The reaction A(aq) → B(aq) is a first order reaction. If it takes 300.0 seconds for the concentration of A to decrease in concentration from 0.50 M to 0.010 M, what is the rate constant for this reaction?
57 s-1 |
1.5 x 10-2 s-1 |
1.3 x 10-2 s-1 |
1.6 x 10-3 s-1 |
1.8 x 10-2 |
Solution:
For a first order reaction, the expession for rate constant (k) is expressed as:
k = (2.303/t) log (a/a-x)
a = initial concentration = 0.50 M
(a-x) =final concentration = 0.010 M
t = time = 300 sec, then,
k = (2.303/ 300 sec) log (0.50 M / 0.010 M)
k = (2.303/ 300 sec) log 50
k = (2.303 / 300 sec) x 1.6990
k = 1.3 x 10^-2 sec-1
Hence, option is C.
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