The following data are for the decomposition of ammonium nitrate in aqueous solution Volume of N2 in cc Time (minutes) 6.25 10 9.50 15 11.42 20 13.65 25 The order of the reaction is

Question

The following data are for the decomposition of ammonium nitrate in aqueous solution Volume of N2 in cc Time (minutes) 6.25 10 9.50 15 11.42 20 13.65 25 The order of the reaction is (A) Zero (B) One (C) Two (D) Three

Tardigrade Admin · Accepted Answer

K=(2.303/t)log(V∞/V∞-Vt)gives constant value of K. With the given date. Hence it is 1st order.

Volume of $N_{2}$ in cc	Time (minutes)
$6.25$	$10$
$9.50$	$15$
$11.42$	$20$
$13.65$	$25$

Q. The following data are for the decomposition of ammonium nitrate in aqueous solution

Volume of $N_{2}$ in cc Time (minutes)

$6.25$ $10$

$9.50$ $15$

$11.42$ $20$

$13.65$ $25$

The order of the reaction is

Zero

One

Two

Three

$K = \frac{2.303}{t} l o g \frac{V _{\infty}}{V _{\infty} - V _{t}}$ gives constant value of $K .$ With the given date. Hence it is 1st order.

Q. The following data are for the decomposition of ammonium nitrate in aqueous solution Volume of N2​ in cc Time (minutes) 6.25 10 9.50 15 11.42 20 13.65 25 The order of the reaction is

Zero

One

Two

Three

K=t2.303​logV∞​−Vt​V∞​​gives constant value of K. With the given date. Hence it is 1st order.

Q. The following data are for the decomposition of ammonium nitrate in aqueous solution

Volume of $N_{2}$ in cc Time (minutes)

$6.25$ $10$

$9.50$ $15$

$11.42$ $20$

$13.65$ $25$

The order of the reaction is

$K = \frac{2.303}{t} l o g \frac{V _{\infty}}{V _{\infty} - V _{t}}$ gives constant value of $K .$ With the given date. Hence it is 1st order.