Record the volume of gas produced every 5 seconds. The gaining of energy enables the particles to move around quicker, this increases their chance of colliding but also, the increase in energy increases the possibility of a collision occurring with sufficient energy. The amount of product is directly proportional to the amount of limiting reactant used.
There are many ways on which to speed up the reaction. FIGURE 6: The graph shows the volume of hydrogen produced over time when different amounts of magnesium ribbon are added to dilute hydrochloric acid.
How much hydrogen is formed if the amount of magnesium is doubled to 0. The greater the surface area of the metal the more of its particles are exposed to the acid. Therefore rate of reaction increases with increasing temperature.
Before, we discover the reasons for the above causing an increase in rate, we must first look at what is needed to cause a reaction to occur! Chemical reactions can be very difficult to undo.
Questions 7Look at the graph in Figure 6. The collision must be with sufficient energy. Each experiment run will need 50 cm3.