A student investigated how the rate of reaction is affected by concentration in the reaction between calcium carbonate and hydrochloric acid.
The method they used is shown below.
- Pour 25 cm3 of hydrochloric acid into a conical flask
- Add 5.0 g of calcium carbonate powder to the conical flask
- Attach a gas syringe to the conical flask
- Measure the volume of gas produced every 30 seconds for 150 seconds
- Repeat steps 1 to 4 two more times
- Repeat steps 1 to 5 with a higher concentration of hydrochloric acid
What piece of equipment would be most suitable to measure the volume of hydrochloric acid?
Tick (✓) one box.
Beaker | |
Measuring cylinder | |
Conical flask | |
Test tube |
Draw lines from each variable to identify two control variables and one dependent variable in this investigation.
Table 1 shows the results collected in the investigation for a low concentration of hydrochloric acid.
Table 1
Volume of gas collected in cm3 |
Time in seconds | Test 1 | Test 2 | Test 3 | Mean |
0 | 0 | 0 | 0 | 0 |
30 | 49 | 47 | 48 | 48 |
60 | 78 | 39 | 80 | 79 |
90 | 93 | 91 | 92 | 92 |
120 | 98 | 97 | 98 | 98 |
150 | 100 | 100 | 100 | 100 |
One result was anomalous.
Identify which result by stating the time in seconds and the test where this occurred.
Time in seconds: _______________________________
Test: __________________________________
Plot the results from Table 1 onto Figure 1.
Use the mean volume of gas collected in cm3.
Draw a line of best fit.
Figure 1
The student repeated the experiment for a higher concentration of hydrochloric acid.
What would happen to the rate of reaction?
Tick (✓) one box.
Remain the same | |
Become quicker | |
Become slower |
Did this page help you?