Question

Given $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$. 5 moles of each of $N_2$ and $H_2$ are heated in 1 $d{m}^3$ container. At equilibrium $60\%$ of $H_2$ is converted to ammonia. The total number of moles of the reactants and products in the equilibrium mixture is:

• A. 6
• B. 8
• C. 10
• D. 12

Answer 1

The correct option is B 8

$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$
Initial conc in mol 5 5 0
At equilibrium
1. No. of moles reacted 1 3
2. No. of moles formed 2
3. No. of moles remaining (5-1)=4 (5-3)=2
Hence total no. of moles = 4+2+2=8