In the reaction, A → Products, a plot of 1/[A] vs. time is linear and the slope is equal to 0.056 M−1 s−1. If the initial concentration of A is 0.80 M, how long will it take one-half of the initial amount of A to react?

t = 22.32 s

Explanation:

The kinetics of a reaction can be known graphically by plotting the concentration vs time experimental data on a sheet of graph.

Given that:- 1/[A] vs. time is linear which means it follows second order kinetics.

Thus,

Given that slope = k = 0.056 M⁻¹ s⁻¹.

Integrated rate law for second order kinetic is:

Where, is the final concentration  = Half of the initial concentration = 0.80 /2 M = 0.40 M

is the initial concentration  = 0.80 M

So,  

t = 22.32 s

a is the answer

explanation:

which statement about trans-fatty acids is false?

a. the conversion of cis-fatty acids to trans-fatty acids is inhibited by the presence of antioxidants.

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