**What is integrated rate of equation?** **An equation representing the dependence of the rate of reaction on the concentration of reacting species** is known as a differential rate equation. The instantaneous rate of reaction is expressed as the slope of the tangent at any instant of time in the concentration-time graph.

**What is the difference between rate laws and integrated rate laws?** Rate laws can be expressed either as a differential rate law, describing the change in reactant or product concentrations as a function of time, or as an integrated rate law, describing the actual concentrations of reactants or products as a function of time.

**How is integrated rate law derived?**

**What is the purpose of an integrated rate law?** We can use an integrated rate law **to determine the amount of reactant or product present after a period of time or to estimate the time required for a reaction to proceed to a certain extent**.

## What is integrated rate of equation? – Additional Questions

### What is integrated rate law for first order reaction?

For the first reaction, A → Products, the integrated rate law is given by the equation. **K=t2**.

### What is the zero-order integrated rate law?

The integrated rate law for the zero-order reaction A → products is **[A]_t = -kt + [A]_0**. Because this equation has the form y = mx + b, a plot of the concentration of A as a function of time yields a straight line. The rate constant for the reaction can be determined from the slope of the line, which is equal to -k.

### What is the integrated rate law for a second-order reaction?

The integrated rate law for a second order reaction says that **one over the concentration of reactant A at some time t, is equal to the rate constant k times the time plus one over the initial concentration of A**.

### What is the zero-order reaction?

Definition of zero-order reaction

: **a chemical reaction in which the rate of reaction is constant and independent of the concentration of the reacting substances** — compare order of a reaction.

### How do you integrate a first-order reaction?

For first-order reactions, the equation **ln[A] = -kt + ln[A]**_{0} is similar to that of a straight line (y = mx + c) with slope -k. This line can be graphically plotted as follows. Thus, the graph for ln[A] v/s t for a first-order reaction is a straight line with slope -k.

### What is the first-order rate law?

First-Order Reactions

[ A ] t = 1 2 [ A ] 0 . This equation describes an expected inverse relation between the half-life of the reaction and its rate constant, k.

### What is 1st order reaction?

Definition of first-order reaction

: **a chemical reaction in which the rate of reaction is directly proportional to the concentration of the reacting substance** — compare order of a reaction.

### How do integrated rate laws determine reaction order?

We measure values for the initial rates of a reaction at different concentrations of the reactants. From these measurements, we determine the order of the reaction in each reactant. Integrated rate laws are determined **by integration of the corresponding differential rate laws**.

### What is zero first and second-order reaction?

A zero-order reaction proceeds at a constant rate. A first-order reaction rate depends on the concentration of one of the reactants. A second-order reaction rate is proportional to the square of the concentration of a reactant or the product of the concentration of two reactants.

### How do you know if a reaction is first or second-order?

Initial Rate (M/s)

Determine the reaction order and the rate constant. **If a plot of reactant concentration versus time is not linear but a plot of 1/reaction concentration versus time is linear, then the reaction is second order**.

### What is the difference between zero order and first-order reaction?

The fundamental difference between zero and first-order kinetics is **their elimination rate compared to total plasma concentration**. Zero-order kinetics undergo constant elimination regardless of the plasma concentration, following a linear elimination phase as the system becomes saturated.

### How do you know if a reaction is zero order?

How do you know if it’s a Zero Order Reaction? **If the reactant concentration increases, the reaction has zero-order kinetics**. It has first-order kinetics if it has no effect. The reaction has second-order kinetics if increasing the reactant decreases the half life.

### What are the examples of zero order reaction?

The rate of the reaction is related to the reactant’s concentration.

**Examples**

- The reaction of hydrogen with chlorine is also known as a Photochemical reaction.
- Decomposition of nitrous oxide on a hot platinum surface.
- Decomposition of NH3 in the presence of molybdenum or tungsten is a zero-order reaction.

### What is the unit for rate constant?

The units of the rate constant, k, depend on the overall reaction order. **The units of k for a zero-order reaction are M/s, the units of k for a first-order reaction are 1/s, and the units of k for a second-order reaction are 1/(M·s)**. Created by Yuki Jung.

### What is first order kinetics?

First order kinetics **occur when a constant proportion of the drug is eliminated per unit time**. Rate of elimination is proportional to the amount of drug in the body. The higher the concentration, the greater the amount of drug eliminated per unit time. For every half life that passes the drug concentration is halved.

### What is 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.

### What is a 3rd order reaction?

A third-order reaction is **a chemical reaction where the rate of reaction is proportional to the concentration of each reacting molecules**. In this reaction, the rate is usually determined by the variation of three concentration terms.