Gcse chemistry coursework magnesium hydrochloric acid

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.

magnesium and hydrochloric acid equation

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.

Magnesium ribbon and hydrochloric acid experiment concentration

Why does the line flatten out? Ensure that there are no naked flames. The gradient slope of the line shows how fast the reaction is. The Effect of a Catalyst Some reactions may be speeded up by using a catalyst. It is important in this practical to use appropriate apparatus to make and record a range of measurements accurately, including mass, time and volume. Clean if necessary by rubbing lengths of the ribbon with fine sandpaper to remove the layer of oxidation. The volume of hydrogen gas produced is measured over a few minutes, and the results are used to plot a graph. Eye protection must be worn. Timing how long it takes for the magnesium to dissolve. However the acid is in excess, so it is mainly the loss of magnesium surface area becomes smaller that causes the change in the rate. More collisions mean a quicker rate of reaction.
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The rate of reaction of magnesium with hydrochloric acid