Question

The decomposition of N₂O₅ to NO₂ and O₂ is a first order reaction where Rate=k[N₂O₅]It has been found experimentally that the decomposition is 80% remains after 325 s at 300K. Calculate the rate constant.

Answer 1

To find the rate constant for this first-order reaction, use the equation ln([A]0/[A]) = kt with the given concentration data (80% remains after 325 seconds) to calculate k.

Step-by-step explanation:

The student is asking to calculate the rate constant (k) for the first-order reaction of the decomposition of N2O5 to NO2 and O2, where it's given that 80% of N2O5 remains after 325 seconds at 300K.

For a first-order reaction, the rate constant can be calculated using the formula k = ln(2) / t1/2, where t1/2 is the half-life of the reaction. If 80% of the reactant remains, 20% has decomposed, meaning we need to find the time it takes for half of the N2O5 to decompose (half-life).

Let's use the first-order kinetics equation: ln([A]0/[A]) = kt, where [A]0 is the initial concentration and [A] is the concentration at time t. Here, [A]0/[A] = 1/0.8 since only 80% remains, and t = 325 s. Through calculation, we can find the value of k.