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 6.091×10−3 M−1s−1. What is the initial rate of reaction in a reactor filled with AhF to a concentration of 3.5 M? Express your answer in M⋅s−1.
Rate Constant * Concentration^2
To find the initial rate of reaction, we can use the rate equation for a second-order reaction:
Rate = k[AhF]^2
Where:
Rate is the rate of reaction in M⋅s^−1,
k is the rate constant, and
[AhF] is the concentration of AhF.
Given:
k = 6.091×10−3 M^−1s^−1
[AhF] = 3.5 M
Substituting these values into the rate equation:
Rate = (6.091×10−3 M^−1s^−1) × (3.5 M)^2
Rate = (6.091×10−3) × (3.5 M)^2
Rate = (6.091×10−3) × (3.5)^2
Rate = (6.091×10−3) × (12.25)
Calculating this expression gives the value of the initial rate of reaction in M⋅s^−1.