Activation energy is
the heat released in a reaction
the energy barrier between reactants and products
the energy given off when reactants collide***
generally very high for a reaction that takes place rapidly
all of these were correct except 3, 3 was A: More H2CO3 is produced
1 b
2 c
3 c
4 c
5 d
6 c
7 b
8 c
9 b
3 is a but everything else is right
1 b
2 c
3 a
4 c
5 d
6 c
7 b
8 c
9 b
100%
I meant to mark B as my answer sorry
B is correct
Activation energy is the energy barrier between reactants and products in a chemical reaction. It represents the minimum amount of energy required for a reaction to occur. The correct answer is: the energy barrier between reactants and products.
To further understand activation energy, it is important to consider the concept of a reaction coordinate diagram. This diagram visualizes the progress of a chemical reaction as the reactants are converted into products. On the diagram, the energy of the system is plotted along the y-axis, while the reaction progress is depicted along the x-axis.
The reactants are located at the beginning of the reaction coordinate, and the products are positioned at the end. However, before the reactants can be converted into products, they must overcome an energy barrier, which is the activation energy.
The activation energy is crucial because it determines the rate at which a reaction occurs. Generally, reactions with higher activation energies tend to take place more slowly, precisely because a larger amount of energy is needed for the reactants to surpass the barrier and reach the product state.
It is important to note that activation energy is not the heat released or energy given off during a reaction. This misconception arises because when reactants collide, they may release heat or energy. However, the activation energy specifically refers to the energy required to initiate the reaction, not the energy released after the reaction has started.