Maxwell-Boltzmann Distribution and Reaction Rates

The video explains collision theory, emphasizing that particles must collide with proper orientation and sufficient kinetic energy to overcome the activation energy barrier. An energy profile illustrates this concept, and a golf ball analogy is used to further explain energy barriers. The Maxwell-Boltzmann distribution is introduced to show the range of particle speeds in a gas sample. The video concludes by discussing how increasing temperature affects the distribution, leading to more particles with enough energy to react, thus increasing the reaction rate.

What is a key requirement for particles to react according to collision theory?

• They must collide with sufficient kinetic energy.

• They must collide with any orientation.

• They must collide without any energy.

• They must collide at low temperatures.

What does the activation energy represent in a reaction's energy profile?

• The energy of the reactants.

• The energy of the products.

• The energy lost during the reaction.

• The minimum energy required to start a reaction.

In the golf ball analogy, what does the hill represent?

• Kinetic energy

• Thermal energy

• Potential energy

• Activation energy

What does the Maxwell-Boltzmann distribution curve show?

• The range of speeds of particles in a gas.

• The temperature of a liquid.

• The energy levels of electrons in an atom.

• The number of particles in a solid.

What does the area under the Maxwell-Boltzmann distribution curve represent?

• The speed of the fastest particle.

• The number of particles in the sample.

• The temperature of the gas.

• The total energy of the system.

What is the relationship between particle speed and kinetic energy?

• Speed is inversely proportional to kinetic energy.

• Speed and kinetic energy are unrelated.

• Higher speed means higher kinetic energy.

• Higher speed means lower kinetic energy.

How does increasing temperature affect the Maxwell-Boltzmann distribution?

• The peak height decreases and the curve narrows.

• The peak height remains the same and the curve narrows.

• The peak height decreases and the curve broadens.

• The peak height increases and the curve narrows.

What happens to the number of particles with enough energy to react when temperature increases?

• It remains the same.

• It fluctuates randomly.

• It decreases.

• It increases.

Why does increasing temperature increase the rate of reaction?

• It reduces the number of particles.

• It changes the orientation of particles.

• It increases the number of particles with sufficient energy.

• It decreases the activation energy.

What remains unchanged when the temperature of a gas sample is increased?

• The energy of the products.

• The activation energy.

• The speed of all particles.

• The number of particles.