In Example 15.3, you determined that the decomposition of SO₂Cl₂ (under the given reaction conditions) is first order and has a rate constant of +2.90 * 10^-4 s^-1. If the reaction is carried out at the same temperature and the initial concentration of SO₂Cl₂ is 0.0225 M, what is the SO₂Cl₂ concentration after 865 s?

Example 15.3

Consider the equation for the decomposition of SO₂Cl₂:

The concentration of SO₂Cl₂ is monitored at a fixed temperature as a function of time during the decomposition reaction, and the following data are tabulated:

Show that the reaction is first order, and determine the rate constant for the reaction.

Transcribed Image Text:

SORT You are given the rate constant of a first-order reaction and the initial concentration of the reactant and asked to find the concentration at 865 seconds. STRATEGIZE Refer to the first-order integrated rate law to determine the SO₂Cl₂ concentration at t = 865 s. GIVEN: k = +2.90 x 10-4s-1 [SO₂Cl2]0= 0.0225 M FIND: [SO₂Cl₂] at t = 865 s EQUATION In [A], = -kt + In [A]o