Y9A Collision Theory in Chemistry

What is the main idea of collision theory in reaction kinetics?

• Particles must collide with enough energy and correct orientation to react.

• All collisions between particles result in a chemical reaction.

• Reactions occur only at high temperatures.

• Particles must collide with low energy to react.

In the context of gases, what happens when you double the amount of gas?

• The number of collisions increases, speeding up the reaction.

• The number of collisions decreases, slowing down the reaction.

• The reaction stops completely.

• The reaction rate remains unchanged.

What is activation energy?

• The smallest amount of energy needed for a reaction to start.

• The energy released during a reaction.

• The energy required to stop a reaction.

• The energy needed to maintain a reaction.

The Arrhenius equation shows that increasing the temperature or lowering the activation energy will make the reaction (a)   .

What factors affect collision frequency in a gas?

• Size of the space, number of particles, and their speed.

• Color of the gas, shape of the container, and pressure.

• Type of gas, color of the container, and volume.

• Temperature, color of the gas, and type of container.

In the Haber process, how can the reaction be sped up?

• By increasing pressure or temperature.

• By decreasing pressure or temperature.

• By adding more reactants without changing conditions.

• By using a larger container.

For a reaction to occur, particles must collide with enough energy to overcome what?

• Activation energy.

• Collision frequency.

• Reaction rate.

• Temperature threshold.