Answer: 3.72 M
Explanation:
Expression for rate law for first order kinetics is given by:
[tex]t=\frac{2.303}{k}\log\frac{a}{a-x}[/tex]
where,
k = rate constant = [tex]3.66\times 10^{-3}s^{-1}[/tex]
t = age of sample = 15.0 minutes
a = let initial amount of the reactant = 10.0 M
a - x = amount left after decay process = ?
[tex]15.0\times 60s=\frac{2.303}{3.66\times 10^{-3}}\log\frac{10.0}{(a-x)}[/tex]
[tex]\log\frac{100}{(a-x)}=1.43[/tex]
[tex]\frac{100}{(a-x)}=26.9[/tex]
[tex](a-x)=3.72M[/tex]
The concentration of [tex]H_2O_2[/tex] in a solution after 15.0 minutes have passed is 3.72 M
