Consider the following hypothetical aqueous reaction. A flask is charged with .065 mol of A in a total volume of 100.0 mL. The following data are collected: Time (min) 0 10 20 30 40
Moles of A 0.065 0.051 0.042 0.036 0.031
This is a second order reaction.
What is the value of the rate constant for the reaction?

0.422 M⁻¹s⁻¹

Explanation: Reaction Rate is the speed of decomposition of the reactant(s) per unit of time.

A Rate Law relates concentration of reactants, rate reaction and rate constant:

where

[A] and [B] are reactants concentration

x and y are reaction order, not related to the stoichiometric coefficients

k is rate constant

r is rate

Before calculating rate constant, first we have to determine reaction order.

In this question, the reactio order is 2. So, the rate law for it is

and the integrated formula is

in which

[A]₀ is initial concentration of reactant

Then, using initial concentration at initial time and final concentration at final time:

k = 0.422

The rate constant for the reaction is 0.422 M⁻¹.s⁻¹

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