The reaction below is at dynamic equilibrium.
[tex]$N_2(g)+3 H_2(g) \longleftrightarrow 2 NH_3(g)$[/tex]
Which statement is true for the equilibrium system?
A. The concentration of [tex]$NH _3$[/tex] is greater than the concentration of [tex]$N _2$[/tex].
B. The rate of the forward reaction equals the rate of the reverse reaction.
C. The rate of the forward reaction is greater than the rate of the reverse reaction.
Answer (2)
Dynamic equilibrium means the forward and reverse reaction rates are equal.
Concentrations of reactants and products are constant, but not necessarily equal.
The statement 'The rate of the forward reaction equals the rate of the reverse reaction' is true.
Therefore, the correct answer is that the rate of the forward reaction equals the rate of the reverse reaction. The rate of the forward reaction equals the rate of the reverse reaction.
Explanation
Understanding Dynamic Equilibrium The reaction N 2 ( g ) + 3 H 2 ( g ) ⇌ 2 N H 3 ( g ) is at dynamic equilibrium. This means the rate of the forward reaction (formation of N H 3 ) is equal to the rate of the reverse reaction (decomposition of N H 3 ). The concentrations of the reactants ( N 2 and H 2 ) and the product ( N H 3 ) are constant at equilibrium, but not necessarily equal.
Analyzing the Statements Let's analyze each statement:
Statement 1: The concentration of N H 3 is greater than the concentration of N 2 . This is not necessarily true. The equilibrium concentrations depend on the equilibrium constant K and the initial concentrations of the reactants and products. It's possible for the concentration of N 2 to be greater than N H 3 , or vice versa.
Statement 2: The rate of the forward reaction equals the rate of the reverse reaction. This is the very definition of dynamic equilibrium, so this statement is true.
Statement 3: The rate of the forward reaction is greater than the rate of the reverse reaction. This is false. At equilibrium, the rates are equal.
Conclusion Therefore, the correct statement is that the rate of the forward reaction equals the rate of the reverse reaction.
Examples
Dynamic equilibrium is crucial in many industrial processes, such as the Haber-Bosch process for ammonia synthesis. Understanding equilibrium helps optimize reaction conditions (temperature, pressure, and reactant ratios) to maximize product yield. For instance, controlling these factors allows manufacturers to produce ammonia efficiently, which is then used in fertilizers, ensuring sufficient food production for the population. By manipulating equilibrium, we can shift the reaction to favor the formation of the desired product, making the process economically viable.
At dynamic equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. Therefore, the correct statement among the provided options is B. This illustrates the balance in the concentrations of reactants and products during equilibrium.
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