Recent questions in Chemistry

0 votes

1 answer 53 views

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 ElaneGuzman (290 points)

0 votes

1 answer 9 views

Calculate the bond dissociation energy of the CO molecule, given that the bond length is 1.128 Å and the electron affinity of carbon and oxygen are -154 kJ/mol and -141 kJ/mol, respectively.

asked Jan 23 in Chemical bonding by JonahFairban (270 points)

0 votes

1 answer 54 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 GaleGeils14 (270 points)

0 votes

1 answer 59 views

Calculate the bond dissociation energy of the carbon-hydrogen bond in methane (CH4) given that the bond enthalpy of C-H bond is 413 kJ/mol.

asked Jan 23 in Chemical bonding by StepaniePetc (430 points)

0 votes

1 answer 66 views

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 LatoyaVela16 (290 points)

0 votes

1 answer 59 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 JulietProvos (810 points)

0 votes

1 answer 50 views

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 Sharyl671254 (310 points)

0 votes

1 answer 64 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 JesseForwood (450 points)

0 votes

1 answer 59 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 BrandonEarnh (550 points)

0 votes

1 answer 64 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 NatishaReite (170 points)

0 votes

1 answer 62 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 AnnabelleBal (250 points)

0 votes

1 answer 64 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 LavonFriedma (330 points)

0 votes

1 answer 78 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 KristieMonck (330 points)

0 votes

1 answer 54 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 RemonaSharp0 (530 points)

0 votes

1 answer 54 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 JimmyBecker9 (290 points)

0 votes

1 answer 47 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 BCRMillie247 (310 points)

0 votes

1 answer 69 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 Michele43T64 (350 points)

0 votes

1 answer 48 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 FranciscoRug (210 points)

0 votes

1 answer 51 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 JarrodCoy68 (310 points)

0 votes

1 answer 63 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 JacquettaFor (330 points)

Categories