Improve Reaction Speed :Temperature and Catalysts

The video tutorial discusses the decomposition of dinitrogen pentoxide and how temperature affects the reaction rate. It explains that higher temperatures increase the number of molecules with energy greater than the activation energy, thus speeding up the reaction. The role of catalysts, such as manganese dioxide, in lowering activation energy and increasing reaction rates is also covered. Additionally, the tutorial highlights how the surface area of reactants, like powdered zinc, influences the rate of reaction by increasing collision frequency.

What happens to the rate of reaction when the temperature is increased from 20°C to 30°C?

• The rate of reaction decreases.

• The rate of reaction remains the same.

• The rate of reaction increases.

• The reaction stops completely.

How does a catalyst affect the activation energy of a reaction?

• It doubles the activation energy.

• It has no effect on the activation energy.

• It decreases the activation energy.

• It increases the activation energy.

Which of the following is true about catalysts?

• They increase the rate of reaction without being consumed.

• They decrease the rate of reaction.

• They are consumed in the reaction.

• They increase the activation energy.

Why does powdered zinc react faster with hydrochloric acid compared to larger zinc pieces?

• Powdered zinc is more reactive.

• Larger zinc pieces have a greater surface area.

• Larger zinc pieces are more reactive.

• Powdered zinc has a greater surface area.

What is the relationship between surface area and the rate of reaction?

• Surface area has no effect on the rate of reaction.

• Rate of reaction decreases with increased surface area.

• Rate of reaction is directly proportional to surface area.

• Rate of reaction is inversely proportional to surface area.