Question

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: $H_{2}$(g) + $Br_{2}$(g) → 2HBr(g), Given that Bond energy of $H_{2}$, $Br_{2}$ and HBr is 435 kJ $mol^{-1}$, 192 kJ $mol^{-1}$ and 368 kJ $mol^{-1}$ respectively.

Answer 1

Risk capital establishment established for:-

a) Import analysis
b) Export analysis
c) none
d) both

Answer 2

Explanation:

ANSWER

Δ

r

H

⊖

=∑ bond enthalpies

reactants

=−∑ bond

enthalpies

products

Δ

r

H

∘

=bond energy of H

2

+Bond crergy of Br

2

−2×Bond

energy of HBr

=435+192−(2×368)kJmol

−1

Δ

r

H

⊖

=−109KJmol

−1