The net enthalpy change of a reaction is the amount of energy required to break all the bonds in reactant molecules minus amount of energy required to form all the bonds in the product molecules. What will be the enthalpy change for the following reaction.
H2(g) + Br2(g) → 2HBr(g)
Given that Bond energy of H2, Br2 and HBr is 435 kJ/ mol, 192 kJ/ mol and 368 kJ/ mol respectively
The net enthalpy change of a reaction is the amount of energy required to break all the bonds in reactant molecules minus amount of energy required to form all the bonds in the product molecules. What will be the enthalpy change for the following reaction.
H2(g) + Br2(g) → 2HBr(g)
Given that Bond energy of H2, Br2 and HBr is 435 kJ/ mol, 192 kJ/ mol and 368 kJ/ mol respectively
This is a Short Answer Type Questions as classified in NCERT Exemplar
ΔrH? =ΣB.E (reactant)-ΣB.E (product)
=B.E.H2 + BEBR2 -2 *B.E>HBr
= 435+192-2 (*368)
= 109KJmol-1
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