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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.

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