## How do you find the initial rate of a second-order reaction?

1/[A] t = kt + 1/[A] 0 is the integrated rate law for the second-order reaction A products. A plot of the inverse of [A] as a function of time shows a straight line because this equation has the form y = mx + b. The reaction’s rate constant can be calculated using the slope of the line, which is equal to k.

## How is half life period related to initial concentration for a second-order reaction?

Upon observation, we can deduce that in second order reactions, the half-life period is inversely proportional to the initial concentration of the reactant.

**Which one of the following is a second order reaction?**

Hydrolysis of ester by an alkali (saponification) is a second order reaction.

### What do you mean by second-order reactions show that for these reactions the half-life period is inversely proportional to the initial concentration?

This inverse relationship suggests that as the initial concentration of reactant is increased, there is a higher probability of the two reactant molecules interacting to form product. Consequently, the reactant will be consumed in a shorter amount of time, i.e. the reaction will have a shorter half-life.

### What is second order?

Adjective. second-order (not comparable) (mathematics, logic) describing the second in a numerical sequence of models, languages, relationships, forms of logical discourse etc.

**What’s the difference between first order and second order reactions?**

The key difference between first and second order reactions is that the rate of a first order reaction depends on the first power of the reactant concentration in the rate equation whereas the rate of a second order reaction depends on the second power of the concentration term in the rate equation.

#### What is the difference between 1st order and 2nd order reactions?

The only obvious difference, as seen in the graph below, is that the concentration of reactants approaches zero more slowly in a second-order, compared to that in a first order reaction. As before, the rate at which A decreases can be expressed using the differential rate equation:

#### What is the differential rate law for second order reactions?

The differential rate law for the simplest second-order reaction in which 2A → products is as follows: (14.6.1) rate = − Δ [ A] 2 Δ t = k [ A] 2 Consequently, doubling the concentration of A quadruples the reaction rate.

**Which is expected for a simple second-order reaction?**

The straight line in (b) is expected for a simple second-order reaction. For two or more reactions of the same order, the reaction with the largest rate constant is the fastest.

## What is the Order of the reaction and the reaction constant?

Determine the order of the reaction and the reaction constant, k, for the reaction using the tactics described in the previous problem. The order of the reaction is second, and the value of k is 0.0269 M -2 s -1. Since the reaction order is second, the formula for t1/2 = k-1 [A] o-1. This means that the half life of the reaction is 0.0259 seconds.