Question

13. Suggest three ways in which the concentration of CO, could be increased if an equilibrium exists in the following equation. CH. (g) + 20, (g) + CO. (g) + 2H20 (1) AH = -213 kcal/mol

Answer 1

The given equilibriumis CH, (g) + 2 02(8) ----------> CO2 (g) + 2 H20 (1) AH =- 213 kJ/mol Since AH is negative, the reaction is exothermic. According to Le Chatelier's principle, When a reversible reaction is at equilibrium, the system adjusts to reduce the effect of the applied change and reach a new equilibrium. According to Le Chatelier's principle, For an exothermic reaction, heat is a product. Therefore, increasing the temperature will shift the equilibrium to the left, while decreasing the temperature will shift the equilibrium to the right. For exothermic reaction, Heat is the product. Cooling the reaction (decreasing the temperature), the equilibrium will shift to the right side. So, the conc. of CO2 is increased by decreasing the temperature 2. Increase in pressure of the system (or decrease in volume ), the equilibrium will shift towards the side with least moles of gas. The number of moles of gaseous reactants = 3 The number of moles of gaseous products = 1 Increase in pressure of the system, the equilibrium will shift towards the side with least moles of gas (that is towards products). So, production of Co, increases 3. Decreasing the volume., the conc. of CO2 increases. 4. According to Le Chatelier's principle, Increase in the conc. of the reactants, the equilibrium will shift towards the product side and vice versa Increasing conc. of CH4 and 02, the equilibrium will shift towards the product side. So, the conc. of CO2 increases.