Which of the following is true for a reaction | vedclass

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(B) According to collision theory,not every collision between reactant molecules leads to a chemical reaction. Only those collisions that possess ener

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It may be expected that rate of reaction is equal to rate of collision.

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(B) According to collision theory,not every collision between reactant molecules leads to a chemical reaction. Only those collisions that possess energy greater than the threshold energy and have proper orientation result in a product.For gas phase reactions,the calculated number of collisions is much higher than the observed rate of reaction.Therefore,the statement that it may be expected that the rate of reaction is equal to the rate of collision is the correct premise for the theory's development before accounting for the steric factor and activation energy.

Which of the following is true for a reaction as per collision theory?

Similar Questions

All energetically effective collisions do not result in a chemical change. Explain with the help of an example.

According to the collision theory,which of the following statements is $NOT$ correct?

For a reaction taking place in three steps at the same temperature,the overall rate constant is $K = \frac{K_1 K_2}{K_3}$. If $E_{a1}$,$E_{a2}$,and $E_{a3}$ are $40 \ kJ/mol$,$50 \ kJ/mol$,and $60 \ kJ/mol$ respectively,the overall activation energy $E_a$ is . . . . . . $kJ/mol$.

For a first-order reaction,if the rate constant is $k_1$ at temperature $T_1$ and $k_2$ at temperature $T_2$,which of the following relations is correct? ($E_a$ = activation energy)

For a first-order reaction $A \to P$,the rate constant equation is given by $\log K = -2000 \, (1/T) + 6.0$. The pre-exponential factor $A$ and the activation energy $E_a$ are,respectively:

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