Flashcards for NEET Chemistry - Chemical Kinetics

Flashcards for NEET Chemistry are designed to boost your NEET preparation. Find below flashcards for the chapter “Chemical Kinetics”. These flashcards are prepared as per the NEET syllabus. These are helpful for aspirants of NEET and other exams, during last-minute revision. It covers all the important points that are frequently asked in the exam. Check BYJU’S, for the full set of Flashcards and Study material for NEET Chemistry.

Download PDF of NEET Chemistry Flashcards for Chemical Kinetics

Name of the NEET Sub-section

Topic

Flashcards Helpful for

Chemistry

Chemical Kinetics

NEET Exams

flashcards for neet chemistry dec13 chemical kinetics 1
flashcards for neet chemistry dec13 chemical kinetics 2
flashcards for neet chemistry dec13 chemical kinetics 3

   

Chemical Kinetics

Order of a Reaction

It is the sum of powers of the concentration of the reactants

Rate = k [A]x [B]y

order = x + y

Zero-Order Reactions

Rate = k[R]0

k = [R]0−[R]/t

unit of k is mol L-1s-1

E.g. The decomposition of gaseous ammonia on a hot platinum surface

The thermal decomposition of HI on gold surface

First-Order Reactions

Rate = k[R]

k = 2.303/t log [R]0/[R]

unit of k is s-1

E.g. All natural and artificial radioactive decay of unstable nuclei, decomposition of N2O5 and N2O

Half-Life of a Reaction

It is the time in which the concentration of a reactant becomes half of its initial concentration. It is denoted by t1/2.

For zero order reaction t1/2 ∝ [R]0 or initial concentration

t1/2 = [R]0/2k

For first order reaction t1/2 is independent of [R]0 and is equal to 0.693/k

Collision Frequency

It is the number of collisions per second per unit volume

Rate of reaction = ZAB e−Ea /RT

ZAB – collision frequency of reactants

e−Ea /RT – fraction of molecules with energies equal or more than Ea (activation energy)

Arrhenius Equation

It explains the temperature dependence of the rate of a reaction

k = A e-Ea /RT

A – Arrhenius factor or the frequency factor

Ea – activation energy in joules/mole (J mol –1)

Pseudo First Order Reaction

Reactions that become first order under certain conditions

E.g. Acid hydrolysis of ethyl acetate

Acid catalysed inversion of cane sugar

Effective Collisions

Collisions in which molecules collide with sufficient kinetic energy or threshold energy and proper orientation

Rate = PZAB e–Ea/RT

P – probability or steric factor

Activation Energy (Ea)

It is the energy required by reactant molecules to form the intermediate or activated complex (C)

ΔH = Activation energy of forward reaction – Activation energy of backward reaction

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