Answer:
[tex][SO_2Cl_2]=0.0175M[/tex]
Explanation:
Hello!
In this case, considering that the decomposition reaction of SO2Cl2 is first-order, we can write the rate law shown below:
[tex]r=-k[SO_2Cl_2][/tex]
We also consider that the integrated rate law has been already reported as:
[tex][SO_2Cl_2]=[SO_2Cl_2]_0exp(-kt)[/tex]
Thus, by plugging in the initial concentration, rate constant and elapsed time we obtain:
[tex][SO_2Cl_2]=0.0225Mexp(-2.90x10^{-4}s^{-1}*865s)[/tex]
[tex][SO_2Cl_2]=0.0175M[/tex]
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