What is the rate of reaction when [A] 0.20 M?

Question

A reaction in which A —–> products was monitored as a function of time and the results are shown below. Time (s) —- [A] (M) 0 —- 1.000 25 —- 0.914 50 —– 0.829 75 —- 0.744 100 —– 0.659 125 —– 0.573 150 —– 0.488 175 —– 0.403 200 —– 0.318 Okay, well I know the order of the reactions is 0.Determine the value of the rate constant. What is the rate of reaction when [A] 0.20 M?

Raymond Moen · Accepted Answer

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⁻¹Alternatively you can make regression analysis.Least square fit of a line of the formy = k∙x to a set of data pairs (x,y)leads to k = ∑(y∙x) / ∑( x² )(∑ denotes summation over all data points)For this problemx = ty = [A]₀ – [A] => k = 3.41×10⁻³Ms⁻¹2.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

Dr. Frankie Medhurst

What is the rate of reaction when [A] 0.20 M?

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