Chemical reactions occur when molecules or atoms collide, the bonds between atom

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? Decreasing the temperature decrease the kinetic energy of the reactants, and the reaction goes more slowly. When the activation energy is high, the reaction rate is fast. If the energy of the products is higher than the energy of the reactants, the reaction is exothermic. Increasing the amount of reactants increases the number of collisions, and the reaction goes faster. Reactants must collide, with proper orientation, with energy greater than or equal to the activation energy for a reaction to occur. 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. The activation energy (E_a) is the energy difference between the energy of the products and the energy of the reactants.

Explanation / Answer

True statements
1. Decreasing the temperature decreases the kinetic energy of the reactants and
reaction goes more slowly.
3. Increasing the amount of reactants increases the number of collisions and the
reaction goes faster.
5. Reactants must collide with proper orientation with energy greater than or equal
to the activation energy for a reaction to occur.
6. The energy of a collision between atoms or molecules must be greater than or equal
to the activation energy for bonds to be broken

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