To determine the relationship between reactants and products at equilibrium for the given reaction:
[tex]\[ H_2(g) + I_2(g) \rightleftharpoons 2 HI(g) \][/tex]
We need to consider the value of the equilibrium constant, [tex]\( K \)[/tex].
1. Understanding the Equilibrium Constant (K):
The equilibrium constant, [tex]\( K \)[/tex], quantifies the ratio of the concentrations of products to reactants at equilibrium. It is expressed as:
[tex]\[ K = \frac{[HI]^2}{[H_2][I_2]} \][/tex]
where [tex]\([HI]\)[/tex], [tex]\([H_2]\)[/tex], and [tex]\([I_2]\)[/tex] represent the concentrations of hydrogen iodide, hydrogen, and iodine, respectively, at equilibrium.
2. Interpreting the Value of [tex]\( K \)[/tex]:
For this reaction, [tex]\( K \)[/tex] is given as:
[tex]\[ K = 5.0 \times 10^{-9} \][/tex]
This is a very small number, much less than 1.
3. Relationship between Reactants and Products:
- When [tex]\( K \)[/tex] is much less than 1, it indicates that the concentrations of reactants are much higher than the concentrations of products at equilibrium.
- This means that the reaction favors the formation of reactants over products.
4. Conclusion:
Since [tex]\( K = 5.0 \times 10^{-9} \)[/tex] is significantly less than 1, the reaction strongly favors the reactants at equilibrium.
Hence, the appropriate relationship between reactants and products at equilibrium for the given reaction is:
The reaction strongly favors the reactants.
