Consider the following reaction:

a + b + c right arrow d

the rate law for this reaction is as follows:

rate = k time fraction [a][c]^2 over [b]^1/2

suppose the rate of the reaction at certain initial concentrations of a, b, and c is 1.12×10-2 m/s.

what is the rate of the reaction if the concentrations of a and c are doubled and the concentration of b is tripled?

rate 2 = ? m/s

The rate of the reaction when concentrations are changed is

Explanation:

For the given chemical reaction:

The given rate law of the reaction follows:

We are given:

When the concentrations are changed:

New concentration of A = 2A  (Concentration is doubled)

New concentration of C = 2C   (Concentration is doubled)

New concentration of B = 3B     (Concentration is tripled)

The new rate law expression becomes:

Hence, the rate of the reaction when concentrations are changed is

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:

its mg hope this