In the reaction, a → products, a plot of ln[a] vs. time is linear and the slope is equal to -0.860 s-1. how long will it take one-half of the initial amount of a to react?

The study of chemicals and bonds is called chemistry. There are different types of elements and these are metals and nonmetals.

The correct answer is -0.806sec.

The plot for ln[a] verses t is linear for a first-order reaction. The integrated rate law equation is as follows:

Here,

The equation will be:-

Compared with the equation for linear graph, y=mx+c

Thus, slope =-k

The value of k will be 0.860

Now, if the final concentration becomes half of its initial value .

Place all the values and rearrange them.

Hence, the correct answer is 0.860.

For more information about the half-life, refer to the link:-

link

The reaction is given as follows:

The plot of ln[a] verses t is linear with slope .

The plot for ln[a] verses t is linear for first order reaction. The integrated rate law equation is as follows:

Here, k is rate constant, t is time of the reaction, is concentration of reactant at time t and is initial concentration of reactant.

Taking ln both sides,

...... (1)

Comparing with equation for linear graph, y=mx+c

Thus, slope =-k

Or,

Now, if final concentration become half of its initial value, and t becomes

Putting the values in equation (1)

On rearranging,

Therefore, it takes 0.806 sec to react half of the reactant a.

it takes on an electronical energy