IIT JEE Test Series — Practice smarter, perform stronger.

Chemical Kinetics formulas

Master Chemical Kinetics through 22 JEE Advanced-level formulas, systematically structured with every variable spelled out. Revise concept-wise, identify the areas where you need improvement, and focus your preparation with greater precision.

Practise these formulas Know more about IIT JEE

Back to Formula Book

Chemical Kinetics, every formula

22 formulas, typeset and free. Print it, or keep it open beside your practice.

Rate of reaction
$rate = - \frac{1}{a} \frac{d [ A ]}{d t} = + \frac{1}{b} \frac{d [ B ]}{d t}$
Q1MCQRate
For $2A\to B$, the rate of reaction is:
- A
  $-\tfrac12\dfrac{d[A]}{dt}$
- B
  $-\dfrac{d[A]}{dt}$
- C
  $-2\dfrac{d[A]}{dt}$
- D
  $\dfrac{d[A]}{dt}$
Rate law
$rate = k [A]^{m} [B]^{n}$
Q1MCQRate law
The rate law of a reaction is:
- A
  $k[A]^{m}[B]^{n}$
- B
  $k[A][B]$ always
- C
  $k[A]+[B]$
- D
  $k$
Order of reaction
$order = m + n$
Zero-order integrated
$[A] = [A]_{0} - k t$
Q1MCQZero order
The integrated rate law for a zero-order reaction is:
- A
  $[A]=[A]_0-kt$
- B
  $\ln[A]=\ln[A]_0-kt$
- C
  $\dfrac{1}{[A]}=\dfrac{1}{[A]_0}+kt$
- D
  $[A]=[A]_0 e^{-kt}$
Zero-order half-life
$t_{1/2} = \frac{[ A ] _{0}}{2 k}$
Q1MCQZero-order t½
The half-life of a zero-order reaction is:
- A
  $\dfrac{[A]_0}{2k}$
- B
  $\dfrac{0.693}{k}$
- C
  $\dfrac{1}{k[A]_0}$
- D
  $\dfrac{2k}{[A]_0}$
First-order integrated
$k = \frac{2.303}{t} lo g \frac{[ A ] _{0}}{[ A ]}$
Q1MCQFirst order
The integrated first-order rate constant is:
- A
  $\dfrac{2.303}{t}\log\dfrac{[A]_0}{[A]}$
- B
  $\dfrac{[A]_0-[A]}{t}$
- C
  $\dfrac{1}{[A]}-\dfrac{1}{[A]_0}$
- D
  $kt$
First-order half-life
$t_{1/2} = \frac{0.693}{k}$
Q1MCQFirst-order t½
The half-life of a first-order reaction is:
- A
  $\dfrac{0.693}{k}$
- B
  $\dfrac{[A]_0}{2k}$
- C
  $\dfrac{1}{k[A]_0}$
- D
  $0.693\,k$
Second-order integrated
$\frac{1}{[ A ]} - \frac{1}{[ A ] _{0}} = k t$
Q1MCQSecond order
The integrated second-order rate law is:
- A
  $\dfrac{1}{[A]}-\dfrac{1}{[A]_0}=kt$
- B
  $[A]=[A]_0-kt$
- C
  $\ln[A]=\ln[A]_0-kt$
- D
  $[A]=[A]_0 e^{-kt}$
Second-order half-life
$t_{1/2} = \frac{1}{k [ A ] _{0}}$
Q1MCQSecond-order t½
The half-life of a second-order reaction is:
- A
  $\dfrac{1}{k[A]_0}$
- B
  $\dfrac{0.693}{k}$
- C
  $\dfrac{[A]_0}{2k}$
- D
  $k[A]_0$
Arrhenius equation
$k = A e^{- E_{a} / R T}$
Q1MCQArrhenius
The Arrhenius equation is:
- A
  $k=A\,e^{-E_a/RT}$
- B
  $k=A\,e^{E_a/RT}$
- C
  $k=\dfrac{A}{E_a}$
- D
  $k=AE_a T$
Arrhenius (log form)
$ln k = ln A - \frac{E _{a}}{R T}$
Q1MCQArrhenius log
The logarithmic Arrhenius form is:
- A
  $\ln k=\ln A-\dfrac{E_a}{RT}$
- B
  $\ln k=\ln A+\dfrac{E_a}{RT}$
- C
  $\ln k=\dfrac{E_a}{RT}$
- D
  $\ln k=A$
Two-temperature Arrhenius
$ln \frac{k _{2}}{k _{1}} = \frac{E _{a}}{R} (\frac{1}{T _{1}} - \frac{1}{T _{2}})$
Q1MCQTwo-T Arrhenius
The two-temperature Arrhenius relation is:
- A
  $\ln\dfrac{k_2}{k_1}=\dfrac{E_a}{R}\left(\dfrac{1}{T_1}-\dfrac{1}{T_2}\right)$
- B
  $\ln\dfrac{k_2}{k_1}=\dfrac{E_a}{R}(T_2-T_1)$
- C
  $\dfrac{k_2}{k_1}=e^{E_a}$
- D
  $k_2=k_1$
Temperature coefficient
$\frac{k _{T + 10}}{k _{T}} \approx 2 to 3$
Q1MCQTemperature coefficient
For a $10$ K rise, the rate constant typically:
- A
  increases 2–3 times
- B
  halves
- C
  is unchanged
- D
  increases 10 times
Units of rate constant
$k : (mol/L)^{1 - n} s^{- 1}$
Q1MCQUnits of k
The units of the rate constant of an $n$th-order reaction are:
- A
  $(\text{mol/L})^{1-n}\text{s}^{-1}$
- B
  $\text{s}^{-1}$
- C
  $\text{mol/L}$
- D
  dimensionless
Rate constant (zero order)
$k = mol L^{- 1} s^{- 1}$
Q1MCQZero-order units
The units of $k$ for a zero-order reaction are:
- A
  $\text{mol L}^{-1}\text{s}^{-1}$
- B
  $\text{s}^{-1}$
- C
  $\text{L mol}^{-1}\text{s}^{-1}$
- D
  dimensionless
Rate constant (first order)
$k = s^{- 1}$
Q1MCQFirst-order units
The units of $k$ for a first-order reaction are:
- A
  $\text{s}^{-1}$
- B
  $\text{mol L}^{-1}\text{s}^{-1}$
- C
  $\text{L mol}^{-1}\text{s}^{-1}$
- D
  dimensionless
Molecularity
$number of species in an elementary step$
Q1MCQMolecularity
Molecularity is the number of species in:
- A
  an elementary step
- B
  the overall reaction
- C
  the products
- D
  the catalyst
Fraction remaining (first order)
$\frac{[ A ]}{[ A ] _{0}} = e^{- k t}$
Q1MCQFraction remaining
For a first-order reaction, the fraction remaining is:
- A
  $e^{-kt}$
- B
  $1-kt$
- C
  $\dfrac{1}{kt}$
- D
  $kt$
Activation energy from graph
$slope of ln k vs \frac{1}{T} = - \frac{E _{a}}{R}$
Q1MCQEa from graph
The slope of $\ln k$ versus $\dfrac{1}{T}$ is:
- A
  $-\dfrac{E_a}{R}$
- B
  $\dfrac{E_a}{R}$
- C
  $E_a$
- D
  $\ln A$
Average rate
$avg rate = \frac{Δ [ A ]}{Δ t}$
Time for nth-life (first order)
$t = \frac{2.303}{k} lo g \frac{[ A ] _{0}}{[ A ]}$
Threshold energy
$E_{t h} = E_{a} + E_{r e a c t an t s}$
Q1MCQThreshold energy
The threshold energy equals:
- A
  $E_a+E_{reactants}$
- B
  $E_a-E_{reactants}$
- C
  $E_a$
- D
  $E_{reactants}$

