Respuesta :
Answer: The reaction is exothermic in nature and the value of q is 852 kJ
Explanation:
Endothermic reactions are defined as the reactions in which energy of products is more than the energy of the reactants. In these reactions, energy is absorbed by the system. The energy term is written on the reactant side of the reaction.
Exothermic reactions are defined as the reactions in which energy of reactants is more than the energy of the products. In these reactions, energy is released by the system. The energy term is written on the product side of the reaction.
We are given:
Heat released in the reaction = 852 kJ/mol
The chemical equation follows:
[tex]Fe_2O_3(s)+2Al(s)\rightarrow Al_2O_3(s)+2Fe(s)+852kJ[/tex]
As, heat is released during the reaction, it is considered as an exothermic reaction.
To calculate the enthalpy change of the reaction, we use the equation:
[tex]\Delta H_{rxn}=\frac{q}{n}[/tex]
where,
[tex]q[/tex] = amount of heat released
n = number of moles = 1 mole
[tex]\Delta H_{rxn}[/tex] = enthalpy change of the reaction = 852 kJ/mol
Putting values in above equation, we get:
[tex]852kJ/mol=\frac{q}{1mol}\\\\q=(852kJ/mol\times 1mole)=852kJ[/tex]
Hence, the reaction is exothermic in nature and the value of q is 852 kJ
