Question

On increasing the temperature of the reacting system by 10 degrees the rate of reaction almost doubles. The most appropriate reason for this is
A. collision frequency increases
B. activation energy decreases by increases in temperature
C. the fraction of molecules having energy equal to threshold energy or more increase
D. the value of threshold energy decreases

Answer 1

The above problem can be resolved using the concept of entropy of any system. The entropy is one of the fundamentals of thermodynamics, that is used to predict the randomness of particles at any specific temperature. The temperature plays a vital role in this because at a higher temperature; the elections are at higher energy levels; this causes the increased vibration of particles.

Complete step by step answer: r
Consider a container of volume V. In which there are some molecules of hydrogen gas and some molecules of the oxygen gas is present. Let T be the value of temperature of the container at initial state.
Now, when the temperature of the container is increased by subsequent heating, then the rate of reaction among the molecules, inside the container also increases. And the major reason behind this is that the randomness or the entropy of the molecules also increases. And this causes the increased frequency of collision of molecules. This collision brings about the faster reaction at a much higher interaction rate.
Therefore, by increasing the temperature of the reacting system by 10 degrees the rate of reaction almost doubles. The most appropriate reason for this is the increased collision frequency and option (A) is correct.

Note: To solve the given problem, one must be aware of the concepts and applications of entropy. When the temperature of an atom is raised, it starts vibrating at a much higher rate, and this causes the reactivity rate to be increased. Due to this, the rate of formation is raised, and hence this all parameters contribute to entropy.