Respuesta :
Answer:
The rate constant of the reaction is [tex]1.0185\times 10^{-2} dm^3/ mol s[/tex].
[tex]1.31\times 10^3 s[/tex] is the half life of the reactant.
Explanation:
A+B → P
Integrated rate law for second order kinetics is given by:
[tex]\frac{1}{A}=kt+\frac{1}{A_0}[/tex]
A = concentration left after time t = [tex]0.02 mol /dm^3[/tex]
[tex]A_o[/tex] = Initial concentration = [tex]0.075 mol /dm^3[/tex]
t = 1 hour = 3600 seconds
[tex]\frac{1}{0.02 mol /dm^3}=k\times 3600 s+\frac{1}{0.075 mol /dm^3}[/tex]
[tex]k=\frac{1}{3600 s}\times (\frac{1}{0.02 mol /dm^3}-\frac{1}{0.075 mol /dm^3)}[/tex]
[tex]k = 1.0185\times 10^{-2} dm^3/ mol s[/tex]
Half life for second order kinetics is given by:
[tex]t_{\frac{1}{2}}=\frac{1}{k\times a_0}[/tex]
[tex]t_{\frac{1}{2}}=\frac{1}{1.0185\times 10^{-2} dm^3/ mol s\times 0.075 mol /dm^3}=1.31\times 10^3 s[/tex]
The rate constant of the reaction is [tex]1.0185\times 10^{-2} dm^3/ mol s[/tex].
[tex]1.31\times 10^3 s[/tex] is the half life of the reactant.
