Answer:
∆H° of reaction is -30.91 KJ/mol.
Explanation:
Given data:
∆Hf ° of Br2 (g) = 30.91 KJ/mol
∆H° of reaction = ?
Solution:
we know that standard heat of formation for Br2 (l) is 0.0 KJ/mol.
Balance chemical equation:
Br2 (g) → Br2 (l)
Formula:
∆H° = ∆Hf ° (product) - ∆Hf °(reactant)
∆H° = 0.0 KJ/mol - 30.91 KJ/mol
∆H° = - 30.91 KJ/mol
