Answer:
16.1 s
Explanation:
The reaction, A → Products, follows first order kinetics.
So,
ln[A] = ln[A]o - kt
Where;
[A] = concentration at time= t
[A]o = initial concentration
k= rate constant
t = time taken
ln(0.205) = ln(0.850) - 0.0882t
ln(0.205) - ln(0.850) = - 0.0882t
-1.5847 - (-0.1625) = - 0.0882t
-1.5847 + 0.1625 = - 0.0882t
-1.4222 = - 0.0882t
t = -1.4222/- 0.0882
t = 16.1 s
Based on first order kinetics, the time taken for the concentration of A to decrease from 0.850 M to 0.205 M is 16.1 seconds.
The order of a reaction refers to the relationship between the rate of a reaction and the the concentration of each reactant.
For a first-order reaction, the rate is dependent on the concentration of a single species.
The reaction, A → Products is a first order reaction.
Therefore, using the first order kinetics equation
ln[A] = ln[A]° - kt
Where;
Substituting the values:
ln(0.205) = ln(0.850) - 0.0882t
ln(0.205) - ln(0.850) = - 0.0882t
-1.5847 - (-0.1625) = - 0.0882t
-1.5847 + 0.1625 = - 0.0882t
-1.4222 = - 0.0882t
t = -1.4222/- 0.0882
t = 16.1 s
Therefore, the time taken for the concentration of A to decrease from 0.850 M to 0.205 M is 16.1 seconds.
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