The reaction x products follows Ist order kinetics in 40 minutes the concetration of x changes from 0.1M to 0.025M then the rate of reaction when conc of x is 0.01
To determine the rate of the reaction when the concentration of X is 0.01 M, we need to find the rate constant (k) for the reaction.
The rate law for a first-order reaction is given by the equation:
rate = k[A]
where [A] is the concentration of reactant A, and k is the rate constant.
We are given that the reaction follows first-order kinetics and takes 40 minutes (t) for the concentration of X ([X]) to change from 0.1 M to 0.025 M.
We can use the integrated rate law for a first-order reaction to find the rate constant (k):
ln([X]0/[X]) = kt
where [X]0 is the initial concentration of X, [X] is the concentration of X at time t, k is the rate constant, and ln is the natural logarithm.
Substituting the given values, we have:
ln(0.1/0.025) = k * 40
Solving this equation for k, we get:
k ≈ (ln(0.1/0.025)) / 40
Now that we have the rate constant, we can use it to determine the rate of the reaction when [X] is 0.01 M.
Using the rate law equation:
rate = k[X]
Substituting the values:
rate = (ln(0.1/0.025)) / 40 * 0.01
Evaluating this expression will give you the rate of the reaction when [X] is 0.01 M.