NO(g) + Cl2(g) → NOCl(g) + Cl(g) 4.0×10^9 /M•s 85 kJ/mol 500℃ rate constant

NO(g) + Cl2(g) → NOCl(g) + Cl(g) 4.0×10^9 /M•s 85 kJ/mol 500℃ rate constant

 

 

Consider the second-order reaction

NO(g) + Cl2(g) → NOCl(g) + Cl(g)

Given that the frequency factor and activation energy

for the reaction are 4.0×10^9 /M•s and 85 kJ/mol,

respectively, calculate the rate constant at 500℃.

 

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아레니우스 식

k = Ae^(–Ea/RT)

( 참고 https://ywpop.tistory.com/7288 )

 

= (4.0×10^9 /M•s) e^[(–85000 J/mol) / ((8.314 J/mol•K) × (273.15+500 K))]

= (4.0×10^9) e^[(–85000) / ((8.314) × (273.15+500))]

= 7231 /M•s

 

 

 

답: k = 7200 /M•s

 

 

 

 

[키워드] 아레니우스 식 기준문서, 2차 반응 기준문서, NO + Cl2 → NOCl + Cl