Question

The reason for almost doubling the rate of reaction on
increasing the temperature of the reaction system by 10°C is
(a) The value of threshold energy increases
(b) Collision frequency increases
(c) The fraction of the molecule having energy equal to
threshold energy or more increases
(d) Activation energy decreases

Answer 1

Answer:

activity energy decrease

please mark it as BRAINIEST ANSWER

Answer 2

Let us answer it

Option b and c both are correct

Explanation:

The rate of reaction is the time taken for the reactants to transform into products .

It is seen that rate of reaction depends upon many factors :

1. Out of which temperature is also one of the factor.For the reaction to occur the reactant molecules must collide efficiently .
2. As the collision frequency  increases , the rate also increases .
3. This  collision frequency can be increased by increasing the energies of reactant molecules and that can be done by increasing the temperature .
4. On increasing the energies of reactant molecules due to increase in temperature : The fraction of the molecule having energy equal to  threshold energy or more increases. So , that more number of reactants can cross energy barrier .
5. Therefore , we can say that on increasing the temperature , collision frequency increases , also  The fraction of the molecule having energy equal to  threshold energy or more increases .

Hence rate of reaction almost doubles .