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 5.5 M? Express your answer in M⋅s−1.
THIS IS NOT AN EXAM QUESTION
rection rate=rate constant * conc^2
To determine the initial rate of reaction, we will use the rate equation for a second-order reaction:
rate = k[A]^2
where "rate" is the initial rate of reaction, k is the rate constant, and [A] is the concentration of AhF.
In this scenario, the concentration of AhF is 5.5 M, and the rate constant is 8.591x10^-3 M^(-1)s^(-1). We can plug in these values into the rate equation to find the initial rate:
rate = (8.591x10^-3 M^(-1)s^(-1))(5.5 M)^2
rate = (8.591x10^-3 M^(-1)s^(-1))(30.25 M^2)
rate ≈ 0.2609 M⋅s^(-1)
Therefore, the initial rate of reaction in the reactor filled with AhF to a concentration of 5.5 M is approximately 0.2609 M⋅s^(-1).