The correct interpretation of the equation below is:
Fe3+(aq) + SCN–(aq) --> and <-- FeSCN2+(aq)
A. A heterogeneous equilibrium exists because of the charged ions.
B. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.
C. The equilibrium constant is Kc = [Fe3+][SCN–]/[FeSCN2+]
D. The reaction is incomplete because the product is still charged.
E. None of these.
Is the problem written as you have it posted or is it written as
Fe3 + SCN^- <-->FeSCN^+2 (with aq after each of course)
At any rate, I think the answer is B.
Check them out. A heterogeneous equilibrium is one in which there are two phases. Here all are the same phase; i.e., in solution.
B. that is a true statement.
C. The equilibrium constant for the reaction is the reciprocal of that shown.
D. Many reactions carry a charge. Of course the charges must balance with the same number on the product side as the reactant side.
Sorry, it is <-->, there was an error when I typed up the problem. Thank you for your help!
C. The correct interpretation of the equation above is that the equilibrium constant is Kc = [Fe3+][SCN–]/[FeSCN2+]. This means that at equilibrium, the concentrations of the reactants and products are related by this equilibrium constant.
To determine the correct interpretation of the given equation, we need to analyze the information provided.
First, let's understand the notation used in the equation:
- Fe3+(aq) represents iron(III) ions in aqueous solution (meaning they are dissolved in water).
- SCN–(aq) represents thiocyanate ions in aqueous solution.
- FeSCN2+(aq) represents the complex ion formed by the combination of iron(III) ions and thiocyanate ions.
Now, let's evaluate each option:
A. A heterogeneous equilibrium exists because of the charged ions.
A heterogeneous equilibrium involves species that are in different phases. In this equation, all the species are in the aqueous phase, so there is no presence of different phases. Therefore, option A is incorrect.
B. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.
This option refers to a state of dynamic equilibrium, where the reaction is still occurring but the rates of the forward and reverse reactions are equal. Since the equation includes a double arrow (indicating a reversible reaction), this option seems plausible. However, further analysis is required.
C. The equilibrium constant is Kc = [Fe3+][SCN–]/[FeSCN2+]
The equilibrium constant (Kc) is a value that quantitatively describes the ratio of products to reactants at equilibrium. It is determined by the concentrations of the species involved in the reaction. The given equation does represent the equilibrium constant expression, where the concentrations of Fe3+, SCN–, and FeSCN2+ are considered. This expression suggests that option C could be the correct interpretation.
D. The reaction is incomplete because the product is still charged.
This option suggests that the presence of charged species indicates an incomplete reaction. However, the charges of the ions alone do not determine the completeness of the reaction. Additionally, the equation implies the formation of a complex ion (FeSCN2+), which can indeed be charged. Therefore, option D is not the correct interpretation.
E. None of these.
This option would be the correct answer if none of the other options accurately interpret the given equation. However, we should thoroughly evaluate the other options before concluding.
Considering the evaluation so far, option B suggests that the reaction is at equilibrium, while option C provides the correct equilibrium constant expression.
To make a final selection, we need to understand the equilibrium conditions in detail. If a reaction is at equilibrium, the concentration of each species remains constant over time. In the given equation, the presence of a double arrow indicates that the reaction is reversible. Thus, the correct interpretation is:
B. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.
To summarize, the correct interpretation of the equation is that at equilibrium, the forward and reverse reactions occur at the same rate.