Which statement is incorrect for collision theory?
- AThe reactant experiencing fruitful collisions are converted to products.
- BThere must be a certain minimum energy for the reactant experiencing collision.
- CThe collision of the reactant molecules should be from any direction.
- DThe collision between the reacting molecules is essential.
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Similar Questions
For an exothermic reaction,the following two steps are involved:
Step $1$: $A + B \to I$ $(slow)$
Step $2$: $I \to AB$ $(fast)$
Which of the following graphs correctly represents this reaction?
Step $1$: $A + B \to I$ $(slow)$
Step $2$: $I \to AB$ $(fast)$
Which of the following graphs correctly represents this reaction?
Medium
View SolutionConsider the following graph of the kinetic energy distribution among molecules at temperature $T$. If the temperature is increased,how would the resulting graph differ from the one above?
Medium
View SolutionActivation energy of any reaction depends on
Easy
View Solution$A$ reaction takes place in three steps with individual rate constant and activation energy,
Step Rate constant and Activation energy $Step \ 1$ $k_1, E_{a_1} = 180 \ kJ \ mol^{-1}$ $Step \ 2$ $k_2, E_{a_2} = 80 \ kJ \ mol^{-1}$ $Step \ 3$ $k_3, E_{a_3} = 50 \ kJ \ mol^{-1}$
Overall rate constant,$k = (k_1 k_2 / k_3)^{2/3}$. The overall activation energy of the reaction will be ........ $kJ \ mol^{-1}$.
| Step | Rate constant and Activation energy |
| $Step \ 1$ | $k_1, E_{a_1} = 180 \ kJ \ mol^{-1}$ |
| $Step \ 2$ | $k_2, E_{a_2} = 80 \ kJ \ mol^{-1}$ |
| $Step \ 3$ | $k_3, E_{a_3} = 50 \ kJ \ mol^{-1}$ |
Overall rate constant,$k = (k_1 k_2 / k_3)^{2/3}$. The overall activation energy of the reaction will be ........ $kJ \ mol^{-1}$.
Difficult
View SolutionAt a constant temperature,the activation energy of a reaction is found to be $2.303 \, RT \, J \, mol^{-1}$. The ratio of the rate constant to the Arrhenius constant will be $......$.
Medium
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