# Which of the following represents the integrated rate law for a first-order reaction?

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

Zero-Order ReactionsZero-OrderFirst-Orderrate lawrate = krate = k[A]units of rate constantM s-1s-1integrated rate law[A] = –kt + [A]0ln [A] = –kt + ln[A]0plot needed for linear fit of rate data[A] vs. tln [A] vs. tЕщё 2 строки

## How do you write a rate law for a first order reaction?

First-Order Reactions

A first-order reaction depends on the concentration of one reactant, and the rate law is: r=−dAdt=k[A] r = − dA dt = k [ A ] .

## What is first order reaction give example?

First-order reactions are very common. We have already encountered two examples of first-order reactions: the hydrolysis of aspirin and the reaction of t-butyl bromide with water to give t-butanol. Another reaction that exhibits apparent first-order kinetics is the hydrolysis of the anticancer drug cisplatin.

## What does a first order reaction mean?

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.

## 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.

## Which step is rate determining?

The rate determining step

The overall reaction rate is determined by the rates of the steps up to (and including) the slowest elementary step. The slowest step in a reaction mechanism is called the rate determining or rate limiting step.

## What is second order reaction give example?

Examples of Second-Order Chemical Reactions

Nitrogen dioxide decomposes into nitrogen monoxide and an oxygen molecule. 2 HI → I2 + H2. Hydrogen Iodide decomposes into iodine gas and hydrogen gas.

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## How do you determine rate law?

In order to determine a rate law we need to find the values of the exponents n, m, and p, and the value of the rate constant, k. If we are given the reaction orders for a reaction, we have the values of the coefficients we need to write the rate law.

## What is the unit of 1st order reaction?

k is the first-order rate constant, which has units of 1/s. The method of determining the order of a reaction is known as the method of initial rates. The overall order of a reaction is the sum of all the exponents of the concentration terms in the rate equation.

## What is a zero order?

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.

## What are first and second order reactions?

Chemical reactions may be assigned reaction orders that describe their kinetics. … 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.

## What is 1st 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.

## What is meant by order of reaction?

: a number that relates the rate of a chemical reaction with the concentrations of the reacting substances : the sum of all the exponents of the terms expressing concentrations of the molecules or atoms determining the rate of the reaction — compare first-order reaction, second-order reaction, third-order reaction, …