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REACTION BALANCE

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  1. REACTION BALANCE LEVEL XII SEMESTER 2 SMKN 7 BANDUNG

  2. Isi dengan Judul Halaman Terkait

  3. PURPOSE OF STUDY 1.Explaining the balance reaction and balancing 2.Determing quantitative connection between reactor and the result of the reaction in counting Kc and Kp from a reaction 3.Determining the factors that influence balancing in a balancing reaction Isi dengan Judul Halaman Terkait

  4. REACTION BALANCE • Most of chemical reaction goes on two direction or reversible. • First, reaction goes to product with V1speed • After some products are formed, the turning back process start to begin to reactant with V2 speed. • If the speed of reaction goes forward and the turning back reaction is as big (V1=V2) Isi dengan Judul Halaman Terkait

  5. and reactant concentration and product do not change any more at the same time, so they will reach chemical balance, • such as water steaming proceeds. • For example : Isi dengan Judul Halaman Terkait

  6. The process of chemical balance between liquid and steam Isi dengan Judul Halaman Terkait

  7. BALANCE CONSTANTA • Generally if a substance A and substance B put into A closed flask in a steady temperature and pressure, it will form substance C and substance D • The Kcvalue : Isi dengan Judul Halaman Terkait

  8. BALANCE CONSTANTA, KC, • Defined as the result of multiplication from balance concentration (mol/Liter) from product (reaction substances) divided by multiplicative result of reactant (the rest of reactor) where each concentration raised to a power with coefficients balance similarity Isi dengan Judul Halaman Terkait

  9. Example of reaction; • Has Kc Value; • So that in desolation reaction formed a bigger product because of Kc>1 Isi dengan Judul Halaman Terkait

  10. Balance Constanta in the shape of partial pressure. Partial shape from gas is concentration size, so balance Constanta can be defined in partial pressure (Kp) • for example; Isi dengan Judul Halaman Terkait

  11. So the value of Kp is; • pNH3, pN2, and pH2 are each of partial pressure from NH3, N2 and H2 which is defined in atmosphere. Isi dengan Judul Halaman Terkait

  12. THE CONNECTION BETWEEN KC AND KP • Let us take a look the balance similarity below; • That similarity has the value; Isi dengan Judul Halaman Terkait

  13. And the Kp valve is; • From the similarity ideal gas; Isi dengan Judul Halaman Terkait

  14. Where the concentration Isi dengan Judul Halaman Terkait

  15. To substitute P/RT for n/v in Kc in similarity above gives connection between Kc and kp; • Or; IsidenganJudulHalamanTerkait

  16. Where Δn = (n products –n reactants) because Kc value refers to unit of mol/liter and Kp at atmosphere so the value of R defined in L.atm/mol.K • For the reaction where the number of product mol is the same as the number of reactant mol, so the value of Kc = Kp because the value of Δn = 0 Isi dengan Judul Halaman Terkait

  17. Homogeneous equilibrium term applied to reaction which all part is reacting stays at the same phase. • Example of from equilibrium of homogenous is reaction of ammonia forming, NH3, nitrogen, N2 (g) and oxygen, O2 (g); Isi dengan Judul Halaman Terkait

  18. with the price of Constanta its the equilibrium is Isi dengan Judul Halaman Terkait

  19. Example of equilibrium in system other homogenous is: Equilibrium in gas system the price of Constanta its the equilibrium is; Isi dengan Judul Halaman Terkait

  20. Reversible reaction entangling reactant and product which its the phase differs in yields heterogeneous equilibrium. • Its the example is reacting decomposition of Mercury oxide: Isi dengan Judul Halaman Terkait

  21. The equilibrium consisted of solid phase ( solid=s), dilution (liquid=l) and gas (g), hence for solid phase ( sulfur) and dilution in significant is not influenced by pressure change. • Hence the price of Kc and Kp to react upper is: Isi dengan Judul Halaman Terkait

