The chemical reaction N2(g)+ 3H2(g)<-->

2NH3(g) is at equilibrium. An expirimenter increases the volume of the reaction chamber by 10%. Explain what happens to bith the forward and reverse reaction rates from the moment the volume is changed until equilibrium is reestablished.

That reduces the pressure, so favors reverse reaction.

So does that mean that the reverse reaction rate increases until equilibrium is reestablished? Would that also mean that the forward reaction rate decreases?

Not necessarily, however, remember that in this case the reverse reaction is
rate = k(NH3) so as the (NH3) decreases the rate will decrease with time.

dasdas

When the volume of the reaction chamber is increased by 10%, the pressure inside the chamber decreases. According to Le Chatelier's principle, changes in pressure can affect the equilibrium of a reaction. In this case, decreasing the pressure favors the reverse reaction.

As a result, the reverse reaction rate increases from the moment the volume is changed until equilibrium is reestablished. This means that more N2 and H2 will react to form NH3 molecules.

On the other hand, the forward reaction rate may initially decrease due to the decrease in pressure. However, it does not necessarily continue to decrease until equilibrium is reestablished. The rate of the forward reaction is determined by the concentration of N2 and H2, which are not directly affected by the change in volume. Therefore, the forward reaction rate may decrease temporarily but eventually stabilizes.

It's important to note that the change in reaction rates is a dynamic process. The forward and reverse reactions are continuously happening, even when the reaction is at equilibrium. When a change is introduced, the rates adjust until a new equilibrium is reached.