How Does The Change In Hcl Concentration Affect The Rate Of Reaction
Interpretation of Data
When looking at my results i can safely say that the change in HCl concentration does affect the rate of reaction with the Calcium carbonate pebbles. The relationship between the change in HCl and reaction rate can be seen in the graph and raw data table presented above. If you compare the lowest concentration with the highest concentration you'd be able to see that there is a very large contrast between their averages. The average gas production of 0.1M HCl was 0.00693 kPa/s whereas the average gas production for 1M HCl was 0.257. This clearly indicates that when the reactant consists of a higher molarity the reaction is much faster. As i mentioned before, collision theory is the explanation for why this happens. An increase in reactant causes the reactants particles to bundle up and cause a fruitful collision much faster than particles that would flow loosely around each other, which would be the case for an experiment using HCl with a low molarity. Another thing that can be noticed about the relationship is that it's linear. As the concentration goes up, the reaction rate goes up as well, therefore creating a linear relationship. The difference between …show more content…
By the looks of the graph i believe that my hypothesis was quite correct in the sense that a higher concentration of HCl would cause a faster reaction. The fact that the graph shows us that 1M of HCl produces around 0.25 kPa/s and that 0.5M of HCl produces around 0.15kPa/s of CO2 justifies collision theory, as well as my hypothesis (which was based entirely off of collision theory. The same evidence to support my hypothesis can be seen with the concentrations 0.1 and 0.2 regardless of the small difference. My hypothesis in the B report also mentioned that each concentration would eventually produce the same amount of CO2 although just at different paces, the graph also demonstrates
When looking at my results i can safely say that the change in HCl concentration does affect the rate of reaction with the Calcium carbonate pebbles. The relationship between the change in HCl and reaction rate can be seen in the graph and raw data table presented above. If you compare the lowest concentration with the highest concentration you'd be able to see that there is a very large contrast between their averages. The average gas production of 0.1M HCl was 0.00693 kPa/s whereas the average gas production for 1M HCl was 0.257. This clearly indicates that when the reactant consists of a higher molarity the reaction is much faster. As i mentioned before, collision theory is the explanation for why this happens. An increase in reactant causes the reactants particles to bundle up and cause a fruitful collision much faster than particles that would flow loosely around each other, which would be the case for an experiment using HCl with a low molarity. Another thing that can be noticed about the relationship is that it's linear. As the concentration goes up, the reaction rate goes up as well, therefore creating a linear relationship. The difference between …show more content…
By the looks of the graph i believe that my hypothesis was quite correct in the sense that a higher concentration of HCl would cause a faster reaction. The fact that the graph shows us that 1M of HCl produces around 0.25 kPa/s and that 0.5M of HCl produces around 0.15kPa/s of CO2 justifies collision theory, as well as my hypothesis (which was based entirely off of collision theory. The same evidence to support my hypothesis can be seen with the concentrations 0.1 and 0.2 regardless of the small difference. My hypothesis in the B report also mentioned that each concentration would eventually produce the same amount of CO2 although just at different paces, the graph also demonstrates