As always… OWL Lon-Capa assignments Lecture videos Textbook HW: equilibrium (due Monday) Quiz: Mon-Wed next week Lecture videos Textbook Read Do text homework

Exam I Thursday, September 26, 7:00-9:00 pm; rooms are on the website. Conflict: (9/26) 4:30-6:30pm in 140 Burrill; sign up in 1026 CA (starting 9/19) Conflict with conflict? Email me right away. Review sessions: Sunday (9/22): 165 Noyes Lab (4-6 pm) Monday (9/23): 1024 Chemistry Annex (6-8 pm)

Exam I Practice exam will be posted after lecture. Take when you feel ready for the exam. Take as an actual exam (not just more practice problems). See the front of the exam for information that you are given and the number of problems.

Heterogeneous Equilibria

K is a Constant (at given T)

Clicker Question Dinitrogen pentoxide is added to an evacuated rigid container at 25°C. The initial pressure is 1.000 atm. The N2O5 decomposes according to the equation 2N2O5 (g) 4NO2 (g) + O2(g)   At equilibrium the total pressure is determined to be 1.423 atm. Determine Kp for the reaction. a) 2.77 x 10-2 b) 2.93 x 10-2 c) 7.55 x 10-5 d) 0.111 e) 0.141

Chapter 6: Challenge Problem/OWL 100. Suppose 1.50 atm of CH4(g), 2.50 atm of C2H6(g), and 15.00 atm of O2(g) are placed in a flask at a given temperature. The reactions are: CH4(g) + 2O2(g) CO2(g) + 2H2O(g) Kp = 1.0 x 104 2C2H6(g) + 7O2(g) 4CO2(g) + 6H2O(g) Kp = 1.0 x 108 Calculate the equilibrium pressures of all gases. Things we know: 1. Stoichiometry works! 2. All reactants and products coexist in the flask. 3. The equilibrium constant values are constant (the ratios of products to reactants are known and constant). 4. The amount of O2 = the amount of O2 (same with CO2 and H2O).