Respuesta :
Explanation:
According to Arrhenius equation with change in temperature, the formula is as follows.
ln [tex]\frac{K_{2}}{K_{1}}[/tex] = [tex]\frac{-E_{a}}{R}[\frac{1}{T_{2}} - \frac{1}{T_{1}}][/tex]
Since, it is given that [tex]K_{1}[/tex] is 0.0191 [tex]s^{-1}[/tex], [tex]T_{1}[/tex] is 24 degree celsius equals 297 K, [tex]T_{2}[/tex] is 120 degree celsius equals 393 K, and [tex]E_{a}[/tex] is 43.4 kJ/mol or 43400 J/mol.
Therefore, putting the value in the above formula as follows.
ln [tex]\frac{K_{2}}{K_{1}}[/tex] = [tex]\frac{-43400 J/mol}{8.314 j/mol K}[\frac{1}{393} - \frac{1}{297}][/tex]
ln [tex]\frac{K_{2}}{0.0191 s^{-1}}[/tex] = [tex]\frac{-E_{a}}{R}[\frac{1}{T_{2}} - \frac{1}{T_{1}}][/tex]
[tex]K_{2}[/tex] = 1.40 [tex]s^{-1}[/tex]
Thus, we can conclude that rate constant be at a temperature of 120°C for a reaction with an activation energy of 43.4 kJ/mol is 1.40 [tex]s^{-1}[/tex].
