Question

Consider the following reaction equilibrium $N_{2\left(g\right)}+3H_{2\left(g\right)}\rightleftharpoons 2N{H}_{3\left(g\right)}$. Initially, $1mol$ of $N_2$ and $3mol$ of $H_2$ are taken in a $2$ litre flask. At equilibrium state if the number of mol of $N_2$ is $0.6$ what is the total number mol of $N_2$ is $0.6$ what is the total number mol of all gases present in the flask.

• A. $0.8$
• B. $1.6$
• C. $2.8$
• D. $3.2$

Answer 1

The correct option is D $3.2$

$N_2+3H_2\rightleftharpoons 2N{H}_3$

$t=0$ 1 3

$tx{g}^m$ 0.t. 1.8. 0.8

$\therefore$ total moles = 3.2