Answer:
After 1326s, the concentration of pyruvic acid fall to 1/64 of its initial concentration.
Explanation:
The first order kinetics reaction is:
ln [A] = ln [A]₀ - kt
Where [A] is concentration after t time, [A]₀ is intial concentration and k is reaction constant.
To convert half-life to k you must use:
t(1/2) = ln 2 / K
221s = ln 2 / K
K = ln 2 / 221s
If [A] = 1/64, [A]₀ = 1:
ln [A] = ln [A]₀ - kt
ln (1/64) = ln 1 - 3.1364x10⁻³t
4.1588 = 3.1364x10⁻³s⁻¹t
1326s = t
The time takes for the concentration of pyruvic acid to fall to 1/64 of its initial value in this first order reaction 1326s.
Time will be calculated by using the first order kinetics equation as:
ln [A] = ln [A]₀ - kt, where
[A] = final concentration = 1/64
[A]₀ = initial concentration = 1
t = required time
k is the rate constant and will be calculated by using the half life duration 221s as:
t(1/2) = ln2 / k
221s = ln2 / k
k = ln2 / 221s = 3.1364x10⁻³ per sec
Now putting all these values on the above equation, we get
ln (1/64) = ln 1 - 3.1364x10⁻³t
4.1588 = 3.1364x10⁻³s⁻¹t
1326s = t
Hence, required time is 1326s.
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https://brainly.com/question/518682
