Answer: The [tex]\Delta H_{rxn}[/tex] for the given chemical reaction is -175.51 kJ/mol
Explanation: Enthalpy change of the reaction is defined as the amount of heat released or absorbed in a given chemical reaction.
Mathematically,
[tex]\Delta H_{rxn}=\Delta H_f_{(products)}-\Delta H_f_{(reactants)}[/tex]
We are given a chemical reaction. The reaction follows:
[tex]NH_3(g)+HCl(g)\rightarrow NH_4Cl(s)[/tex]
[tex]H_f_{(NH_3)}=-46.19kJ/mol[/tex]
[tex]H_f_{(HCl)}=-92.30kJ/mol[/tex]
[tex]H_f_{(NH_4Cl)}=-314.4kJ/mol[/tex]
Enthalpy change for the reaction of he given chemical reaction is given by:
[tex]\Delta H_{rxn}=H_f_{(NH_4Cl)}-(H_f_{(NH_3)}+H_f_{(HCl)})[/tex]
Putting the values in above equation, we get
[tex]\Delta H_{rxn}=-314.4-(-92.30-46.19)kJ/mol[/tex]
[tex]\Delta H_{rxn}=-175.51kJ/mol[/tex]
