{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

CH 118 lechateliers equilibrium - exothermic reactions...

Info icon This preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
CH 118 Chemical Equilibrium and LeChatelier’s Principle I. Color of Complex Ions Pink -> [Co(H 2 O) 6 ] 2+ Blue -> [CoCl 4 ] 2- Blue -> [Cu(H 2 O) 6 ] 2+ Blue -> [Cu(NH 3 )4(H 2 O) 2 ] 2+ Blue -> Cu(OH) 2 Blue -> [CuBr 4 ] 2- II. Addition of Water Water is not included in the equilibrium constant expression because the concentration of it cannot change as the reaction occurs. However, adding water can decrease the concentration of the reactant and cause a shift towards the left. For example, the addition of water to CuBr 2 caused the color to go from green to blue. Also, the reaction between [Co(H 2 O) 6 ] 2+ and HCl was blue (product favored), but when water was added it turned purple (shifting left and almost at equilibrium). III. Temperature Dependence of K The value of K can be different for the same reaction at different temperatures. For example,
Image of page 1

Info icon This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: exothermic reactions favor the products. Also, reactions can occur faster at higher temperatures than lower temperatures. Therefore, it is important to note the temperature for each K value. Test tube #1 was purple (K = 1) at room temperature, blue (K >> 1) at 100 C, and pink (K <<1) at 0 o C. Test tubes #2, 3, and 4 all remained pink (K << 1) at all three temperatures. IV. Gibbs Free Energy Exercise The relationship between Gibbs free energy and equilibrium constant is ∆G = -RT ln K If K is much greater than 1, then ∆G is negative, indicating a product-favored reaction. If K is much less than 1, then ∆G is positive, indicating a reactant-favored reaction....
View Full Document

{[ snackBarMessage ]}

What students are saying

  • Left Quote Icon

    As a current student on this bumpy collegiate pathway, I stumbled upon Course Hero, where I can find study resources for nearly all my courses, get online help from tutors 24/7, and even share my old projects, papers, and lecture notes with other students.

    Student Picture

    Kiran Temple University Fox School of Business ‘17, Course Hero Intern

  • Left Quote Icon

    I cannot even describe how much Course Hero helped me this summer. It’s truly become something I can always rely on and help me. In the end, I was not only able to survive summer classes, but I was able to thrive thanks to Course Hero.

    Student Picture

    Dana University of Pennsylvania ‘17, Course Hero Intern

  • Left Quote Icon

    The ability to access any university’s resources through Course Hero proved invaluable in my case. I was behind on Tulane coursework and actually used UCLA’s materials to help me move forward and get everything together on time.

    Student Picture

    Jill Tulane University ‘16, Course Hero Intern