  22. Some things which must be gave attention to equilibrium of heterogeneous which relates to statement of law of mass action is: • If matters which there is in equilibrium is in the form of solid and gas • packed into by equation of equilibrium only matters gasiform only, • because concentration of solid matter is permanent and its the value has counted in the price of Kc and Kp. IsidenganJudulHalamanTerkait

  23. If equilibrium between solid matters and condensation entered in calculation Kc only concentration of dissolving matters only, while Kp cannot expressed. • Example : Isi dengan Judul Halaman Terkait

  24. For equilibrium between matters in condensation if its the solvent pertained one of reactant or result of its the reaction hence concentration from the solvent is not packed into calculation Kc. • Example : Isi dengan Judul Halaman Terkait

  25. FACTOR INFLUENCING EQUILIBRIUM If an external pressure given to a balance system, hence this system will adapt to in such a manner to make balance to some of this pressures at the time of system tries is balance returned. This order known as Le ChatelierLaw (taken away from name of chemistry Prances Henri Le Chatelier) that is : Isi dengan Judul Halaman Terkait

  26. CONCENTRATION INFLUENCE • If in homogenous equilibrium system, wrong concentration one matters is enlarged, hence equilibrium will shift towards which at the opposite from the matter. • On the contrary, if concentration one of matter minimized, hence equilibrium will shift towards the matter. Isi dengan Judul Halaman Terkait

  27. Change influence of concentration of in equilibrium Isi dengan Judul Halaman Terkait

  28. ACCENTUAL INFLUENCE OR VOLUME • If pressure from system is boosted up, hence will reduce full scale of mole gas, on the contrary if system pressure is degraded, hence will boost up full scale of gas mole. • So the statement can be told : • If system pressure is enlarged = system volume is minimized, equilibrium will shift towards small reaction coefficient amounts. Isi dengan Judul Halaman Terkait

  29. If system pressure is minimized = system volume is enlarged, equilibrium will shift towards big reaction coefficient amounts. • In equilibrium system where coefficient amounts reaction of left side = number of coefficients right side, hence accentual change / volume doesn't shift situation of equilibrium. Isi dengan Judul Halaman Terkait

  30. TEMPERATURE INFLUENCE • Increase of temperature will cause equilibrium to shift toward forming of compound permeating temperature (endothermic reaction). • On the contrary degradation of temperature will cause equilibrium to shift towards forming of compound releasing temperature (exothermic reaction). Isi dengan Judul Halaman Terkait

  31. ADDITION OF CATALYST • Addition of catalyst at system will change reaction speed, • cannot shift equilibrium of good reaction towards product (shifts dextrose) and or towards to reactant • catalyst only influence activation energy for forward reaction and or reaction of returning, what changes its(the speed is of equal size. • Equilibrium will be reached is quicker with existence of catalyst. Isi dengan Judul Halaman Terkait

  32. What is going on if at the equilibrium : a) temperature is boosted up; b) temperature is degraded; c) accentual is boosted up by lessening volume; d) addition of catalyst Platinum; e) addition of H2 into system? f) lessens NH3 in system? Isi dengan Judul Halaman Terkait

  33. REPLY • Reaction is upper is exothermic reaction (Δ H negativity) for forward reaction (from left of dextrose). Addition of temperature will shift equilibrium towards endothermic reaction, means will equilibrium. b) Reduction temperature will shift equilibrium to exothermic reaction that is dextrose. IsidenganJudulHalamanTerkait

  34. c) Addition pressure will shift equilibrium to mole amounts smaller that is dextrose. d) Addition catalyst doesn't shift equilibrium. e) Addition matter reactant will shift equilibrium to product that is dextrose. f) Reduction matter ( product matter) will shift equilibrium to part lessened that is dextrose. Isi dengan Judul Halaman Terkait

  35. Thanks Isi dengan Judul Halaman Terkait