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In the Arrhenius equation equation,the B...

In the Arrhenius equation equation,the Boltzmann factor `e^(Ea//RT)` represents the…………..of the molecules possessing energ in excess of activation energy

A

number

B

fraction

C

weight

D

percentage

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The correct Answer is:
B
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Arrhenius studied the effect of temperature on the rate of a reaction and postulated that rate constant varies with temperature exponentially as k=Ae^(-E_(a)//RT) . For most of the reactions it was found that the temperature coefficient of the reaction lies between 2 to 3. The method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied by studying how much the rate of reaction changes in the presence of catalyst. In most of the cases, it is observed that catalyst lowers the activationenergy barrier and increases the rate of reaction. The pre-exponential factor in the Arrhenius equation of a second order reaction has the units

Arrhenius studied the effect of temperature on the rate of a reaction and postulated that rate constant varies with temperature exponentially as k=Ae^(-E_(a)//RT) . For most of the reactions it was found that the temperature coefficient of the reaction lies between 2 to 3. The method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied by studying how much the rate of reaction changes in the presence of catalyst. In most of the cases, it is observed that catalyst lowers the activationenergy barrier and increases the rate of reaction. Which of the following plot will be linear?

Arrhenius studied the effect of temperature on the rate of a reaction and postulated that rate constant varies with temperature exponentially as k=Ae^(-E_(a)//RT) . For most of the reactions it was found that the temperature coefficient of the reaction lies between 2 to 3. The method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied by studying how much the rate of reaction changes in the presence of catalyst. In most of the cases, it is observed that catalyst lowers the activationenergy barrier and increases the rate of reaction. If the rate oc reaction grwos 15.6 times on increasing the temperature by 30 K the temperature coefficient of the reaction will be nearly

On the basis of the postulates of kinetic theory of gases, it is possible to derive the mathematical expression, commonly known as kinetic gas equation. PV = 1/3 m n u^3? where, P= Pressure of the gas, V a volume of the gas, m=Mass of a molecule, n = Number of molecules present in the given amount of a gas and u = root mean square speed For one mole of gas, PV = RT and n=N_A 1/3 m N_a u^2 = RT or 2/3 .1/2m N_A u^2 = N_A [1/2mN_Au^2 = KE "per mole"] ,2/3K.E. = RT implies K.E. 3/2RT Average kinetic energy per mol does not depend on the nature of the gas but depends only on temperature. This, when two gases are mixed at the same temperature, there will be no rise or decrease in temperature unless both react chemically. Average kinetic energy per molecule = ("Average K.E. per mole")/N = 3/2(RT)/(N) implies 3/2kT where k is the Boltzmann constant In deriving the kinetic gas equation, the use of the root mean square speed of the molecules is done, hecause it is

The rate constant K_(1) of a reaction is found to be double that of rate constant K_(2) of another reaction. The relationship between corresponding activation energies of the two reactions E_(1) and E_(2) can be represented as

The total energy of molecules is divided equally amongst the various degrees of freedom of a molecule. The distribution of kinetic energy along x, y, z axis are E_(K_(x)), E_(K_(y)), E_(K_(z)) Total K.e =E_(K_(x)) + E_(K_(y)) + E_(K_(z)) Since the motion of molecule is equally probable in all the three directions, therefore E_(K_(x)) = E_(K_(y)) = E_(K_(z)) =1/3 E_(K) =1/3 xx 3/2 kT = 1/2 kT , where k =R/N_(A) = Botzman constant. K.E. = 1/2 kT per molecule or =1/2 RT per mole. In vibration motion, molecules possess both kinetic energy as well as potential energy. This means energy of vibration involves two degrees of fiuedom. Vibration energy =2 xx 1/2kT =2 xx 1/2RT [ therefore two degrees of freedom per mole] If the gas molecules have n_(1) translational degrees of freedom, n_2 rotational degrees of freedom and n_(3) vibrational degrees of freedom, that total energy = n_(1)[(kT)/2] + n_(2) [(kT)/2] + n_(3) [(kT)/2] xx 2 Where 'n' is atomicity of gas. The rotational kinetic energy of H20 molecule is equal to

The total energy of molecules is divided equally amongst the various degrees of freedom of a molecule. The distribution of kinetic energy along x, y, z axis are E_(K_(x)), E_(K_(y)), E_(K_(z)) Total K.e =E_(K_(x)) + E_(K_(y)) + E_(K_(z)) Since the motion of molecule is equally probable in all the three directions, therefore E_(K_(x)) = E_(K_(y)) = E_(K_(z)) =1/3 E_(K) =1/3 xx 3/2 kT = 1/2 kT , where k =R/N_(A) = Botzman constant. K.E. = 1/2 kT per molecule or =1/2 RT per mole. In vibration motion, molecules possess both kinetic energy as well as potential energy. This means energy of vibration involves two degrees of fiuedom. Vibration energy =2 xx 1/2kT =2 xx 1/2RT [ therefore two degrees of freedom per mole] If the gas molecules have n_(1) translational degrees of freedom, n_2 rotational degrees of freedom and n_(3) vibrational degrees of freedom, that total energy = n_(1)[(kT)/2] + n_(2) [(kT)/2] + n_(3) [(kT)/2] xx 2 Where 'n' is atomicity of gas. The vibrational kinetic energy of CO_2 molecule is

AAKASH SERIES-CHEMICAL KINETICS-Objective Exercise - 4 (Assertion (A) & Reason (R) Type Questions)
  1. In the Arrhenius equation equation,the Boltzmann factor e^(Ea//RT) rep...

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  2. (A) Spontaneous reaction may be slow or fast. (R ) Spontaneous natur...

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  3. A: Rate of reaction increases with increasse in concentration of react...

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  4. A: Hydrolysis of an ester is a slow reaction R: Reactions between co...

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  5. (A) All collisions lead to chemical reaction (R ) All molecules brin...

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  6. A: Order of reaction is evaluated from the mechanism of a reaction ...

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  7. A: A catalyst increases the rate of a reaction. R: In presence of a ...

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  8. (A) The rate of the reaction is the rate of change of concentration of...

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  9. (A ) If in a zero order reaction, the concentration of the reactant is...

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  10. (A) The addition of catalyst lowers the activation barrier, yet there ...

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  11. (A) In a multiple reaction, the rate determining step is the fast step...

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  12. (A) Half-life period of a reaction of first order is independent of in...

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  13. (A) Order of recation is related to molecularity of reaction (R ) Mo...

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  14. (A) The rate law equation can be found only by experiment. (R ) Rate...

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  15. (A) Reactions of higher order are rare (R ) The chances of multimole...

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  16. (A) Rate of reaction increases with increase in temperature. (R ) Nu...

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  17. (A) The mass of the products formed in a reaction depends upon the lim...

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  18. (A) Order with respect to any reactant or product can be zero or posit...

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  19. (A) The rections 2NO+O(2) to 2NO(2) and 2CO+O(2) to 2CO(2), proceed at...

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  20. (A) Hydrolysis of ethyl acetate in presence of acid is a reaction of f...

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  21. (A) The rate of reaction is always negative. (R ) Minus sign used in...

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