Recent questions in Chemistry

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Calculate the bond dissociation energy of a molecule of hydrogen (H₂) given that the bond length is 74 pm and the energy required to break the bond is 436 kJ/mol.

asked Jan 23 in Chemical bonding by ChanteCamari (610 points)

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1 answer 50 views

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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Calculate the bond dissociation energy for the H-H bond, given that the average H-H bond energy is 436 kJ/mol. Show all the steps in your calculation.

asked Jan 23 in Chemical bonding by JacquieElias (390 points)

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1 answer 50 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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1 answer 54 views

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 53 views

Calculate the bond dissociation energy (in kJ/mol) of the H-Cl bond in hydrogen chloride molecule, given that the bond length is 127 pm and the vibrational frequency is 8.8 x 10^13 Hz.

asked Jan 23 in Chemical bonding by HattieSteven (310 points)

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1 answer 61 views

Calculate the bond dissociation energy (in kJ/mol) of the H-Cl bond in HCl using the following data: the standard enthalpy of formation of HCl is -92.31 kJ/mol, the bond energy of H-H is 436 kJ/mol, and the bond energy of Cl-Cl is 240 kJ/mol.

asked Jan 23 in Chemical bonding by MayraMcGuire (570 points)

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1 answer 41 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 52 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 36 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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1 answer 53 views

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 42 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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1 answer 49 views

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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1 answer 49 views

Calculate the bond dissociation energy (in kJ/mol) for the breaking of the carbon-hydrogen (C-H) bond in methane (CH4), given the following information: CH4 (g) → CH3 (g) + H (g) ∆H = 432 kJ/mol Note: The bond dissociation energy is the amount of energy required to break a bond between two atoms in a molecule, resulting in two separate atoms.

asked Jan 23 in ThermoChemistry by JerrellGoodi (370 points)

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1 answer 55 views

Calculate the bond angles and molecular geometry of the methane (CH4) molecule by using quantum chemistry principles.

asked Jan 23 in Quantum Chemistry by GraigHardiso (730 points)

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1 answer 51 views

Calculate the boiling point of sodium chloride using Raoult's law assuming that the vapor pressure of pure water at the given temperature is 25 Torr and the mole fraction of NaCl in the solution is 0.2.

asked Jan 23 in Inorganic Chemistry by StepaniePetc (410 points)

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1 answer 56 views

Calculate the boiling point of potassium chloride (KCl) using the Clausius-Clapeyron equation, given that its enthalpy of vaporization is 40.0 kJ/mol and its standard boiling point is 1500 K. What would be the expected boiling point of KCl at an atmospheric pressure of 1.0 atm (760 mmHg)?

asked Jan 23 in Inorganic Chemistry by KraigPxi0162 (470 points)

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1 answer 60 views

Calculate the binding energy of a hydrogen molecule and a helium atom in their ground state using Quantum chemical calculations of non-covalent interactions. What is the strength of the interaction between these two species?

asked Jan 23 in Computational Chemistry by AnnmarieMcCl (530 points)

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