Answer:
0.16 M.
Explanation:
Hello!
In this case, since the reaction can be determined as zeroth-order because of the units of M/s, we can write the rate law as:
[tex][X]=[X]_0-kt[/tex]
In such a way, since we need the initial concentration of X, we proceed as follows:
[tex][X]_0=[X]+kt[/tex]
So we plug in to obtain:
[tex][X]_0=0.096M+3.6x10^{-5}\frac{M}{s}*30.min*\frac{60s}{1min}[/tex]
[tex][X]_0=0.16M[/tex]
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