A reaction in which A —–> products was monitored as a function of time and the results are shown below.

**Answer 1**

1.

Zero order integrated rate law is:

[A] = [A]₀ – k∙t

[A]₀ denotes initial concentration.

So if you plot [A] versus t you get a straight line with the slope -k.

The result should be something about:

k = 3.4×10⁻³Ms⁻¹

Alternatively you can make regression analysis.

Least square fit of a line of the form

y = k∙x

to a set of data pairs (x,y)

leads to

k = ∑(y∙x) / ∑( x² )

(∑ denotes summation over all data points)

For this problem

x = t

y = [A]₀ – [A]

=>

k = 3.41×10⁻³Ms⁻¹

2.

The rate of a zero order reaction is dependent from the concentration level. As long as some reactant is present it will react away at the same, constant rate.:

rate = -d[A]/dt = k = 3.41×10⁻³Ms⁻¹