Consider the following elementary reaction: CFCl3(g)→CFCl2(g)+Cl(g).Suppose we let k1 stand for the rate constant of this reaction, and k−1 stand for the rate constant of the reverse reaction.

Write an expression that gives the equilibrium concentration of CFCl3 in terms of k1,k−1, and the equilibrium concentrations of CFCl2 and Cl.

Explanation:

The equilibrium constant is equal to the ratio of the rate constant of the forward reaction to the rate constant of the reverse reaction:

Then, using k₁ and k₋₁ for the rate constants of the forward and the reverse reactions, respectively:

The equilibrium equation is:

          CFCl₃(g)   ⇄   CFCl₂(g)   +   Cl(g)

For which the equilibrium constant is:

Now you can write the equilibrium concentraion of CFCl₃(g) in terms of k₁, k₋₁, [CFCl₂(g)], and [Cl(g)]:

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

aquifers are bounded above and below by impermeable rock. the driving force of groundwater movement in confined aquifers is pressure, rather than gravity.