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.
0.0746
Rate Constant * Concentration^2
To find the initial rate of reaction in a reactor filled with AhF to a concentration of 3.5 M, we can use the second-order rate law equation:
rate = k * [AhF]^2
Where:
rate is the initial rate of reaction
k is the rate constant
[AhF] is the concentration of AhF
In this case, we are given the value of the rate constant (k = 6.091×10^−3 M^−1s^−1) and the concentration of AhF ([AhF] = 3.5 M).
Plugging in these values into the rate law equation, we have:
rate = (6.091×10^−3 M^−1s^−1) * (3.5 M)^2
First, calculate the square of the concentration of AhF:
(3.5 M)^2 = 12.25 M^2
Then, multiply the rate constant by the squared concentration:
rate = (6.091×10^−3 M^−1s^−1) * 12.25 M^2
To simplify the units, we can cancel out one of the M units in the concentration with the M in the rate constant:
rate = (6.091×10^−3 s^−1) * 12.25 M
Now, simply multiply the two values:
rate = 0.0746 M⋅s^−1
Therefore, the initial rate of reaction in the reactor filled with AhF to a concentration of 3.5 M is 0.0746 M⋅s^−1.