Question

In which of the following system, doubling the volume of the container cause a shift to the right?

• A. $H_{2\left(g\right)}+C{l}_{2\left(g\right)}\rightleftharpoons 2HC{l}_{\left(g\right)}$
• B. $2C{O}_{\left(g\right)}+O_{2\left(g\right)}\rightleftharpoons 2C{O}_{2\left(g\right)}$
• C. $N_{2\left(g\right)}+3H_{2\left(g\right)}\rightleftharpoons 2N{H}_{3\left(g\right)}$
• D. $PC{l}_{5\left(g\right)}\rightleftharpoons PC{l}_{3\left(g\right)}+C{l}_{2\left(g\right)}$

Answer 1

The correct option is D $PC{l}_{5\left(g\right)}\rightleftharpoons PC{l}_{3\left(g\right)}+C{l}_{2\left(g\right)}$

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.
Increase(doubling) in volume, i.e., decrease in pressure shifts the equilibrium in the direction in which number of moles increases. option 'd' is the only case where number of mole is increasing. hence it is correct.