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The two most common forms of second-order reactions will be discussed in detail in this section. To describe how the rate of a second-order reaction changes with concentration of reactants or products, the differential (derivative) rate equation is used as well as the integrated rate equation.
The simplest kind of second-order reaction is one whose rate is proportional to the square of the concentration of one reactant. These generally have the form 2A → products. A second kind of second-order reaction has a reaction rate that is proportional to the product of the concentrations of two reactants.
Second Order Reaction. Second order reactions can be defined as chemical reactions wherein the sum of the exponents in the corresponding rate law of the chemical reaction is equal to two. The rate of such a reaction can be written either as r = k [A]2, or as r = k [A] [B].
A second order reaction is a reaction where x + y = 2. This can happen if one reactant is consumed at a rate proportional to the square of the reactant's concentration (rate = k [A] 2) or both reactants are consumed linearly over time (rate = k [A] [B]).
What is a second-order reaction. Learn the differential & integrated forms of the second-order formula, along with units. What is the half-life. Check out a few examples.
Either the differential rate law or the integrated rate law can be used to determine the reaction order from experimental data. Often, the exponents in the rate law are the positive integers: 1 and 2 or even 0. Thus the reactions are zeroth, first, or second order in each reactant.
The integrated rate law for the second-order reaction A → products is 1/ [A]_t = kt + 1/ [A]_0. Because this equation has the form y = mx + b, a plot of the inverse of [A] as a...