Respuesta :
Answer:
The standard reaction enthalpy for the given reaction is 235.15 kJ/mol.
Explanation:
[tex]O_2(g) \rightarrow \frac{2}{3}O_3(g),\Delta H^o_{1}=142.7 kJ/mol [/tex]..[1]
[tex]O_2(g) \rightarrow 2 O(g),\Delta H^o_{2}=498.4 kJ/mol [/tex]..[2]
[tex]NO(g) + O_3(g)\rightarrow NO_2(g) + O_2(g) ,\Delta H^o_{3} = -200 kJ/mol[/tex]..[3]
[tex]NO_2(g)\rightarrow NO(g) + O(g),\Delta H^o_{4}=? [/tex]..[4]
Using Hess's law:
Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.
2 × [4] = [2]- (3 ) × [1] - (2) × [3]
[tex]2\times \Delta H^o_{4}=\Delta H^o_{2} -3\times \Delta H^o_{1}-2\times \Delta H^o_{3}[/tex]
[tex]2\times \Delta H^o_{4}=498.4 kJ/mol-3\times 142.7 kJ/mol-2\times -200 kJ/mol[/tex]
[tex]2\times \Delta H^o_{4}=470.3 kJ/mol[/tex]
[tex]\Delta H^o_{4}=\frac{470.3 kJ/mol}{2}=235.15 kJ/mol[/tex]
The standard reaction enthalpy for the given reaction is 235.15 kJ/mol.
