475

17 The experimental and calculated data are recorded in a table in the form: Time from the beginning of the experiment t , sec. (V‑n)/V 1/ t ln ((V‑n/V)) k 1 2 3 4 5 The following expression is obtained for the concentration of the reacting substance (hydrogen peroxide) at any time from the kinetic equation for the first order reaction: t k 1 −= ln 0 С С . The concentration ratio can be replaced by proportional quantities in the kinetic equation. In our experiment V n V С С − = 0 . This equation is used for obtaining a formula for calculating the rate constant: t k 1 −= ln V nV − . The value of the rate constant is calculated for the moment t 1  and the moment t 2 , etc. and put into the table. Then we find the average value of the rate constant corresponding to the temperature of the solutions during the experiment. LESSON 8. FINAL CONTROL № 1 Final control № 1 is conducted on the following topics: 1. Methods of expressing the concentration of solutions. 2. Acid-base titration: alkalimetry and acidimetry. 3. Buffer solutions. Buffer capacity 4. Colligative properties of solutions: the laws of Raul and Vant-Goff. 5. Heterogeneous equilibria and processes. 6. Fundamentals of chemical thermodynamics. Thermochemistry. Hess’s Law. Entropy. The free energy of Gibbs. 7. Chemical kinetics. Catalysis.