Hydrochloric Acid Affect The Rate Of Reaction
Investigate the effect of concentration on the rate of a reaction
Research question: To what extent does the concentration of hydrochloric acid affect the rate of the following reaction: 2 HCl(aq) + CaCO3(s) → CaCl2(aq) + H2O(l) + CO2(g)
Data Collection and Processing:
Table1: Different volumes of Co2 gas produced by Different concentrations of HCL acid.
Volume of CO2gas formed from 5 different concentrations of HCL acid ±0.5ml
5 different concentrations of HCL acid (Mol) ±0.5ml
Time (sec) ±0.1 0.25mol 0.50mol 1.0mol 1.5mol 2.0mol
0.00 0.00 0.00 0.00 0.00 0.00
10 2.00 5.00 6.00 7.00 8.00
20 4.00 9.00 12.00 13.00 15.00
30 6.00 13.00 16.00 19.00 21.00
40 7.00 16.50 20.00 23.50 26.00
50 7.50 19.00 23.00 26.50 29.00
60 8.00 21.50 25.00 28.00 31.00 …show more content…
• Volume of HCL used: 10ml ±0.5
• Mass of the cup: 0.29g ±0.
Table 2: Rate of reaction produced by different concentrations of HCL acid.
5 different concentration of HCL used (Mol) ±0.5 Volume of Co2 Gas produced in 1 minute (ml) ±0.5 Rate of Reaction (ml/s)
0.25 8.00 0.13
0.50 21.50 0.36
1.00 25.00 0.42
1.50 28.00 0.47
2.00 31.00 0.52
Sample Calculations:
• In the experiment, the time was calculated by using a stopwatch with an uncertainty of ±0.1sec.
• The volume of HCL acid was calculated through measuring cylinder with an uncertainty of ±0.5ml.
• Rate of reaction: Volume of CO2 gas produced in 1 minute/60sec
Example: For 0.25mol concentration of HCL acid, the volume of Co2 gas produced in one minute was= …show more content…
From the graph, we can see that the gradient of the concentration of 2.0mol of HCL acid is the steepest. While, the gradient of the concentration of 0.25mol is the lowest.
Conclusion:
From the data tables and graph, we can conclude that as the concentration increases, the rate of reaction also increases. This is because as the concentration is increased, the number of particles or atoms in the same volume is also increases. Due to that, the chances of collisions between the atoms or particles also increases and thus, the rate of reaction.
Research question: To what extent does the concentration of hydrochloric acid affect the rate of the following reaction: 2 HCl(aq) + CaCO3(s) → CaCl2(aq) + H2O(l) + CO2(g)
Data Collection and Processing:
Table1: Different volumes of Co2 gas produced by Different concentrations of HCL acid.
Volume of CO2gas formed from 5 different concentrations of HCL acid ±0.5ml
5 different concentrations of HCL acid (Mol) ±0.5ml
Time (sec) ±0.1 0.25mol 0.50mol 1.0mol 1.5mol 2.0mol
0.00 0.00 0.00 0.00 0.00 0.00
10 2.00 5.00 6.00 7.00 8.00
20 4.00 9.00 12.00 13.00 15.00
30 6.00 13.00 16.00 19.00 21.00
40 7.00 16.50 20.00 23.50 26.00
50 7.50 19.00 23.00 26.50 29.00
60 8.00 21.50 25.00 28.00 31.00 …show more content…
• Volume of HCL used: 10ml ±0.5
• Mass of the cup: 0.29g ±0.
Table 2: Rate of reaction produced by different concentrations of HCL acid.
5 different concentration of HCL used (Mol) ±0.5 Volume of Co2 Gas produced in 1 minute (ml) ±0.5 Rate of Reaction (ml/s)
0.25 8.00 0.13
0.50 21.50 0.36
1.00 25.00 0.42
1.50 28.00 0.47
2.00 31.00 0.52
Sample Calculations:
• In the experiment, the time was calculated by using a stopwatch with an uncertainty of ±0.1sec.
• The volume of HCL acid was calculated through measuring cylinder with an uncertainty of ±0.5ml.
• Rate of reaction: Volume of CO2 gas produced in 1 minute/60sec
Example: For 0.25mol concentration of HCL acid, the volume of Co2 gas produced in one minute was= …show more content…
From the graph, we can see that the gradient of the concentration of 2.0mol of HCL acid is the steepest. While, the gradient of the concentration of 0.25mol is the lowest.
Conclusion:
From the data tables and graph, we can conclude that as the concentration increases, the rate of reaction also increases. This is because as the concentration is increased, the number of particles or atoms in the same volume is also increases. Due to that, the chances of collisions between the atoms or particles also increases and thus, the rate of reaction.