The reactions with low activation energy area)Slowb)Non-spontaneousc)Fastd)Always spontaneousCorrect answer is option 'C'. Can you explain this answer?

Question

Answer

Low activation energy mean energy reguire for reaction to occur is low so product making is fast

Answer

The correct answer is Option C.

The reactions with low activation energies are always fast whereas the reactions with high activation energy are always slow. The process of speeding up a reaction by reducing its activation energy is known as catalysis, and the factor that's added to lower the activation energy is called a catalyst.

Answer

We can call it as a example of reversible reacn why bcoz it's is the reacn which takes break at every step of reacn an still we can find it at end point with stable products

Answer

Reactions with Low Activation Energy

Introduction:
Activation energy is the minimum amount of energy required for a chemical reaction to occur. It can be thought of as a barrier that reactant molecules must overcome in order to form products. Reactions with low activation energy have a faster rate of reaction compared to reactions with high activation energy.

Explanation:
Reactions with low activation energy are characterized by the following features:

1. Fast Reaction:
Reactions with low activation energy are generally fast. This is because the lower the activation energy, the easier it is for reactant molecules to acquire the necessary energy to overcome the activation barrier and proceed to the product state. As a result, the reaction occurs more quickly.

2. Spontaneity:
Reactions with low activation energy can be both spontaneous and non-spontaneous. Spontaneous reactions are those that occur naturally without the need for external energy input. Non-spontaneous reactions, on the other hand, require an input of energy to occur. Therefore, it is not accurate to say that reactions with low activation energy are always spontaneous.

3. Increased Reactivity:
Low activation energy allows reactant molecules to collide more frequently and with sufficient energy to undergo the reaction. This leads to increased reactivity and a higher likelihood of successful collisions, resulting in a faster reaction rate.

4. Lower Energy Barrier:
Reactions with low activation energy have a lower energy barrier, which means that a larger proportion of reactant molecules possess the required energy to overcome the barrier. Consequently, a higher fraction of collisions between reactant molecules leads to the formation of products.

5. Temperature Dependence:
While low activation energy facilitates faster reactions at all temperatures, the effect is more pronounced at lower temperatures. This is because at higher temperatures, a larger proportion of reactant molecules already possess the required energy to overcome the activation barrier, regardless of the activation energy.

In conclusion, reactions with low activation energy exhibit a fast reaction rate, increased reactivity, and a lower energy barrier. While these reactions can be both spontaneous and non-spontaneous, they are generally associated with faster reaction rates due to the ease of overcoming the activation barrier.

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