Question

In which of the following equilibrium reactions the equilibrium would shift to the right, if total pressure is increased?

• A. $N_2\left(g\right)$ + $3H_2\left(g\right)$ $\rightleftharpoons$ $2N{H}_3\left(g\right)$
• B. $H_2\left(g\right)$ + $I_2\left(g\right)$ $\rightleftharpoons$ $2HI\left(g\right)$
• C. $H_2\left(g\right)$ + $C{l}_2\left(g\right)$ $\rightleftharpoons$ $2HCl\left(l\right)$
• D. $N_2{O}_4\left(s\right)$ $\rightleftharpoons$ $2NO\left(g\right)$

Answer 1

The correct option is A $N_2\left(g\right)$ + $3H_2\left(g\right)$ $\rightleftharpoons$ $2N{H}_3\left(g\right)$

According to Le-Chatelier principle if any change happen in any component then the equilibirium is going to shift that direction where this change can be neutralize.
When we increased the pressure the equilibirium will shift in that direction where the number of atoms are less so only reaction one there is less number of atoms so in reaction one it will go forward directon upon increasing the pressure.