Benzene diazonium chloride in aqueous solution decomposes according to the equation C^(6)H^(5)N^(2)Cl rarr C_(6)H_(5)Cl+N_(2) Starting with an initial concentration of 10 g L^(-1), the volume of N_(2) gas obtained at 50^(@)C at different intervals of time was found to be as under : {:("t (min)":,6,12,18,24,30,oo),("Vol. of "N_(2) (ml):,19.3,32.6,41.3,46.5,50.4,58.3):} Show that the above reaction follows the first order kinetic. What is the value of the rate constant ?

Benzene diazonium chloride in aqueous solution decomposes according to

1.	Benzene diazonium chloride in aqueous solution decomposes according to the equation C^(6)H^(5)N^(2)Cl rarr C_(6)H_(5)Cl+N_(2) Starting with an initial concentration of 10 g L^(-1), the volume of N_(2) gas obtained at 50^(@)C at different intervals of time was found to be as under : {:("t (min)":,6,12,18,24,30,oo),("Vol. of "N_(2) (ml):,19.3,32.6,41.3,46.5,50.4,58.3):} Show that the above reaction follows the first order kinetic. What is the value of the rate constant ?
Answer» Solution :For a FIRST order REACTION `k=(2.303)/(t)"log"([A_(0)])/([A])` `k=(2.303)/(t)"log"(V_(oo))/(V_(oo)-V_(1))` In the PRESENT case, `V_(oo) = 58.3 ml`. The value of k at different time can be calculated as FOLLOWS.