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For Br2(l) Enthalpy of atomisation = x kJ/mol Bond dissociation enthalpy of bromine = y kJ/mole
then
then
- a)x > y
- b)x < y
- c)x = y
- d)Relation does not exist
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
For Br2(l) Enthalpy of atomisation = x kJ/mol Bond dissociation enthal...
ΔHatomisation = ΔHvap + Bond energy
Hence x > y
Most Upvoted Answer
For Br2(l) Enthalpy of atomisation = x kJ/mol Bond dissociation enthal...
Understanding Enthalpy of Atomisation
The enthalpy of atomisation refers to the energy required to break down a substance into its individual atoms in the gas phase. For bromine (Br2), the enthalpy of atomisation is the energy required to convert liquid bromine into gaseous bromine atoms.
Bond Dissociation Enthalpy of Bromine
The bond dissociation enthalpy (BDE) is the energy required to break a specific bond in a molecule. For bromine, this represents the energy needed to break the Br-Br bond in a bromine molecule to form two separate gaseous bromine atoms.
Comparison of x and y
- Enthalpy of Atomisation (x): This value reflects the energy needed to completely separate the atoms of bromine from the liquid phase into gaseous atoms.
- Bond Dissociation Enthalpy (y): This value is specifically the energy required to break the Br-Br bond.
Why x > y
- The enthalpy of atomisation (x) is greater than the bond dissociation enthalpy (y) because the enthalpy of atomisation accounts for both the energy needed to break the Br-Br bond and the energy associated with the phase change from liquid to gas.
- In essence, when you convert liquid bromine to gaseous bromine atoms, you also need to overcome intermolecular forces in addition to breaking the bond between the bromine atoms.
Conclusion
Thus, since the enthalpy of atomisation encompasses both the bond dissociation and the energy needed to overcome intermolecular forces in the liquid phase, it is correctly concluded that:
x > y
This leads to the selection of option 'A' as the correct answer.
The enthalpy of atomisation refers to the energy required to break down a substance into its individual atoms in the gas phase. For bromine (Br2), the enthalpy of atomisation is the energy required to convert liquid bromine into gaseous bromine atoms.
Bond Dissociation Enthalpy of Bromine
The bond dissociation enthalpy (BDE) is the energy required to break a specific bond in a molecule. For bromine, this represents the energy needed to break the Br-Br bond in a bromine molecule to form two separate gaseous bromine atoms.
Comparison of x and y
- Enthalpy of Atomisation (x): This value reflects the energy needed to completely separate the atoms of bromine from the liquid phase into gaseous atoms.
- Bond Dissociation Enthalpy (y): This value is specifically the energy required to break the Br-Br bond.
Why x > y
- The enthalpy of atomisation (x) is greater than the bond dissociation enthalpy (y) because the enthalpy of atomisation accounts for both the energy needed to break the Br-Br bond and the energy associated with the phase change from liquid to gas.
- In essence, when you convert liquid bromine to gaseous bromine atoms, you also need to overcome intermolecular forces in addition to breaking the bond between the bromine atoms.
Conclusion
Thus, since the enthalpy of atomisation encompasses both the bond dissociation and the energy needed to overcome intermolecular forces in the liquid phase, it is correctly concluded that:
x > y
This leads to the selection of option 'A' as the correct answer.
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For Br2(l) Enthalpy of atomisation = x kJ/mol Bond dissociation enthalpy of bromine = y kJ/molethena)x > yb)x < yc)x = yd)Relation does not existCorrect answer is option 'A'. Can you explain this answer?
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