What do second-order reactions depend on?
A second order reaction is a type of chemical reaction that depends on the concentrations of one-second order reactant or two first-order reactants. This reaction proceeds at a rate proportional to the square of the concentration of one reactant, or the product of the concentrations of two reactants.
What are the characteristics of second-order reaction?
A) The rate of the reaction is not proportional to the concentration of the reactant. B) The rate of the reaction is directly proportional to the square of the concentration of the reactant. C) The rate of the reaction is directly proportional to the square root of the concentration of the reactant.
What is the rate constant for second-order reaction?
Zero-Order Reactions
| Zero-Order | Second-Order | |
|---|---|---|
| rate law | rate = k | rate = k[A]2 |
| units of rate constant | M s−1 | M−1 s−1 |
| integrated rate law | [ A ] = − k t + [ A ] 0 [ A ] = − k t + [ A ] 0 | 1 [ A ] = k t + ( 1 [ A ] 0 ) 1 [ A ] = k t + ( 1 [ A ] 0 ) |
| plot needed for linear fit of rate data | [A] vs. t | 1 [ A ] vs. t |
Do second-order reactions depend on concentration?
A second-order reaction will depend on the concentration (s) of one second-order reactant or two first-order reactants. To determine the order of a reaction with respect to each reactant, we use the method of initial rates.
What is the 2nd order reaction?
Definition of second-order reaction : a chemical reaction in which the rate of reaction is proportional to the concentration of each of two reacting molecules — compare order of a reaction.
Which reaction is 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].
What are the units of second order reaction?
What are the units of a second order reaction? mol-1L s-1 is the unit of rate constant for second order reaction.
What is the unit of 2nd order reaction?
Which of the following is 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. Give the characteristic of a second order reaction having only one reactant. The rate of the reaction is proportional to the square of the concentration of the reactant.
What is an example of second order reaction?
Second-order reactions generally have the form 2A → products or A + B → products. Simple second-order reactions are common. In addition to dimerization reactions, two other examples are the decomposition of NO2 to NO and O2 and the decomposition of HI to I2 and H2.
What is the rate of a second order reaction?
Since second order reactions can be of the two types described above, the rate of these reactions can be generalized as follows: Where the sum of x and y (which corresponds to the order of the chemical reaction in question) equals two. A few examples of second order reactions are given below:
What is variation of parameters?
Variation of Parameters (that we will learn here) which works on a wide range of functions but is a little messy to use. To keep things simple, we are only going to look at the case: where p and q are constants and f (x) is a non-zero function of x. The complete solution to such an equation can be found by combining two types of solution:
How do you find the variation of parameters in a differential equation?
In general, when the method of variation of parameters is applied to the second‐order nonhomogeneous linear differential equation with y = v 1 ( x ) y 1 + v 2 ( x ) y 2 (where y h = c 1 y 1 + c 2 y 2 is the general solution of the corresponding homogeneous equation), the two conditions on v 1 and v 2 will always be So…
What is the problem with second order differential equations?
This method relies on integration. The problem with this method is that, although it may yield a solution, in some cases the solution has to be left as an integral. On Introduction to Second Order Differential Equations we learn how to find the general solution.