Question

Of the following, all are valid units for a reaction rate except _______ mol/hr M/s g/s mol/L-hr mol/L Give the characteristic of a second-order reaction having only one reactant. The rate of the reaction is not proportional to the concentration of the reactant. The rate of the reaction is proportional to the square of the concentration of the reactant The rate of the reaction is proportional to the squareroot of the concentration of the reactant. The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. The rate of the reaction is directly proportional to the concentration of the reactant. A rate is equal to 0.0200 M/s. If [A] = 0.100 M and rate = k[A]^1. what is the new rate if the concentration of [A] is increased to 0.200 M?

Answer 1

The invalid unit for a reaction rate is metres per second (M/s). A second-order reaction with one reactant has a rate proportional to the square of its concentration. For a first-order reaction, doubling a reactant's concentration will double the reaction rate.

Step-by-step explanation:

Among the units listed for a reaction rate, metres per second (M/s) is not a valid unit for a reaction rate because it is a unit of speed typically used for physical movements, not chemical reactions. Chemical reaction rates are measured in units that reflect the change in concentration over time, such as moles per liter per second (M/s).

In a second-order reaction having only one reactant, the rate of the reaction is proportional to the square of the concentration of the reactant. This means that if the concentration of the reactant is doubled, the reaction rate increases by a factor of four.

For the given reaction with rate = k[A]1 and an original rate of 0.0200 M/s at [A] = 0.100 M, if the concentration of [A] is increased to 0.200 M, since it is a first-order reaction, the new rate will be doubled to 0.0400 M/s because the rate is directly proportional to the concentration of A.