Question

1. Consider the reaction at equilibrium: CO(g) + Cl₂(g)   $\longleftrightarrow$ COCl₂(g). Predict how addition of CO(g) will affect the equilibrium system.

2. What would be the net effect of decreasing the temperature on the following exothermic reaction? $CO\left(g\right)\:+\:Cl_2\left(g\right)\longleftrightarrow\:COCl_2\left(g\right)$

3. What is the effect on the following equilibrium system if CaO(s) is added? $CaCO_3\left(s\right)\:\longleftrightarrow\:CaO\left(s\right)\:+\:CO_2\left(g\right)$

4. Consider the reaction at equilibrium. CO(g) + Cl₂(g)   $\longleftrightarrow$ ⟷ COCl₂(g) Predict how addition of CO(g) will affect the equilibrium system.

Please help explain the answers to these!

Answer 1

Addition of CO(g) will affect the equilibrium system. CO(g) + Cl2(g) <==> COCl2(g). Le Chatelier's Principle: According to this principle, whenever an equilibrium system is subjected to change, certain processes takes place which have a tendency to partially neutralize the initial change, which result in bringing the system to a new position of equilibrium. This principle mainly explains three different equilibrium changes: addition of CO(g) will affect the equilibrium system 1. Reaction shifts towards Forward direction because CO is a reactant. 2. addition of CO(g) will increase the concentration of CO. 1. Equilibrium change due to change in the concentration Exothermic reaction: 2. Equilibrium change due to change in the volume or pressure 3. Equilibrium change due to change in the temperature If the energy is removed to this system at equilibrium by decreasing the temperature it, Le Chatelier's principle predict th at the shift will be in the direction that produces energy, that is, to the right. The value of K increases with decreased temperature, as predicted. Equilibrium change due to change in the concentration: Changing the concentration of a species will shift the equilibrium that side which would reduce that change in concentration. CaCO3(s) <---- Cao (s) +CO2 (g) if Cao(s) is added in the above equilibrium system Reaction shifts towards reverse or backward direction because CaO is a product. addition of CO(g) will affect the equilibrium system. Equilibrium change to change in the volume or pressure: According to this law a change in the volume of an equilibrium system that one or more gases changes the concentration of those gases. CO(g) + Cl2(g) <==> COCl(g). If equilibrium of gaseous of molecules is condensed than the pressure of equilibrium is increased. This increased pressure will be partially relieved by a shift of equilibrium in the less gaseous molecules. addition of CO(g) will affect the equilibrium system 1. Reaction shifts towards Forward direction because CO is a reactant. 2. addition of CO(g) will increase the concentration of CO. If equilibrium of gaseous of molecules is expanded than the pressure of equilibrium is decreased. This decreased pressure will be partially restored by a shift of equilibrium in the more gaseous molecules. Equilibrium change due to change in the temperature: According to Le Chatelier's Principle if heat is removed in a system than the equilibrium will shift towards heat producing direction and if heat is absorbed than the equilibrium will shift towards heat removing direction.