Reaction Balance.

Reaction Balance

Isi dengan Judul Halaman Terkait
Standard Competency Basic Competency Understanding the concept of Balance reaction Mastering balance reaction Mastering the factors that influence balance movement Determining quantitative relation between reactor and the result of reaction from a balance reaction Using unit concentration in making solution The aim of the lesson 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 Hal.: 2 Isi dengan Judul Halaman Terkait

Reaction balance Most of chemical reaction goes on two direction or reversible. First, reaction goes to product with V1 speed 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) and reactant concentration and product do not change any more at the same time, so they will reach chemical balance, such as water steaming procees. Hal.: 3 Isi dengan Judul Halaman Terkait

The process of chemical balance between liquid and steam Hal.: 4 Isi dengan Judul Halaman Terkait

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 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 Hal.: 5 Isi dengan Judul Halaman Terkait

Example of reaction; Has Kc Value; So that in desolation reaction formed a bigger product because of Kc>1 Hal.: 6 Isi dengan Judul Halaman Terkait

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; So the value of Kp is; pNH3, pN2, and pH2 are each of partial pressure from NH3, N2 and H2 which is defined in atm Hal.: 7 Isi dengan Judul Halaman Terkait

The Connection between Kc and Kp
Let us take a look the balance similarity below; That similarity has the value; And the Kp valve is; From the similarity ideal gas; Where the concentration is; Hal.: 8 Isi dengan Judul Halaman Terkait

To substitute P/RT for n/v in Kc in similarity above gives connection between Kc and kp; Or; Where Δn = (nproduct – nreactant) 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 Hal.: 9 Isi dengan Judul Halaman Terkait

Homogeneous equilibrium term applied to reaction which all spesi is reacting stays at the same phase. Example of from equilibrium of homogen is reaction of ammonia forming, NH3, nitrogen, N ( g) and oxygen, O ( g); with the price of konstanta its the equilibrium is: Hal.: 10 Isi dengan Judul Halaman Terkait

Example of equilibrium in system other homogen is: Equilibrium in gas system the price of Constanta its the equilibrium is; Hal.: 11 Isi dengan Judul Halaman Terkait

Reversible reaction entangling reaktan and product which its(the phase differs in yields heterogene equilibrium. Its the example is reacting decomposition of Merkuri oxide: The equilibrium consisted of solid phase ( solid=s), dilution (liquid=l) and gas ( g), hence for solid phase ( sulfur) and dilution ( levator skapula) in signifikan is not influenced by pressure change. Hence the price of Kc and Kp to react upper is: Hal.: 12 Isi dengan Judul Halaman Terkait

Some things which must be gave attention to equilibrium of heterogene 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. If equilibrium between solid matters and condensation enterred in calculation Kc only concentration of dissolving matters only, while Kp cannot expressed. For equilibrium between matters in condensation if its(the solvent pertained one of reaktan or result of its(the reaction hence concentration from the solvent is not packed into calculation Kc. Hal.: 13 Isi dengan Judul Halaman Terkait

Factor Influencing Equilibrium
This order known as Asas Le Châtelier ( taken away from name of chemistry Prancis Henri Le ChÇtelier) that is : 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. Hal.: 14 Isi dengan Judul Halaman Terkait

Concentration Influence
If in homogen equilibrium system, wrong concentration one matters is enlarged, hence equilibrium will shift towards which at the oposite from the matter. On the contrary, if concentration one of matter minimized, hence equilibrium will shift towards the matter. Change influence of concentration of in equilibrium Hal.: 15 Isi dengan Judul Halaman Terkait

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. 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. Hal.: 16 Isi dengan Judul Halaman Terkait

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). Hal.: 17 Isi dengan Judul Halaman Terkait

Addition of Catalyst Addition of catalyst at system will change reaction speed, but cannot shift equilibrium of good reaction towards product (shifts dextrorse) and or towards to reaktan ( shifts sinistrorse). Because 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. Example; Reaction of under this to equilibrium in place of closed at temperature 500 degree Celciuses Hal.: 18 Isi dengan Judul Halaman Terkait

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? Hal.: 19 Isi dengan Judul Halaman Terkait

Reply: a) Reaction is upper is exothermic reaction (Δ H negativity) for forward reaction (from left of dextrorse). Addition of temperature will shift equilibrium towards endothermic reaction, means will shift sinistrorse equilibrium. b) Reduction temperature will shift equilibrium to exothermic reaction that is dextrorse. c) Addition pressure will shift equilibrium to mole amounts smaller that is dextrorse. d) Addition catalyst doesn't shift equilibrium. e) Addition matter reaktan will shift equilibrium to product that is dextrorse. f) Reduction matter ( product matter) will shift equilibrium to part lessened that is dextrorse. Hal.: 20 Isi dengan Judul Halaman Terkait

Thank Hal.: 21 Isi dengan Judul Halaman Terkait

Reaction Balance.

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