Respuesta :
Activation energy can be calculated using the formula:
[tex]ln\frac{K_{1}}{K_{2}}=\frac{E_{a}}{8.314}[\frac{1}{T_{2}}-\frac{1}{T_{1}}][/tex]
At T₁=650 K, the rate constant, K₁ = 1.66 sec-1.
At T₂=700 K, the constant, K₂ =7.39 sec-1.
Putting the values in the above equation,
[tex]ln\frac{1.66}{7.39}=\frac{E_{a}}{8.314}[\frac{1}{700}-\frac{1}{650}][/tex]
Eₐ=1.12 ×10⁵ J mol⁻¹
or
Eₐ=112 KJ mol⁻¹
A decomposition reaction is the splitting of the reactant into two or more products. The activation energy for the reaction will be 112 kJ/mol.
What is activation energy?
Activation energy is the minimum energy required and essential for the reactant to have so the reaction can proceed and the products can be formed.
The activation energy can be given as,
[tex]\rm ln \dfrac{K_{1}}{K_{2}} = \rm \dfrac{E^{\circ}}{8.314} [\dfrac{1}{T_{2}}- \dfrac{1}{T_{1}}][/tex]
Given,
Initial temperature = 650 K
Final temperature = 700 K
Rate constant at initial temperature = 1.66 per sec
Rate constant at final temperature = 7.39 per sec
Substituting values in the above equation:
[tex]\begin{aligned}\rm ln \dfrac{1.66}{7.39} &= \rm \dfrac{E^{\circ}}{8.314} [\dfrac{1}{700} - \dfrac{1}{650}]\\\\&= 1.12 \times 10^{5} \;\rm J/mol\end{aligned}[/tex]
Therefore, the activation energy is 112 kJ/mol.
Learn more about activation energy here:
https://brainly.com/question/14119715
