2. The table below shows how the volume of carbon dioxide collected varied against time when small and large calcium carbonate chips were added to an excess of hydrochloric acid.
(c) How long did each experiment take to go to completion? How can you tell from the graph?
Read from the graph the point at which the curves become horizontal
Kinetics Summary Worksheet
2. The table below shows how the volume of carbon dioxide collected varied against time when small and large calcium carbonate chips were added to an excess of hydrochloric acid.
(d) What are possible units of rate of reaction in this experiment?
2. The table below shows how the volume of carbon dioxide collected varied against time when small and large calcium carbonate chips were added to an excess of hydrochloric acid.
(e) Write a chemical reaction for this process.
CaCO3(s) + 2HCl(aq) CaCl2(aq) + CO2(g) + H2O(l)
(f) Why is gas produced at different rates in the two different experiments?
Size of chips dictates surface area. The smaller the chips, the greater the surface area and the faster the rate of reaction
Kinetics Summary Worksheet
3. Kinetic results for a reaction involving substance A are shown below.
(b) What is the order of this reaction with respect to A?
First Order
Kinetics Summary Worksheet
3. Kinetic results for a reaction involving substance A are shown below.
(c) Use your graph to calculate the half-life for this reaction.
Approximately 7 minutes.
Kinetics Summary Worksheet
3. Kinetic results for a reaction involving substance A are shown below.
(d) Given that in this reaction A reacts with G, and that the order with respect to G is second, write the rate equation for this reaction.
Rate = k [A][G]2
Kinetics Summary Worksheet
4.
(b) What is the order with respect to B in this reaction?
Zero
(c) What can be said about the rate of consumption of B in this reaction?
It is constant.
Kinetics Summary Worksheet
5.
(b) What is the order with respect to X in this reaction?
