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 5.591×10−3 M−1s−1. What is the initial rate of reaction in a reactor filled with AhF to a concentration of 3.0 M? Express your answer in M⋅s−1
use the formula
rection rate=rate constant * conc^2
and the answer is=0.050319
To determine the initial rate of reaction, we need to use the rate equation for a second order reaction. The rate equation for a second order reaction is:
Rate = k * [A]^2
Where:
- Rate is the rate of reaction
- k is the rate constant
- [A] is the concentration of the reactant
In this case, the reactant is AhF and its concentration is 3.0 M. The rate constant is given as 5.591×10^-3 M^-1s^-1.
Plugging in the values, we have:
Rate = (5.591×10^-3 M^-1s^-1) * (3.0 M)^2
Simplifying the equation, we have:
Rate = (5.591×10^-3) * (9.0) M^2 s^-1
Rate = 0.05032 M⋅s^-1
Therefore, the initial rate of reaction in the reactor filled with AhF to a concentration of 3.0 M is 0.05032 M⋅s^-1.