We have this following gas equilibrium :
H2 + Cl2 <==> 2HCl + 184 kJ
then predict the following to know Le chatlier's prediction
1) adding Cl2
2) removing HCl
3) elevation of pressure
4) lowering of the temperature
5) removing H2 and lowering pressure
6) adding catalyst
7) elevation of temperature
8) reducing the volume of system
thank you very much
See you last post for that detail explaination I gave for CO2
To predict the effect of Le Chatelier's principle on a gas equilibrium, we need to consider the following:
1) Adding Cl2: By adding more Cl2 to the system, it will increase the concentration of Cl2. According to Le Chatelier's principle, an increase in the concentration of reactants will shift the equilibrium to the right, favoring the formation of products. Therefore, adding more Cl2 will increase the concentration of HCl.
2) Removing HCl: Removing HCl will decrease its concentration. According to Le Chatelier's principle, when a product is removed, the equilibrium will shift to compensate for the loss. Therefore, the equilibrium will shift to the left, favoring the formation of reactants, H2, and Cl2.
3) Elevation of pressure: Increasing the pressure will shift the equilibrium towards the side with fewer moles of gas. In this case, H2 and Cl2 have 1 mole each, while 2HCl only has 2 moles. Therefore, increasing the pressure will shift the equilibrium to the right, increasing the concentration of HCl.
4) Lowering the temperature: Decreasing the temperature will favor the exothermic reaction, which releases heat (184 kJ in this case). According to Le Chatelier's principle, decreasing the temperature will shift the equilibrium towards the side that produces more heat. Therefore, the equilibrium will shift to the right, favoring the formation of HCl.
5) Removing H2 and lowering pressure: Removing H2 and lowering the pressure simultaneously will decrease the concentration of reactants. According to Le Chatelier's principle, decreasing the concentration of reactants will shift the equilibrium to compensate for the loss. Therefore, the equilibrium will shift to the left, favoring the formation of H2 and Cl2.
6) Adding a catalyst: Adding a catalyst does not affect the position of the equilibrium. A catalyst speeds up the forward and reverse reactions equally, allowing the equilibrium to be reached faster but not altering the final composition.
7) Elevation of temperature: Increasing the temperature will favor the endothermic reaction, which absorbs heat (184 kJ in this case). According to Le Chatelier's principle, increasing the temperature will shift the equilibrium towards the side that consumes more heat. Therefore, the equilibrium will shift to the left, favoring the formation of H2 and Cl2.
8) Reducing the volume of the system: Decreasing the volume will increase the pressure. As explained earlier, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas. In this case, it will favor the formation of HCl. Therefore, reducing the volume will shift the equilibrium to the right, increasing the concentration of HCl.
Remember, Le Chatelier's principle states that a system at equilibrium will respond to a change by shifting its position to counteract the change.