The reaction X → products is second order in X and has a rate constant of 0.035 M−1s−1. If a reaction mixture is initially 0.45 M in X, what is the concentration of X after 155 seconds?

The concentration of X after 155 seconds is 0.13 M

Explanation:

Integrated rate law for second order kinetics is given by:

= initial concentration = 0.45 M

a= concentration left after time t = ?

k = rate constant =

t = time of decmposition = 155 s

Thus the concentration of X after 155 seconds is 0.13 M

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:

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