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.

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., ∆ r H ⊖ = +134 kJ mol –1, ∆ r H ⊖ = +109 kJ mol –1, ∆ r H ⊖ = –134 kJ mol –1, ∆ r H ⊖ = –109 kJ mol –1

MARKS App · Accepted Answer

Correct Option is : (D) ∆ r H ⊖ = –109 kJ mol –1

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