Recent questions in ThermoChemistry

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Calculate the enthalpy change (in kJ/mol) for the ionization of magnesium, given that the first ionization energy of magnesium is 738 kJ/mol and the second ionization energy is 1450 kJ/mol.

asked Jan 23 in ThermoChemistry by HNWAlyssa098 (450 points)

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Calculate the enthalpy change (in kJ/mol) for dissolving 10 grams of NaOH in 100 mL of water at 25°C, given that the molar heat of solution for NaOH is -444.6 kJ/mol.

asked Jan 23 in ThermoChemistry by CortezDale67 (550 points)

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Calculate the enthalpy change (∆H) for the combustion reaction of methane gas (CH4) using Hess’s Law, when the enthalpy changes for the following reactions are given: Reaction 1: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l); ∆H = -891 kJ/mol Reaction 2: C (s) + O2 (g) → CO2 (g); ∆H = -393.5 kJ/mol Reaction 3: 2H2 (g) + O2 (g) → 2H2O (l); ∆H = -484 kJ/mol

asked Jan 23 in ThermoChemistry by Corazon66R68 (510 points)

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Calculate the bond dissociation energy required to break a carbon-carbon single bond in methane (CH4).

asked Jan 23 in ThermoChemistry by DerekAmess50 (490 points)

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Calculate the bond dissociation energy of the O-H bond in a water molecule if the enthalpy change for the following reaction is -285.8 kJ/mol:2H2(g) + O2(g) -> 2H2O(l)

asked Jan 23 in ThermoChemistry by MaribelWesto (650 points)

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Calculate the bond dissociation energy of the O-H bond in a water molecule (H2O) given the enthalpy change for the reaction:H2O (g) → H2 (g) + 1/2 O2 (g)ΔH = +483.6 kJ/mol(Note: the bond dissociation energy represents the energy required to break a bond into its constituent atoms.)

asked Jan 23 in ThermoChemistry by Rex516068171 (650 points)

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Calculate the bond dissociation energy of the nitrogen-nitrogen (N-N) bond in N2O4 given that the enthalpy change for the reaction 2N2O4(g) --> 4NO2(g) is -109.7 kJ/mol.

asked Jan 23 in ThermoChemistry by HelenaGodoy5 (670 points)

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Calculate the bond dissociation energy of the H-H bond given the following information: The enthalpy change for the reaction 2H2(g) → 4H(g) is +436 kJ/mol, and the average bond dissociation energy for a H-H bond is 436 kJ/mol.

asked Jan 23 in ThermoChemistry by AprilCutlack (610 points)

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1 answer 34 views

Calculate the bond dissociation energy of the carbon-hydrogen bond in methane (CH4), given that the reaction CH4(g) → CH3(g) + H(g) has a ΔH° of 435 kJ/mol.

asked Jan 23 in ThermoChemistry by JanetteBrewi (450 points)

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Calculate the bond dissociation energy for the single bond in methane (CH4) given the following data: ΔHºf(CH4) = -74.8 kJ/molΔHºrxn = -890.4 kJ/mol Note: The bond dissociation energy is the amount of energy needed to break a bond between two atoms in a molecule, while keeping the other bonds intact.

asked Jan 23 in ThermoChemistry by FedericoClow (530 points)

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1 answer 48 views

Calculate the bond dissociation energy for the H-H bond in a diatomic hydrogen molecule, given that the enthalpy change for the reaction H2(g) → 2 H(g) is 436 kJ/mol.

asked Jan 23 in ThermoChemistry by TeresaCulpep (470 points)

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1 answer 51 views

Calculate the bond dissociation energy for the Cl-Cl bond in Cl2(g) given that the standard enthalpy change for the reaction Cl2(g) → 2 Cl(g) is +121 kJ/mol and the bond dissociation energy for the Cl-Cl bond in Cl2(g) is known to be 242 kJ/mol.

asked Jan 23 in ThermoChemistry by JaiMarston48 (450 points)

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Calculate the bond dissociation energy for the C-H bond in methane (CH4) using the following data:- The heat of combustion of methane is -890 kJ/mol.- The enthalpy of formation of CO2 is -393.5 kJ/mol.- The enthalpy of formation of H2O is -285.8 kJ/mol.- The heat of combustion of hydrogen is -286 kJ/mol.

asked Jan 23 in ThermoChemistry by EugeniaDozie (890 points)

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1 answer 53 views

Calculate the bond dissociation energy (in kJ/mol) required to break the carbon-hydrogen bond in methane using the given bond dissociation energies: C-H = 413 kJ/mol, C-C = 347 kJ/mol, C=C = 602 kJ/mol, H-H = 436 kJ/mol.

asked Jan 23 in ThermoChemistry by AlanaEarly83 (490 points)

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1 answer 38 views

Calculate the bond dissociation energy (in kJ/mol) of the C-H bond in methane (CH4) using the following given data:- Enthalpy of formation of methane (CH4) = -74.8 kJ/mol- Enthalpy of combustion of methane (CH4) = -890.4 kJ/mol- Enthalpy change for the breaking of all four C-H bonds in methane = 1665 kJ/mol.

asked Jan 23 in ThermoChemistry by MaybelleKram (510 points)

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1 answer 50 views

Calculate the bond dissociation energy (in kJ/mol) of the C-H bond in methane (CH4) using the following data: - The enthalpy change for the combustion of one mole of methane gas is -890.3 kJ/mol.- The energy required to break one mole of H-H bonds is 433.4 kJ/mol.- The energy required to break one mole of C=O bonds is 799.5 kJ/mol.- The energy required to break one mole of O-H bonds is 463.0 kJ/mol.

asked Jan 23 in ThermoChemistry by JeremyGorsuc (430 points)

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1 answer 34 views

Calculate the bond dissociation energy (in kJ/mol) of the C-H bond in methane (CH4) using experimental data.

asked Jan 23 in ThermoChemistry by SaundraKauff (390 points)

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Calculate the bond dissociation energy (in kJ/mol) of chlorine gas (Cl2) if it requires 243 kJ of energy to break a single Cl-Cl bond in the gas phase.

asked Jan 23 in ThermoChemistry by NadineToothm (230 points)

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1 answer 40 views

Calculate the bond dissociation energy (in kJ/mol) for the O-H bond in water (H2O) given that the enthalpy change for the reaction H2O (g) → H (g) + OH(g) is +495 kJ/mol and the enthalpy change for the reaction H2(g) + 1/2O2(g) → H2O(g) is -241.8 kJ/mol.

asked Jan 23 in ThermoChemistry by Holly81G1945 (610 points)

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Calculate the bond dissociation energy (in kJ/mol) for the carbon-hydrogen bond in methane (CH4) using the following information: - The enthalpy change for the reaction CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) is -890.3 kJ/mol. - The enthalpy change for the reaction 2H2(g) + O2(g) → 2H2O(g) is -484.2 kJ/mol.

asked Jan 23 in ThermoChemistry by DuaneGilbert (290 points)

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