The fictitious compound, arrhenium fluoride (AhF), reacts with itself to form a dimer with the formula Ah2F2 . The reaction is second order in AhF. The value of the rate constant is 8.591x10-3 M-1s-1. What is the initial rate of reaction in a reactor filled with AhF to a concentration of 5.5M ? Express your answer in M.s-1.

I understand that this is an exam question. Is that right?

No this is homework not an exam

rection rate=rate constant * conc^2

To find the initial rate of the reaction, we need to use the rate equation. The rate equation for a second-order reaction is given by:

rate = k[A]^2

Where:
- rate is the rate of the reaction
- k is the rate constant
- [A] is the concentration of the reactant

In this case, the reactant is AhF. The concentration of AhF is given as 5.5 M.

Plugging in the values into the rate equation:

rate = k[A]^2
rate = (8.591x10^(-3) M^(-1)s^(-1))(5.5 M)^2

Now, let's calculate the value of the initial rate:

rate = (8.591x10^(-3) M^(-1)s^(-1))(5.5 M)^2
rate = (8.591x10^(-3))(5.5)^2 M^(-1)s^(-1)
rate = (0.708) M.s^(-1)

Therefore, the initial rate of the reaction in a reactor filled with AhF to a concentration of 5.5 M is 0.708 M.s^(-1).