Question

Please can anyone explain me collision theory with formulas......please.... don't spam.....​

Answer 1

Collision Theory

According to the collision theory, “the molecules of reactants are assumed to be hard spheres and the reactions are assumed to occur only when these spheres (molecules) collide with each other”. So it was important to quantify the number of collisions occurring in order to form products so that we can have a clear picture of the reaction, and hence came the term collision frequency.

Collision Frequency can be understood as the number of collisions per second per unit volume of the reacting mixture. It is generally denoted by Z.

Let’s consider the following bimolecular elementary reaction:

P + Q → Product

Now as per the collision theory, the rate of the above reaction can be given by:

Rate=ZPQe−EaRT………………………….(1)

Where:

ZPQ = collision frequency of reactants P and Q

Ea = Activation Energy

R = Universal Gas Constant

T = Temperature in absolute scale

One more parameter that affected the rates of chemical reactions significantly is activation energy (Ea). The term activation energy was given by Arrhenius, it is the minimum amount of energy that the reactants must possess in order to form a product during a chemical reaction.

Answer 2

Answer:

Collision theory, theory used to predict the rates of chemical reactions, particularly for gases. The collision theory is based on the assumption that for a reaction to occur it is necessary for the reacting species (atoms or molecules) to come together or collide with one another. Not all collisions, however, bring about chemical change. A collision will be effective in producing chemical change only if the species brought together possess a certain minimum value of internal energy, equal to the activation energy of the reaction. Furthermore, the colliding species must be oriented in a manner favourable to the necessary rearrangement of atoms and electrons. Thus, according to the collision theory, the rate at which a chemical reaction proceeds is equal to the frequency of effective collisions. Because atomic or molecular frequencies of collisions can be calculated with some degree of accuracy only for gases (by application of the kinetic theory), the application of the collision theory is limited to gas-phase reactions.

The rate for a bimolecular gas-phase reaction, predicted by collision theory is

${\displaystyle r(T)=kn_{\text{A}}n_{\text{B}}=Z\rho \exp \left({\frac {-E_{\text{a}}}{RT}}\right)}{\displaystyle r(T)=kn_{\text{A}}n_{\text{B}}=Z\rho \exp \left({\frac {-E_{\text{a}}}{RT}}\right)}$

where:

k is the rate constant in units of (number of molecules)−1 s−1m3.

nA is the number density of A in the gas in units of m−3.

nB is the number density of B in the gas in units of m−3. E.g. for a gas mixture with gas A concentration 0.1 mol L−1 and B concentration 0.2 mol L−1, the number of density of A is 0.1×6.02×1023÷10−3 = 6.02×1025 m−3, the number of density of B is 0.2×6.02×1023÷10−3 = 1.2×1026 m−3.

Z is the collision frequency in units of m−3s−1.

$\displaystyle \rho }\rho$  is the steric factor.

Ea is the activation energy of the reaction, in units of J mol−1.

T is the temperature in units of K.

R is the gas constant in units of J mol−1K−1.

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