Question

In a closed system, how will an increase in pressure affect the following reaction: N2O4(g) ⇌ 2NO2(g)?

Answer 1

Step-by-step explanation:

According to Le Chatelier's principle, any change in an equilibrium reaction will shift the equilibrium in the direction that will be opposing the change.

For example, in the reaction
`N_(2)O_(4)(g) \rightleftharpoons 2NO_(2)(g)`, when we increase the pressure.

Then there will occur a decrease in volume of the reaction mixture. Due to this there will be increase in number of moles per unit volume.

Hence, equilibrium will shift in a direction where there are less number of moles. This means that the reaction will shift in the backward direction.

Thus, we can conclude that concentration of
`N_(2)O_(4)` will increase as a result more dinitrogen tetraoxide will be formed.