Question

Diazonium salt decomposes as
\[\ce{C6H5N{^+_2}Cl- -> C6H5Cl + N2}\]

At 0°C, the evolution of N₂ becomes two times faster when the initial concentration of the salt is doubled. Therefore it is ______.

Options

• a first order reaction

• a second order reaction

• independent of the initial cone, of the salt

• a zero order reaction

Answer 1

Diazonium salt decomposes as
\[\ce{C6H5N{^+_2}Cl- -> C6H5Cl + N2}\]

At 0°C, the evolution of N₂ becomes two times faster when the initial concentration of the salt is doubled. Therefore it is a first order reaction.

Explanation:

The given reaction is \[\ce{C6H5N{^+_2}Cl- -> C6H5Cl + N2}\]

It is given that when the initial concentration is doubled, the rate of nitrogen evolution also doubles.

This implies:

Rate ∝ \[\ce{[C6H5N{^+_2}Cl-]^{1}}\]

So, the reaction follows a first-order rate law.