H2(g)+Cl2(g)<--->2HCl(g)+184kj
addition of Cl2
I suggest you repost at the top of the page an clarify exactly what question yu are asking.
To determine the effect of adding Cl2 to the reaction H2(g) + Cl2(g) <-> 2HCl(g) + 184kJ, we need to consider Le Chatelier's principle.
Le Chatelier's principle states that when a system in equilibrium is subjected to a stress, it will shift its position in order to mitigate that stress and restore equilibrium.
In this case, adding Cl2 is increasing the concentration of Cl2, which is a reactant. According to Le Chatelier's principle, the reaction will shift in the direction that consumes the added Cl2 in order to reduce its concentration.
Therefore, the equilibrium will shift towards the right side, favoring the formation of more HCl. This means that more HCl will be produced, consuming the added Cl2 until a new equilibrium is reached.
It is important to note that the amount of HCl formed will depend on the initial concentration of the reactants and the equilibrium constant of the reaction. The equilibrium constant describes the ratio of the concentrations of the products to the concentrations of the reactants at equilibrium.
To determine the exact amount of HCl formed, you would need to know the initial concentrations, the volume of the system, and the equilibrium constant. With this information, you could use the equilibrium expression and solve for the concentration of HCl.
Remember, Le Chatelier's principle can only give us information about the direction of the shift and the qualitative changes in the equilibrium position. To determine the quantitative changes, you need additional information or experimental data.