Consider the following initial conditions of a Chemical Reaction.
Initial Conditions for reaction A <---> B
Initial Amount of A = 5.99 moles
Initial Amount of B = 2.15 moles
Forward Rate (A --> B) = 0.95 moles/second
Reverse Rate (B --> A) = 0.95 moles/second
Which of the following is true about this Chemical reaction?
This chemical reaction is at equilibrium.
This chemical reaction is not at equilibrium.
There is no way to determine if this chemical reaction is at equilibrium based on the information given.
The chemical reaction is at equilibrium, but will not be at equilibrium after 30 seconds.
The reaction is at equilibrium because the rate of forward reaction = rate of reverse reaction
The correct statement is: This chemical reaction is at equilibrium.
Explanation:
Since the forward and reverse rates are equal (0.95 moles/second), the reaction is in a state of dynamic equilibrium. At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. Therefore, the given conditions indicate that the reaction has reached equilibrium.
To determine if this chemical reaction is at equilibrium, we need to compare the rate of the forward reaction (A --> B) with the rate of the reverse reaction (B --> A).
In this case, the forward rate is given as 0.95 moles/second and the reverse rate is also given as 0.95 moles/second. Since the rates of the forward and reverse reactions are equal, it indicates that the reaction is occurring in both directions at the same rate.
When the rates of the forward and reverse reactions are the same, it means that the concentrations of the reactants and products are stable and not changing over time. This is a characteristic of a system at equilibrium.
Therefore, based on the given information, we can conclude that this chemical reaction is at equilibrium.
The correct answer is: This chemical reaction is at equilibrium.