Understanding the high-temperature formation and breakdown of the nitrogen oxides is essential for controlling the pollutants generated by car engines. the second-order reaction for the breakdown of nitric oxide to its elements has rate constants of 0.0796 l/mol-s at 737°c and 0.0815 l/mol-s at 947°c. what is the activation energy of this reaction? give your answer in scientific notation.

Question

Chemistry

Isabelle Simmons

9 September, 06:35

Understanding the high-temperature formation and breakdown of the nitrogen oxides is essential for controlling the pollutants generated by car engines. the second-order reaction for the breakdown of nitric oxide to its elements has rate constants of 0.0796 l/mol-s at 737°c and 0.0815 l/mol-s at 947°c. what is the activation energy of this reaction? give your answer in scientific notation.

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Krista · Answer 1

Answer is: activation energy of this reaction is 1062 J/mol.

Arrhenius equation: ln (k₁/k₂) = Ea/R (1/T₂ - 1/T₁).

k₁ = 0,0796 l/mol·s.

k₂ = 0,0815 l/mol·s.

1/T₁ = 1/737+273 = 0,00099 1/K.

1/T₂ = 1/947+273 = 0,00081 1/K.

ln (0,0796/0,0815) = Ea/8,3145 J/Kmol · (-0,00018 1/K).

0,023 / 0,00018 = Ea/8,3145 J/Kmol.

Ea = 1062 J/mol.