The first-order rate law is given by the equation:
ln([A]t/[A]0) = -kt
Where [A]t is the concentration of reactant at time t, [A]0 is the initial concentration, k is the rate constant, and t is time.
We can rearrange this equation to solve for time t:
t = ln([A]0/[A]t)/k
Plugging in the given values:
t = ln(0.5/0.05)/1.00*10^-2
t = 16.1 min
Therefore, it will take approximately 16.1 minutes for the concentration of the reactant to reduce to 0.05 mol/L.
The rate constant of a first order reaction k is 1.00*10^-2 and an initial concentration of 0.5mol/l. At what time will the concentration reduce to 0.05mol/l
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