A student says, "The initial concentration of a reactant was doubled, and the rate doubled. Therefore the reaction is second order in that reactant." Why might the student say that? What is wrong with the statement? What is the actual order with respect to the reactant?

Answer is in the explanation.

Explanation:

The statement:  "The initial concentration of a reactant was doubled, and the rate doubled" implies the initial concentration is directly proportional to rate of reaction. That is:

Rate = K [A]₀

But this law is rate law of first order reaction. Second order reaction has as law:

Rate = K [A]₀²

These law implies:  "The initial concentration of a reactant was doubled, and the rate quadruplicate", a different statement.

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.