LT6.1 Reaction Rates

Front

What is the effect of decreasing temperature on the rate of reaction?

Back

Decreasing temperature lowers the rate of reaction by reducing the energy and speed of the particles, leading to fewer effective collisions.

Front

How does increasing temperature affect reaction rates?

Back

Increasing temperature increases the rate of reaction by providing more energy to the particles, resulting in more frequent and effective collisions.

Front

What happens to the rate of reaction when the concentration of reactants is increased?

Back

Increasing the concentration of reactants increases the rate of reaction because it raises the frequency of particle collisions due to more collision sites.

Front

Why does crushing a solid reactant increase the rate of reaction?

Back

Crushing a solid reactant increases the surface area, allowing more particles to collide with the other reactants, thus speeding up the reaction.

Front

What is the role of catalysts in chemical reactions?

Back

Catalysts increase the rate of reaction by lowering the activation energy required for the reaction to occur without being consumed in the process.

Front

Define activation energy.

Back

Activation energy is the minimum energy required for reactants to collide and form products in a chemical reaction.

Front

What is the relationship between particle size and reaction rate?

Back

Smaller particle size increases the reaction rate because it provides a larger surface area for collisions.

Front

How does stirring a reaction mixture affect the rate of reaction?

Back

Stirring increases the rate of reaction by distributing the reactants more evenly and increasing the frequency of collisions.

Front

What is the effect of pressure on the rate of reaction for gases?

Back

Increasing pressure on gaseous reactants increases the rate of reaction by reducing the volume and increasing the concentration of the gas particles.

Front

Explain why more effective collisions lead to a faster reaction rate.

Back

More effective collisions occur when particles collide with sufficient energy and proper orientation, leading to the formation of products.