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

Question

A reaction where A → products was monitored over time, and the following data was collected:
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  
Given that the reaction is zero-order, determine the value of the rate constant. Additionally, calculate the rate of reaction when [A] = 0.20 M.

Beau Eichmann · Accepted Answer

1.Zero order integrated rate law is:[A] = [A]&#8320; &ndash; k&#8729;t[A]&#8320; 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&times;10&#8315;&sup3;Ms&#8315;&sup1;Alternatively you can make regression analysis.Least square fit of a line of the formy = k&#8729;x to a set of data pairs (x,y)leads to k = &sum;(y&#8729;x) / &sum;( x&sup2; )(&sum; denotes summation over all data points)For this problemx = ty = [A]&#8320; &ndash; [A] =>k = 3.41&times;10&#8315;&sup3;Ms&#8315;&sup1;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&times;10&#8315;&sup3;Ms&#8315;&sup1;

Alexie Dach

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

1 Answers

AI-Powered Insights

Want to answer this question?

Categories

Tags

Related Questions