No2 and n2o4 undergo the reaction shown. when a sealed
container of no2 reaches chemical equilibrium, which must be true?
a) no n2o4 is present.
b) no chemical reactions are occurring.
c) the rates of the forward and reverse reactions are equal.
d) the maximum number of molecules has been reached.
NO₂ and N₂O₄ undergo the following equilibrium reaction:2NO₂(g) ⇄ N₂O₄(g)
That is a reversible reaction, i.e. there are two simultaneous reactions: the direct or forward reaction and the reverse reaction:Direct reaction: 2NO₂(g) → N₂O₄(g) Reverse reaction: 2NO₂(g) ← N₂O₄(g)
At the beginning, only NO₂(g) is in the sealed container. The NO₂ concentration is maximum, and the rate of the forward reaction is maximum.
As the reaction progresses, the concentration of NO₂ diminishes, and, consequently, the rate of the forward reaction decreases.
As soon as the N₂O₄ appears, the reverse reaction starts. At the beginning the rate is low, but as the N₂O₄ concentration increases the rate of the reverse reaction increases.
When both forward and reverse rates become equal the equilibrium has been reached. This is what is called a dynamical equilibrium.
Then, as per the choices, you have that, at equilibrium:
A) No N₂O₄ is present:False: as explained above, at equilibrium both NO₂ and N₂O₄ are present.
B) No chemical reactions are occurring.False: as explained above, at equilibrium both forward and reverse reaction are occurring at the same rate.
C) The rates of the forward and reverse reactions are equal.True: as explained, this is the meaning of dynamic equilibrium.
D) The maximum number of molecules has been reached.False: the number of molecules of each compound at equilibrium will be given by the constant of equiibrium, Keq = [N₂O₄] / [NO₂]², and this value varies with the temperature.
h The rates of the forward and reverse reaction are equal.
The reaction takes place in a closed container . So both the reactant (NO₂) and product N₂O₄ are present in the reaction container. Under such conditions, the reaction reaches chemical equilibrium. At chemical equilibrium the rates of the forward and reverse reactions are equal. The concentration of the reactants and products remain constant at Chemical Equilbrium.
Correct Option H. Rates of forward and reverse reactions are equal.
The reactant NO2 and product N2O4 are in equilibrium. One of the important criteria for the equilibrium system is that the rates of forward and backward reactions are same. Due to this, the rate at which reactant gets converted into product, at the same rate, products gets converted back into reactant. Thus, at any given time, there is always an effective concentration of both reactant and product in the reaction vessel
h let me think
the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .
container of no2 reaches chemical equil...