Answer:
The enthalpy of reaction per mole of HBr for this reaction = ΔrH = -40.62 kJ/mole.
Explanation:
2HBr(g) + Cl2(g) → 2HCl(g) + Br2(g)
When 23.9 g HBr(g) reacts with sufficient Cl2(g), 12.0 kJ of heat is evolved, calculate the value of ΔrH for the chemical reaction.
Note that ΔrH is the enthalpy per mole for the reaction.
Molar mass of HBr (g) = 80.91 g/mol.
Hence, 1 mole of HBr = 80.91 g
23.9 g of HBr led to the reaction giving off 12.0 kJ of heat
80.91 g of HBr will lead to the evolution of (80.91 × 12/23.9) = 40.62 kJ heat is given off.
Hence, 40.62 kJ of heat is given off per 80.91 g of HBr.
This directly translates to that 40.62 kJ of heat is given off per 1 mole of HBr
Hence, the heat given off per mole of HBr for this reaction is 40.62 kJ/mole.
But since the reaction liberates heat, it means the reaction is exothermic and the enthalpy change for the reaction (ΔHrxn) is negative.
Hence, ΔrH = -40.62 kJ/mole.
Hope this Helps!!!
