Time (in minutes | 0 | 5 | 10 | 15 | 20 | 25 | 30 | 35 |
Volume of oxygen with catalyst A (in cm3) | 0 | 4 | 8 | 12 | 16 | 17 | 18 | 18 |
Volume of oxygen with catalyst B (in cm3) | 0 | 5 | 10 | 15 | 16.5 | 18 | 18 | 18 |
a. Plot a graph to show both sets of results
c. Explain why both experiments were done at the same temperature
To keep it a fair test and also catalyst may work at different rates if they were under different temperatures
d. Explain why both sets of figures stop at 18 cm3 of oxygen
e. Add a line to your graph to show the shape of the graph you would obtain for the uncatalysed reaction.
4. The graph below shows the results of three experiments involving the reaction of magnesium and dilute hydrochloric acid
a. Which experiment has the fastest rate at the start? 1
b. Which experiment produced the greatest final volume of gas? 2
c. Which experiment used the most concentrated acid? 1
5. Copper (II) oxide catalyses the decomposition of hydrogen peroxide. 0.5 g of the copper oxide was added to a flask containing 100 ml of hydrogen peroxide. A gas was released. It was collected and its volume noted every 10 seconds. The table below shows the results:
Time (in seconds) | 0 | 10 | 20 | 30 | 40 | 50 | 60 | 70 | 80 | 90 |
Volume (in ml) | 0 | 18 | 30 | 40 | 48 | 53 | 57 | 58 | 58 | 58 |
a. What is a catalyst? A catalyst is a substance which increases the rate of a reaction but is not affected by some sort of change, it isn't used up.
b. Draw a diagram of suitable apparatus that you would use to carry out this experiment.
c. Name the gas that is formed. Oxygen + (water)
d. Write a balanced chemical equation for the decomposition of hydrogen peroxide. H2O2 --> H2+O2
e. Plot a graph of the volume of gas against time.
f. What happen to the concentration of hydrogen peroxide as the reaction proceeds? The concentration decreases
g. What chemicals are present in the flask after 90 seconds? water and catalyst
h. What mass of copper (II) oxide would be left in the flask at the end of the reacting? The same mass
i. Sketch on your graph the curve that might be obtained when:
i) 1.0 g of copper (II) oxide is used (green line on graph)
ii) 0.5 g of copper (II) oxide is used in a hydrogen peroxide solution of a lower concentration
6. The equation for the reaction between calcium carbonate and hydrochloric acid is
CaCO3 (s) + 2 HCl (aq) ¾® CaCl2 (aq) + H2 O (l) + CO2 (g)
Two different 10.0 g samples of calcium carbonate were reacted at 25 C with excess hydrochloric acid for a period of 6 minutes. One of the samples was in the form of large lumps and the other consisted of small lumps.
Mass of flask and contents (in g) | ||
Time (min) | Large lumps | small lumps |
0 | 112.4 | 111.6 |
0.5 | 111.6 | 109.2 |
1 | 111.1 | 108.3 |
2 | 110.2 | 107.4 |
3 | 109.6 | 107.2 |
4 | 109.1 | 107.2 |
5 | 108.7 | 107.2 |
6 | 108.5 | 107.2 |
a. Draw a diagram of apparatus which would be suitable for carrying out this experiment.
b. Explain why the mass of each flask and contents decreases. The mass of the contents decrease because hydrochloric acid displaces the calcium carbonate to form calcium chloride. Also gas is given off during the experiment.
c. Draw two graphs on the same set of axes to show how the total loss of mass changes with time for each sample.
d. On the same grid sketch the graph you would expect to obtain if the experiment was repeated with 10g of powdered calcium carbonate
