Part 2: Thinking like a Chemist 2. Part of thinking like a chemist is being able to visualize processes that cannot be d

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Part 2 Thinking Like A Chemist 2 Part Of Thinking Like A Chemist Is Being Able To Visualize Processes That Cannot Be D 1 (54.73 KiB) Viewed 11 times

Part 2: Thinking like a Chemist 2. Part of thinking like a chemist is being able to visualize processes that cannot be directly observed by our eyes. a. Describe in your own words what is happening on the molecular level as the copper(II) chloride solid dissolves in the water, and as the water from the hydrate dissolves in the water. Is this even possible? Food for Thought: What does the term "dissolving" mean anyway? Is the dissolving process different for an ionic compound versus a covalent compound? b. Type the balanced chemical equation for the chemical reaction in this experiment (remember, an equation is a symbolic representation of the chemical process on the molecular and atomic level). The reactants and products are given in a word description below. Include phase labels for each reactant and product. Aluminum metal reacts with aqueous CuCl, 2H₂O to form copper metal, aqueous aluminum chloride and water. c. Dissolved copper (II) chloride dihydrate will impart a light blue color to the solution due to the presence of the hydrated Cu²+ ion. Dissolved AICI, is colorless in aqueous solution. This knowledge can lead to the discovery of which reactant is the limiting and which is in excess. In the video, there were physical observations that would lead you to identify the limiting and excess reactant. With careful observation of the final solution, a slight blue color can be seen. This would indicate the hydrate was in excess. With this in mind, how would the final reaction mixture appear if the aluminum was in excess? Explain your answer.