Recent questions in ThermoChemistry

0 votes

1 answer 63 views

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 OtisMacGilli (2.0k points)

0 votes

1 answer 69 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 ZakOleary170 (1.8k points)

0 votes

1 answer 68 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 JudithMackni (2.3k points)

0 votes

1 answer 71 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 JulianKnetes (2.0k points)

0 votes

1 answer 71 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 PeggyBednall (1.9k points)

0 votes

1 answer 86 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 MerryGoodsel (1.9k points)

0 votes

1 answer 78 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 NadiaN491716 (2.1k points)

0 votes

1 answer 75 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 GabrielCantu (1.6k points)

0 votes

1 answer 79 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 ChanteStroh (1.5k points)

0 votes

1 answer 65 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 TimNakamura (2.0k points)

0 votes

1 answer 70 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 IsabellaOcto (1.9k points)

0 votes

1 answer 80 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 AlineBacon1 (1.5k points)

0 votes

1 answer 67 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 UweEales0685 (1.8k points)

0 votes

1 answer 81 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 JordanChun58 (2.3k points)

0 votes

1 answer 79 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 FerminRosale (1.5k points)

0 votes

1 answer 75 views

Calculate the amount of heat that needs to be absorbed to crystallize 100 grams of sodium acetate (CH3COONa) from a saturated solution at 40°C. The heat of crystallization for sodium acetate is -264 kJ/mol.

asked Jan 23 in ThermoChemistry by VickeyPeacoc (2.4k points)

0 votes

1 answer 72 views

Calculate the amount of heat required to sublime 50 grams of dry ice (CO2) at -78.5°C given that the heat of sublimation for CO2 is 25.2 kJ/mol.

asked Jan 23 in ThermoChemistry by JonasHaller8 (1.5k points)

0 votes

1 answer 69 views

Calculate the amount of heat required to sublimate 10 grams of dry ice (solid carbon dioxide) at a temperature of -78.5°C. The heat of sublimation of carbon dioxide is 25.2 kJ/mol.

asked Jan 23 in ThermoChemistry by BYUBlake479 (2.0k points)

0 votes

1 answer 74 views

Calculate the amount of heat required to raise the temperature of 50 grams of water from 25°C to 85°C, given the specific heat of water is 4.184 J/g°C.

asked Jan 23 in ThermoChemistry by AgnesXyg5256 (2.0k points)

0 votes

1 answer 65 views

Calculate the amount of heat required to polymerize 2 moles of styrene into polystyrene given the following information:The enthalpy of polymerization for styrene is -56 kJ/mol and the reaction is exothermic.

asked Jan 23 in ThermoChemistry by NamSampson2 (1.8k points)

Categories