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The standard enthalpy of formation (∆f Ho) at 298 K for CH₄(g) is -74.8 KJ mol⁻1. The additional information required to determine the average energy of C-H bond would be
- a)the dissociation energy of H₂ and enthalpy of sublimation of carbon
- b)latent heat of vaporisation of methane
- c)first four ionisation energies of carbon and electron gain enthalpy of hydrogen
- d)the dissociation energy of H₂ molecule
Correct answer is option 'A'. Can you explain this answer?
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The standard enthalpy of formation (f Ho) at 298 K for CH(g) is -74.8 ...
Explanation:
To determine the average energy of C-H bond, we need to use the Hess's law, which states that the enthalpy change of a reaction is independent of the pathway between the initial and final states. We can use this law to calculate the energy of the C-H bond by comparing the enthalpy of formation of CH4 with the sum of the enthalpies of formation of C and H2.
The standard enthalpy of formation of CH4 is -74.8 kJ/mol, which means that 74.8 kJ of energy is released when 1 mole of CH4 is formed from its constituent elements. To calculate the energy of the C-H bond, we need to know the enthalpy of formation of C and H2.
The additional information required to determine the average energy of C-H bond would be:
a) The dissociation energy of H and enthalpy of sublimation of carbon:
The dissociation energy of H is the energy required to break the H-H bond, and the enthalpy of sublimation of carbon is the energy required to convert 1 mole of solid carbon into its gaseous state. These values are required to calculate the enthalpy of formation of C and H2 using Hess's law.
b) Latent heat of vaporization of methane:
The latent heat of vaporization of methane is the amount of energy required to convert 1 mole of methane from its liquid state to its gaseous state. This value is not required to calculate the energy of the C-H bond.
c) First four ionization energies of carbon and electron gain enthalpy of hydrogen:
The first four ionization energies of carbon are the energies required to remove 1, 2, 3, and 4 electrons from 1 mole of carbon atoms. The electron gain enthalpy of hydrogen is the energy released when 1 mole of hydrogen atoms gains 1 mole of electrons to form 1 mole of H- ions. These values are not required to calculate the energy of the C-H bond.
d) The dissociation energy of H molecule:
The dissociation energy of H molecule is the energy required to break the H-H bond in a molecule of H2. This value is required to calculate the enthalpy of formation of H2 using Hess's law, but it is not required to calculate the energy of the C-H bond.
Therefore, the correct answer is option 'A' - the dissociation energy of H and enthalpy of sublimation of carbon.
To determine the average energy of C-H bond, we need to use the Hess's law, which states that the enthalpy change of a reaction is independent of the pathway between the initial and final states. We can use this law to calculate the energy of the C-H bond by comparing the enthalpy of formation of CH4 with the sum of the enthalpies of formation of C and H2.
The standard enthalpy of formation of CH4 is -74.8 kJ/mol, which means that 74.8 kJ of energy is released when 1 mole of CH4 is formed from its constituent elements. To calculate the energy of the C-H bond, we need to know the enthalpy of formation of C and H2.
The additional information required to determine the average energy of C-H bond would be:
a) The dissociation energy of H and enthalpy of sublimation of carbon:
The dissociation energy of H is the energy required to break the H-H bond, and the enthalpy of sublimation of carbon is the energy required to convert 1 mole of solid carbon into its gaseous state. These values are required to calculate the enthalpy of formation of C and H2 using Hess's law.
b) Latent heat of vaporization of methane:
The latent heat of vaporization of methane is the amount of energy required to convert 1 mole of methane from its liquid state to its gaseous state. This value is not required to calculate the energy of the C-H bond.
c) First four ionization energies of carbon and electron gain enthalpy of hydrogen:
The first four ionization energies of carbon are the energies required to remove 1, 2, 3, and 4 electrons from 1 mole of carbon atoms. The electron gain enthalpy of hydrogen is the energy released when 1 mole of hydrogen atoms gains 1 mole of electrons to form 1 mole of H- ions. These values are not required to calculate the energy of the C-H bond.
d) The dissociation energy of H molecule:
The dissociation energy of H molecule is the energy required to break the H-H bond in a molecule of H2. This value is required to calculate the enthalpy of formation of H2 using Hess's law, but it is not required to calculate the energy of the C-H bond.
Therefore, the correct answer is option 'A' - the dissociation energy of H and enthalpy of sublimation of carbon.
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The standard enthalpy of formation (f Ho) at 298 K for CH(g) is -74.8 KJ mol1. The additional information required to determine the average energy of C-H bond would bea)the dissociation energy of H and enthalpy of sublimation of carbonb)latent heat of vaporisation of methanec)first four ionisation energies of carbon and electron gain enthalpy of hydrogend)the dissociation energy of H moleculeCorrect answer is option 'A'. Can you explain this answer?
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