Question

Chemical reactions occur when molecules or atoms collide, the bonds between atoms are broken, and new bonds are formed. Breaking the bonds of the reactants requires energy; bond formation releases energy. Which of the following statements regarding energy changes during a reaction are true? The activation energy ($E_a$) is the energy difference between the energy of the products and the energy of the reactants. If the energy of the products is lower than the energy of the reactants, the reaction is endothermic. When the activation energy is high, the reaction rate is fast. Decreasing the temperature decreases the kinetic energy of the reactants, and the reaction goes more slowly. Reactants must collide, with proper orientation, with energy greater than or equal to the activation energy for a reaction to occur. Increasing the amount of reactants increases the number of collisions, and the reaction goes faster. The energy of a collision between atoms or molecules must be greater than or equal to the activation energy ($E_a$) for bonds to be broken.

          Chemical reactions occur when molecules or atoms collide, the bonds between atoms are broken, and new
bonds are formed. Breaking the bonds of the reactants requires energy; bond formation releases energy.
Which of the following statements regarding energy changes during a reaction are true?
The activation energy ($E_a$) is the energy difference between the energy of the products and
the energy of the reactants.
If the energy of the products is lower than the energy of the reactants, the reaction is
endothermic.
When the activation energy is high, the reaction rate is fast.
Decreasing the temperature decreases the kinetic energy of the reactants, and the
reaction goes more slowly.
Reactants must collide, with proper orientation, with energy greater than or equal to the
activation energy for a reaction to occur.
Increasing the amount of reactants increases the number of collisions, and the reaction
goes faster.
The energy of a collision between atoms or molecules must be greater than or equal to the
activation energy ($E_a$) for bonds to be broken.

Chemical reactions occur when molecules or atoms collide, the bonds between atoms are broken, and new
bonds are formed. Breaking the bonds of the reactants requires energy; bond formation releases energy.
Which of the following statements regarding energy changes during a reaction are true?
The activation energy (Ea) is the energy difference between the energy of the products and
the energy of the reactants.
If the energy of the products is lower than the energy of the reactants, the reaction is
endothermic.
When the activation energy is high, the reaction rate is fast.
Decreasing the temperature decreases the kinetic energy of the reactants, and the
reaction goes more slowly.
Reactants must collide, with proper orientation, with energy greater than or equal to the
activation energy for a reaction to occur.
Increasing the amount of reactants increases the number of collisions, and the reaction
goes faster.
The energy of a collision between atoms or molecules must be greater than or equal to the
activation energy (Ea) for bonds to be broken.

Added by Kevin O.

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