Give the ΔH value for the formation of binary compounds as shown in the reaction H2(s)+Br2(g)→2HBr(s)+36.3kJ.

Express your answer using three significant figures. If the value is positive, do not include the + sign in your answer.

In the above equation , the amount of energy i.e. 36.3 kJ is released , i.e. it is in the product side , hence , the reaction is an example of an exothermic reaction .

Hence ,

The value of the change in enthalphy , i.e. , the enthalpy of product minus the enthalpy of the product .

Therefore ,

The value of the change in enthalphy = - ve .

Hence ,

ΔH = - 36.3 kJ

Give the ΔH value for the formation of binary compounds as shown in the reaction H2(s)+Br2(g)→2HBr(s)+36.3kJ. Express your answer using three significant figures. If the value is positive, do not include the + sign in your answer.

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Give the ΔH value for the formation of binary compounds as shown in the reaction H2(s)+Br2(g)→2HBr(s)+36.3kJ.

Express your answer using three significant figures. If the value is positive, do not include the + sign in your answer.