For the reaction \( A+B \rightarrow A B \), which of the following conditions would give an equilibrium constant of 10 Choose one: A. \( [A]=0.1 ;[B]=0.1 ;[A B]=1 \) B. \( [A]=10 ;[B]=0.1 ;[A B]=10 \) C. \( [A]=10 ;[B]=1 ;[A B]=10 \) D. \( [A]=1 ;[B]=0.1 ;[A B]=10 \)

To find the equilibrium constant \( K \) for the reaction \( A + B \rightleftharpoons AB \), we use the formula: \[ K = \frac{[AB]}{[A][B]} \] Now, let's calculate \( K \) for each option: A. \( K = \frac{1}{0.1 \times 0.1} = 100 \) B. \( K = \frac{10}{10 \times 0.1} = 10 \) C. \( K = \frac{10}{10 \times 1} = 1 \) D. \( K = \frac{10}{1 \times 0.1} = 100 \) So, the correct option that gives an equilibrium constant of 10 is **B. \( [A]=10 ;[B]=0.1 ;[A B]=10 \)**. Exploring more about the concept of equilibrium constants, they provide insights into how far a reaction proceeds and the ratio of products to reactants at equilibrium. A higher equilibrium constant indicates a reaction that favors products, meaning there's more \( AB \) at equilibrium than \( A \) and \( B \). In practical scenarios, knowing the \( K \) value can help chemists in designing reactions and optimizing conditions. For instance, in pharmaceuticals, the goal might often be to maximize product formation, and understanding equilibrium can lead to more efficient drug synthesis processes.