1. Reacting molecules or ions in a solution at room temperature are in constant motion and collide. Some collisions lead to formation of product and some don't. what determines a reaction will take place.

2. Is there any evidence in the experiment that would support the notion that the same material in a powder form would react faster than in a lump form?

3. The decomposition of hydrogen peroxide, H2O2, yields water and oxygen gas.
a) Write a balanced equation for this decomposition reaction.

b) The reaction is faster with the addition of manganese dioxide, MnO2. Should this chemical appear in the balanced equation? What is the purpose of manganese dioxide?

4. For the reaction shown in equation (1) in the background section, what should you observe happening to the gas produced.
a) If the concentration of the HCl increased?

b) If the solid calcium carbonate is in powder form?

5. The temperature of a reaction was increased from 20 to 40 0C. You were determining the rate of reaction at each of the two temperatures. The second reaction should be faster by how much?