Final answer:
To find the concentration of A after 855 seconds, we can use the integrated rate law for a second-order reaction. With the initial concentration and the rate constant provided,
Step-by-step explanation:
The student has asked to calculate the concentration of reactant A after 855 seconds given the reaction's rate constant and initial concentration. This is a typical chemistry problem involving reaction kinetics and the use of rate laws to determine concentrations over time.
The rate constant for the reaction is given as 0.800 M⁻¹ ⋅ s⁻¹ and the initial concentration of A is 0.00320 M. Since the rate constant has units of M⁻¹ ⋅ s⁻¹, this suggests that the reaction is of second-order with respect to A. The integrated second-order rate law is given by:
1/[A] = kt + 1/[A]0
Where:
- [A] = concentration of A at time t
- k = rate constant
- t = time
- [A]0 = initial concentration of A
Substituting the provided values:
1/[A] = (0.800 M⁻¹ ⋅ s⁻¹)(855 s) + 1/(0.00320 M)
After solving for [A], this will yield the concentration of A after 855 seconds.