Question

Why does increasing the temperature of two reactants in solution make a reaction proceed more quickly? a. at higher temperatures, the particles move more quickly and collide more often. b. increasing the temperature reduces the activation energy of the reaction. c. when the particles move more quickly, they can collide in a better orientation. d. increasing the temperature increases the concentration of the particles and the speed of the reaction.

Answer 1

Raising the temperature of reactants in solution increases the reaction rate by boosting the kinetic energy of the particles, leading to more frequent and energetic collisions that can overcome the activation energy barrier.

Step-by-step explanation:

Increasing the temperature of two reactants in solution speeds up the reaction primarily because it increases the kinetic energy of the particles. Higher kinetic energy means that the particles move faster, and thus, collide more frequently and with greater force. These more frequent and forceful collisions are more likely to overcome the activation energy barrier, leading to an increased number of effective collisions and consequently, a faster reaction rate.

While increasing temperature also can increase the collision orientation, the main reasons for the increased reaction rate are the higher kinetic energy, resulting in more collisions and more energy provided to the particles that do collide, allowing more of them to reach the activation energy needed for the reaction to occur.

Answer 2

Increasing the temperature of reactants in a solution leads to a higher reaction rate because it causes the particles to move faster and collide more often, which increases the number of effective collisions necessary to surpass the activation energy barrier. So the correcct option is a.

Step-by-step explanation:

The question asks why increasing the temperature of two reactants in solution makes a reaction proceed more quickly. The answer is that at higher temperatures, the particles move more quickly and collide more often (a). This increase in particle speed results in a greater frequency of collisions and thus more chances for reactions to occur. It is important to note, that while increasing the temperature does not reduce the activation energy of the reaction (b), it does increase the kinetic energy of the particles. This allows more particles to surpass the activation energy barrier needed for a reaction to occur. Additionally, the orientation of the particles upon collision is not affected by the temperature (c), and increasing the temperature does not change the concentration of the particles (d).