The rate constant for this first-order reaction is 0.610 s–1 at 400 °C.
A--->products
How long (in seconds) would it take for the concentration of A to decrease from 0.690 M to 0.260 M?
The rate constant for this second-order reaction is 0.590 M–1·s–1 at 300 °C.
How long (in seconds) would it take for the concentration of A to decrease from 0.950 M to 0.330 M?
The rate constant for this zero-order reaction is 0.0230 M·s–1 at 300 °C
How long (in seconds) would it take for the concentration of A to decrease from 0.890 M to 0.240 M?
First order reaction a= 0.690 a-x= 0.260 k1 =0.610 s-1 t=?
FORMULA TIME t=[2.303/k] log[0.690/0.260]
= 2.303/0.610 log [69/26]
= 3.77541 x[log69-log26]
= 3.77541 [1.8388-1.41497]
= 3.77541x0.42383
= 1.600 seconds
FOR second oder reaction
K2=1/t[(1/a-x)-1/a] k2= a-x= 0.330 a= 0.950
t=1/0.590[(1/0.330)-(1/0.950)]
t=1/0.590[3.030-1.052]
t=1/0.590[1.978]
t=3.3525 seconds
For Zero ORDER REACTION
a= 0.890 a-x= 0.240 k0=0.0230
t=1/k0[a-(a-x)]
t=[1/0.0230] x[0.890-0.240]
t= [1/0.0230][0.650]
t= 28.260secs
The rate constant for this first-order reaction is 0.610 s–1 at 400 °C. A--->products How long...
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