Applications Of Chemical Equilibrium In Industrial Processes Environmental Sciences Essay

Applications Of Chemical Equilibrium In Industrial Processes Environmental Sciences Essay From the simple processes of dissolution and crystallization in a saturated sugar solution to a complicated industrial process of oxidation and reduction in industry chemical equilibrium plays a major role. Chemical equilibrium is the balance in the rate of two opposing reversible reactions with no change applied to the system with applied constant pressure and temperature. In a system where carbon monoxide is reacting with oxygen gas to form carbon dioxide there will be quantity of carbon monoxide left in the solution for as long as the reaction is placed. This is due to this reaction being a reversible reaction, although carbon monoxide and oxygen gas are synthesizing to form carbon dioxide, a contradicting reversible reaction is taking place, the decomposition of carbon dioxide to form carbon monoxide and oxygen gas. Figure 1: Chemical EquilibriumAs shown in Figure 1, in a reversible process, the rate of reaction for products turning into reactants [forward reaction] slows down a s more reactants are changed into products simultaneously the rate of reaction of products changing into reactants [backwards reaction] speeds up. At a certain time for a specific temperature and pressure, the rate of reaction for both would be equal with no further change in the system.reaction-rate-time-graph.gif Still, when the system is under influence of a change in temperature or pressure the reversible reaction would be affected. Le Chatelier’s principle generalizes this in â€Å"if a system in equilibrium is subjected to a stress the equilibrium will shift in the direction which tends to relive the stress†. (Le Chatelier’s Principle) If the system is under the influence of a temperature altering the system will oppose this change. If an increase in temperature causes the increase in the rate of an endothermic reaction then the system will oppose this reaction by lowering the temperature thus favoring the endothermic reaction. Similarly, if the decrease i n temperature increases the rate of the endothermic reaction, then the system opposes this stress by favoring the exothermic reaction. Pressure, is another variable contributing in affecting the state of equilibrium that affects gaseous reaction only. If an increase in pressure is applied, then the system opposes this change by aiming to lower the pressure favoring the side with less gas molecules. Likewise, if a decrease in pressure is applied then the system opposes this change by increasing the pressure favoring the side with more gaseous molecules. Several process in industry depend on Le Chatelier’s principle, the Haber-Posch process, the contact process, and the Ostwald process. In the Haber process nitrogen gas from air reacts with hydrogen gas from natural gas [mainly methane] in order to provide ammonia gas. Since ammonia is a crucial substance in agriculture for the manufacturing of fertilizers it is vital to produce as much as possible in the lowest time possible. N2(g) + 3 H2(g) is in equilibrium with 2 NH3(g) ΆH=-92KJ mol-1 The previous equation shows the chemical equation for the formation of ammonia. In order to obtain the highest amount of ammonia the reaction needs to be stimulated forward.