Answer:
4.748 seconds
Step-by-step explanation:
second-order is one in which the rate is proportional to the square of the concentration of one reactant. This can be expressed below;
2A----->P
Where
A is the reactant.
P is the product.
The rate can be expressed as
Rate= k[A]^2
Half-life reffers to time required to reduce the concentration of reactant to half of its initial value.
The half life of reaction can be calculated using below formula
Half-life =. 1/(K*I)
Where,
K = Rate constant = 0.54 1/ms
I = Initial concentration = 0.39 m
If we substitute these values we have
Half-life t(1/2) =1/(0.54×0.39)
=4.748 seconds
Therefore, the half life is 4.748 seconds