Br2(g) + 5F2(g) 2BrF5(g)-1.Removing F2 from the system. 2. Increasing the volume of the system.
2HCN(g) N2(g) + C2H2(g)-Adding C2H2 to the system.
Cl2(g) + F2(g) 2ClF(g)-1.Adding Cl2 to the system. 2.Removing ClF from the system.
Because it means that the equilibrium mixture contains more product than reactants.
More Reactants will form!!
Product added to a system at equilibrium will result in the reaction moving left, or using up product to make more reactants until it reaches equilibrium again.
The equilibrium of the system will be upset.
If reactants are removed (thus taken away from the left side) the equilibrium moves 'to counteract' the reason of disturbance: removing is countered by forming back:So this eq'b'm. will move to the LEFT (
Because it means that the equilibrium mixture contains more product than reactants.
The reaction quotient is the ratio of products to reactants not at equilibrium. If the system is at equilibrium then Q becomes Keq the equilibrium constant. Q = products/reactants If Q < Keq then there are more reactants then products so the system must shift toward the products to achieve equilibrium. If Q > Keq then there are more products than reactants and the system must shift toward the reactants to reach equilibrium.
The concentrations of reactants and products are modified.
decrease in reactants and increase in products
When a system has reached chemical equilibrium, the concentrations of the reactants and product remain constant.
The system is in equilibrium.
heterogenous equilibrium
Heterogeneous Equilibrium
More Reactants will form!!
Different physical states
more reactants will form
Le Chatelier's principle says that, when a equilibrium is disturbed by adding or removing one or more of the contents, the system will attain a new equilibrium to minimize its effect. So when reactants are added to the system, some of they will react and give products in order to gain the new equilibrium.