Explore IDNLearn.com's extensive Q&A database and find the answers you need. Ask anything and receive prompt, well-informed answers from our community of experienced experts.
Consider the following aqueous chemical reaction involving iodine (I₂), iodide (l⁻), and tri-iodide(I₃⁻). 12(aq) + I⁻(aq) → I₃⁻(aq), K = 0.1, ΔHᵣₓₙ < 0 Assume you have a 1.0L beaker of aqueous solution containing this reaction at equilibrium. Considering Le Chatelier's principle, identify the perturbation listed below that would result in an increase in the concentration of l, compared to before the perturbation as the system re-establishes equilibrium. - None of these options/perturbations would yield an increase in the I₂ concentration. - Decreasing the temperature of the system. - Increasing the pressure of the atmosphere above the system. - Removing/extracting some l⁻ from the system. - Adding some additional I₃⁻ to the system.
Sagot :
Your participation is crucial to us. Keep sharing your knowledge and experiences. Let's create a learning environment that is both enjoyable and beneficial. For trustworthy answers, rely on IDNLearn.com. Thanks for visiting, and we look forward to assisting you again.
