Consider these reactions, where M represents a generic metal. 2 M ( s ) + 6 HCl ( aq ) ⟶ 2 MCl 3 ( aq ) + 3 H 2 ( g ) Δ H 1 = − 760.0 k J HCl ( g ) ⟶ HCl ( aq ) Δ H 2 = − 74.8 k J H 2 ( g ) + Cl 2 ( g ) ⟶ 2 HCl ( g ) Δ H 3 = − 1845.0 k J MCl 3 ( s ) ⟶ MCl 3 ( aq ) Δ H 4 = − 267.0 k J Use the given information to determine the enthalpy of the reaction 2 M ( s ) + 3 Cl 2 ( g ) ⟶ 2 MCl 3 ( s )

Answer : The enthalpy of the reaction is, -6209.8 kJ

Explanation :

According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.

The Main reaction is:

The intermediate balanced chemical reaction will be,

(1)    

(2)    

(3)    

(4)    

We are multiplying equation 3 by 3, reverse reaction of 4 by 2 and reaction 2 by 6 and then adding all the equations, we get :

(1)    

(2)    

(3)    

(4)    

The expression for enthalpy of the reaction is,

Therefore, the enthalpy of the reaction is, -6209.8 kJ