A + 2B → C
was studied by measuring the [A] as a function of time. Reactant B was always present in excess and it was assumed that the [B] remained essentially constant during the reaction. Shown below is a table of the [A] as a function of time, in seconds. In this experiment, [B] = 1.0 M. Also shown is the plot of these data which gave a linear relationship, ln[A] versus time.
t (s) [A] (M)
40 0.220
80 0.162
120 0.119
160 0.088
200 0.065
Click the following link to see the graph:
https://access1.lon-capa.uiuc.edu/res/uiuc/cyerkes/post_lab_4/pl4ver1-2.gif
When the [B] was doubled, the rate of the reaction doubled, making it first order in B.
Use these data to solve for kapp and k.
Remember that you are measuring the apparent rate constant (kapp) which is related to the true rate constant (k) by the equation kapp = k [B]
The apparent rate constant (kapp) and true rate constant (k) are:
a.)kapp = 9.69 x 10-4 s-1, k = 1.94 x 10-3 M-1 s-1
b.)kapp = 9.69 x 10-4 s-1, k = 4.84 x 10-4 M-1 s-1
c.)kapp = 7.62 x 10-3 s-1, k = 3.81 x 10-3 M-1 s-1
d.)kapp = 7.62 x 10-3 s-1, k = 1.52 x 10-3 M-1 s-1
e.)kapp = 7.62 x 10-3 s-1, k = 7.62 x 10-3 M-1 s-1
更新1:
I rearrange it , hope it will make you easier understand t (s) [A] (M) 40 0.220 80 0.162 120 0.119 160 0.088 200 0.065
更新2:
t (s)--- [A] (M) 40--- 0.220 80--- 0.162 120 ---0.119 160 ---0.088 200 ---0.065
