Given that the initial rate constant is 0.0191 s-1 at an initial temperature of 24°c, what would the rate constant be at a temperature of 120°c for a reaction with an activation energy of 43.4 kj/mol?

Explanation:

According to Arrhenius equation with change in temperature, the formula is as follows.

             ln =

Since, it is given that is 0.0191 , is 24 degree celsius equals 297 K, is 120 degree celsius equals 393 K, and is 43.4 kJ/mol or 43400 J/mol.

Therefore, putting the value in the above formula as follows.

               ln =

                ln =

                      = 1.40

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 .

d they tend to lose electrons and become cations.

explanation:

0.11 m/s and 0.28 m/s should be correct