More JEE Advanced Chemistry formula sheets

Every chapter sheet is typeset, free and open without a sign-in.

Other ways to revise this chapter

Master this chapter with similar other learning materials.

Preparing students for India’s top institutes

Our students are currently into top technological and medical institutes of India.

IIT Bombay
IIT Delhi
IIT Madras
IIT Kanpur
IIT Kharagpur
IIT Roorkee
IIT Guwahati
IIT BHU Varanasi
AIIMS Delhi
NIT Tiruchirappalli
NIT Rourkela
IIT Bombay
IIT Delhi
IIT Madras
IIT Kanpur
IIT Kharagpur
IIT Roorkee
IIT Guwahati
IIT BHU Varanasi
AIIMS Delhi
NIT Tiruchirappalli
NIT Rourkela

Join QuestPix, Today!

Get notified first, with exam & curriculum updates, course & test series launch offers, motivation & success stories and free learning resources recommended by toppers.

Chemical Kinetics formulas

Chemical Kinetics, every formula

Rate of reaction

Rate law

Order of reaction

Zero-order integrated

Zero-order half-life

First-order integrated

First-order half-life

Second-order integrated

Second-order half-life

Arrhenius equation

Arrhenius (log form)

Two-temperature Arrhenius

Temperature coefficient

Units of rate constant

Rate constant (zero order)

Rate constant (first order)

Molecularity

Fraction remaining (first order)

Activation energy from graph

Average rate

Time for nth-life (first order)

Threshold energy

More JEE Advanced Chemistry formula sheets

Other ways to revise this chapter

Preparing students for India’s top institutes

Join QuestPix, Today!