The rate constant for this first-order reaction is 0.610 s–1 at 400 °C. A--->pro

ID: 888667 • Letter: T

Question

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

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.