2. CATALITIC REACTION ( 053.KK.06 ) INDUSTRIAL CHEMISTRY CLASS : XI SEMESTER : 3

3. The Equation reaction  The Equation reaction described about the reaction before the material is processed and the results with reactan products and limited shaft. A + B → P + Q In the above reaction, A and B are reactan while P and Q is a product.

4. Chemical reaction  Reaction is a chemical reaction between the chemical compound or chemical element that involves the change of molecular structure, which is generally associated with the formation of chemical bonds and dissolution. during the process has two possibilities that require energy (called the reaction endotermal) melepaskn or energy (reaction eksotermal).

5. Symptoms that accompany the chemical reaction  Forming deposition  Forming gas  The change color  The change in temperature

6. The reaction rate  The reaction rate is oxygen- concentration changes of substances involved in the reaction each time. Concentration expressed in mol / L while the time period stated in the second (mol / L.second)

7.  Substances involved in the reaction there are two classes, namely reactan, R and the product, P. In a reaction, reactants always decreases, while the products is always increasing.  The reaction rate can be defined as the reduced concentration reagent each time or increasing the concentration of the reaction each time. Teknologi dan Rekayasa

8. Reaction rate formula  Reaction: A + B → C + D A and B is reactan (R), C and D is the product (P), and the reaction rate is r, then: r = - [ΔR] / Δt = + [ΔP] / Δt

9. Relationships between the reaction rate coefficients and reaction  Rate of reaction have mol / L. second  Based on the rate of reaction is proportionate to the straight mol  Thus, comparison of the reaction coefficients represent comparison mol while the reaction rate comparison

10. Exercise Reaction: 1A + 3B → 2 C + 4D Firstly the concentration of A is 0.2 mol / L, after 10 seconds was a concentration of 0.1 live mol / L. Determine the reaction rate of A, to B, to C, and D against

11. Factors affecting reaction rate  Temperature  Concentration  Surface area  Catalyst

12. Reaction and collision theory  This theory states that the atom-atom, molecule-molecule, or ion-ion as particles always move randomly with a certain speed in accordance with the energy kinetiknya  If the two types of compound are mixed, then there will be a collision between two particles so that the compound reaction occurs.  Collision will produce a reaction, when the energy level reached kinetiknya called the activation energy and collision position accordingly.

13. Activation energy  Is the minimum energy that must be owned by a particle that produces a collision reaction Activation energy for endoterm and exoterm reaction can be described as follows

14. The influence of temperature on reaction rate  The higher the temperature, the energy particles kinetik the rise, more and more particles reach the activation energy, so that the more a reaction to occur  The higher the temperature, the reaction takes place faster  The research shows that every increase in temperature of 10 OC the reaction rate increased 2-3 fold

15. The relationship between temperature and reaction rate  r = r0. (2) ΔT/10 T = T0. (½) ΔT/10 Description: r = reaction rate is now r0 = reaction rate in the first ΔT = temperature increase t = time now T0 = time in the first

16. The influence of concentration on reaction rate  Concentration increased density means the particles so that the greater the chance of collision occurs  The more collision occurs, the reaction occurs more  The reactions take place faster if the concentration of the larger reagent

17. Relationship between concentration and reaction rate  Relationships between concentration and reaction rate can be expressed with the following equation: pA (aq) + qB (aq) → rC (aq) + sD (aq)  r = k (A) m (B) n  m and n is reaction order, the value depending on the experiment results, not depending on the reaction coefficients

18. Phases of reaction  In general, a reaction takes place gradually, there is a two-phase, three phase, or multiple stages.  Phase-phase reactions are fast, some are slow  Rate is determined by the reaction of the slow reaction

19. The influence of catalyst  Catalyst material is a solid, liquid, gas in the presence of a reaction can accelerate the reaction.  A reaction without the catalyst may be completed after the long hours, many days, even many years.  With the addition of a catalyst, the reaction can take place only a few minutes, even a few seconds only.

20. Attributes catalyst  Catalyst is physically not reactan  The molecular, catalyst participate in a reaction, but at the end of the reaction form again  Catalyst can only accelerate the reaction, but can not be initiated reaction

21. How it works catalyst  Catalyst follow a reaction to react so that the stages become more  Cause increased phase reaction activation energy is reduced  Decreasing the activation energy causes the particles to reach the activation energy increases, so the sooner the reaction  At the end of the reaction, catalyst re- form

22. Reaction mechanism with the catalyst  Reaction A + B → D would be done by using C as the catalyst.  Reaction mechanism that occurs is: A + C → AC (1) B + AC → ABC (2) ABC → CD (3) CD → C + D (4) A + B → D (total)

23. Activation energy  Collision reaction will result if the particles collide with enough energy to start a reaction. minimum energy required is called the reaction activation energy.  We can describe the state of activation energy in the Maxwell- Boltzmann distribution like this:

24. Activation energy  Collision-collision reaction will result if the particles collide with enough energy to start a reaction. minimum energy required is called the reaction activation energy. We can describe the state of activation energy in the Maxwell-Boltzmann distribution like this:

25. Activation energy  Only particles that are in the area on the right side of the activation energy will reaction when they collide. Most of the particles do not have enough energy and does not produce a reaction.

