Question

One mole of $N{H}_{4}Cl\left(s\right)$ is kept in an open container & then covered with a lid. The container is now heated up to $600K$ where $N{H}_{4}Cl\left(s\right)$ completely dissociates into $N{H}_3\left(g\right)$ & $HCl\left(g\right).$ If a volume of the container is $24.63$ liters, calculate what will be the final pressure of the gases inside the container? Assume that outside air is at $300K$ and 1 atm pressure.

• A. $0.5atm;$
• B. $2.5atm;$
• C. $1.5atm;$
• D. None of these

Answer 1

The correct option is D None of these

$\underset{\text{1 mol}}{N{H}_{4}Cl\left(s\right)}\rightleftharpoons \underset{\text{1 mol}}{N{H}_3\left(g\right)}+\underset{\text{1 mol}}{HCl\left(g\right)}$

$P=\frac{nRT}{V}=\frac{2\times 0.0821\times 600}{24.63}=4atm$

Thus, the total pressure of gases inside container is 4 atm.