2C(s) + 3H2(g) → C2H6(g); ΔH° = ?

asked Feb 3 in ThermoChemistry by LaunaRxf8120 (1.7k points)

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1 answer 159 views

Calculate the standard enthalpy of formation of aluminum oxide from its elements given the following information:2 Al(s) + 3/2 O2(g) → Al2O3(s) ΔH°rxn = - 1675.7 kJ/molStandard enthalpy of formation of Al(s) = 0 kJ/molStandard enthalpy of formation of O2(g) = 0 kJ/mol

asked Feb 3 in ThermoChemistry by EdgardoHinch (2.2k points)

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1 answer 113 views

Calculate the standard enthalpy of formation for magnesium oxide (MgO) given the standard enthalpy of formation for magnesium (Mg) is -601.8 kJ/mol and the standard enthalpy of formation for oxygen (O₂) is 0 kJ/mol.

asked Feb 3 in ThermoChemistry by FrancisGepp5 (1.8k points)

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Calculate the standard enthalpy of formation (ΔH°f) of methane (CH4) given the following data: 2H2(g) + O2(g) → 2H2O(l) ΔH°rxn = -572 kJ/mol C(graphite) + O2(g) → CO2(g) ΔH°rxn = -394 kJ/mol Note: The enthalpy of formation of an element in its standard state is zero (0).

asked Feb 3 in ThermoChemistry by AstridMusser (1.9k points)

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Calculate the standard enthalpy of formation (ΔH°f) of carbon dioxide (CO2) at 25°C given the following data:CO(g) + 1/2 O2(g) → CO2(g) ΔH° = -283.3 kJ/molC(s) + O2(g) → CO2(g) ΔH° = -393.5 kJ/molΔH°f (C(s)) = 0 kJ/molΔH°f (O2(g)) = 0 kJ/mol

asked Feb 3 in ThermoChemistry by EmileR968610 (2.0k points)

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1 answer 119 views

Calculate the standard enthalpy of formation (∆Hf) of water (H2O) given the following information: 2H2(g) + O2(g) → 2H2O(l); ∆H = -572 kJ/mol and the standard enthalpy of formation of O2 is 0 kJ/mol.

asked Feb 3 in ThermoChemistry by CatherineMcc (2.5k points)

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1 answer 83 views

Calculate the standard enthalpy change of the oxidation of hydrogen gas (H2) to form water (H2O) at 298 K, given that the standard enthalpy of formation of water is -285.8 kJ/mol and the bond dissociation enthalpy of the H-H bond is 436 kJ/mol.

asked Feb 3 in ThermoChemistry by HenryBorella (2.2k points)

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1 answer 156 views

Calculate the standard enthalpy change of the following reduction reaction if the standard enthalpy of formation of FeO is -272.0 kJ/mol and that of Fe is 0 kJ/mol.FeO(s) + H2(g) → Fe(s) + H2O(l)

asked Feb 3 in ThermoChemistry by Lourdes26529 (2.1k points)

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