26. Catalyst and activation energy  To increase the reaction rate we need to increase the number of the collision work.  One alternative way to created is to lower the activation energy.  Adding a catalyst to give change which means that the activation energy.

27.  Catalyst provides an alternative route for a reaction.  This alternative route has a lower activation energy.  The diagram below is a description of the energy. Teknologi dan Rekayasa

28. Catalyst and activation energy  Catalyst only affects the rate of achievement equilibrium, not the position of equilibrium (for example: reverse reaction). Catalyst is not possible shock result of a reaction and the equilibrium concentration mass or after the reaction is complete with the same concentration or mass reaction to take place before

29. Catalyst and reaction temperature  Catalyst can lower the activation energy so the reaction is faster  Because of decrease in activation energy, the only reaction that can take place spontaneously at high temperature, can even at lower temperatures or even room temperature

30. Catalyst and the chemical equilibrium  Catalyst basically can only accelerate the reaction but the reaction can not  Catalyst does not work on the reactions that have been in balance  Only a catalyst to accelerate the reaction to the left and right  Catalyst at the beginning of the reaction equilibrium will accelerate the achievement of balance

31. Classification catalyst  Based on phase, catalytic devide two, namely: (1) homogeneous catalysts: phase catalytic reaction with the mixture and (2) heterogeneous catalysts: catalytic phase is not equal to the reaction mixture, generally a solid  Heterogeneous catalyst (solid) is preferred because the process of separation of catalyst and the results of the reaction is easier to do

32. Homogeneous and heterogeneous catalyst

33. Heterogeneous catalyst  A solid catalyst consisting of 3 main components, namely (1) active phase, serves to accelerate and direct reactions, (2) buffer, to provide broad work surface for a larger active phase, and (3) promoter, working to improve catalytic performance.  Active phase of the catalyst can not be active because of some reason such as the presence of CO, CO2, and sulfur compound- compound and the operating temperature is too high.

34. Various catalyst  In the human body and animals, each phase reaction always requires a catalyst  Catalyst in a reaction called biokatalisator body metabolism, and the role performed by this enzyme  Enzyme is actually the protein that have specific functions as a specific reaction to certain biokatalisator  Reaction chemistry of slow progress that requires a catalyst, good reaction and inorganic reactions involving carbon compound

35. Transition element as a catalyst 1.Making Ammonia using Ni or Fe catalyst 2.Acid sulphate of making contact with the process using a catalyst V2O5 3.Reaction hidrogenasi oil in the making of margarine using Ni catalyst 4.MnO2 or stone can accelerate the dissociation kawi H2O2 into H2O and O2

36. The other catalyst  Esterification hydrolysis reaction and requires a strong catalyst acid sulphate  Primary alcohol oxidation reactions using K2Cr2O7 require acid sulphate catalyst  Substitution reaction requires a alkane catalyst  Burning fuel requires a catalyst or Pt TEL  Making biodiesel with the H2SO4 and KOH catalyst  Making VCO with pure VCO catalyst

37. Biodiesel Industry  Biodiesel is a simple chemical compound with the contents of six to seven types of fatty acid ester. Biodiesel is defined as metyl ester with carbon chain length of between 12 and 20 of fatty acid derived from vegetable oils such lipid or animal fat.

38.  Vegetable oil or animal fat can be made with the biodiesel reaction trans esterification with alcohol use. Composition and chemical nature of biodiesel depends on the purity, long short, degree of saturation, and the structure of alkyl chain fatty acid Teknologi dan Rekayasa

39.  Biodiesel is an alternative Renewable sources fuel, with the fatty acid ester composition of vegetable oils include: palm oil, coconut oil, castor oil fence, oil kapok seed, and there is still more than 30 kinds of plants of a potential made for biodiesel Teknologi dan Rekayasa

40. Trans esterification catalytic Reaction to making biodiesel  Biodiesel is made through a chemical process called trans esterification. This process produces two products, namely metal esters (biodiesel) / mono-alkyl esters and glycerin, which is the product side.  Raw materials for the main biodiesel, among other vegetable oils, animal fat, used fat / fat recycling. Meanwhile, as the raw material was the alcohol  Catalyst is also required to improve solubility in the reaction time progresses, the catalyst generally used is the strong alkali NaOH or KOH or sodium metoksida.

41. Flow chart making biodiesel with the trans esterification reaction

42. Trans esterification catalytic reaction