Question

Diazonium salt decomposes as
$C_6{H}_5{N}_2^{\oplus }C{l}^{\ominus }\to C_6{H}_{5}Cl+N_2$
At $0^0$C, the evolution of $N_2$ becomes two times faster when the initial concentration of the salt is doubled. Thus, it is :

• A. A first order reaction
• B. A second order reaction
• C. Independent of the initial concentration of reactant
• D. A zero order reaction

Answer 1

The correct option is A A first order reaction

$r_1=k[salt{]}^n$
$r_2=2r_1=k[2salt{]}^n$
$\frac{2r_1}{r_1}=(2{)}^n$
$(2{)}^1=(2{)}^n$
n = 1.