Calorimetry Lab Conclusion

Conclusion
Observing the graph above, I can conclude that the higher the concentration of hydrochloric acid (in molars) the faster the rate of reaction it has with calcium carbonate. I can see this because on my graph the higher the concentration the higher the line goes on the graph. An example, 1.0 molar concentration is above 0.5 molar but it is below 2.0 molar at the 60-second line. Therefore it has a faster rate of reaction then 0.5 molar but a slower rate of reaction that 1.5 molar.
The results were what I expected although some anomalies did occur and are highlighted (outliers) in the tables and on graphs, however these did not affect any of the results and were probably only misreading as there were never more than one for the same

Factors that might have influenced the results may include the force applied to shake the flask during the procedure, or the fact that not every time when the calcium carbonate powder was measured it was only measured it to the approximate amount rather than the precise amount etc... One of the biggest faults in my experiment was the fact that I did not have enough time to complete it in one day. Due to various problems, I had to do the experiment on two different days. This means that all the equipment was different which may mean that they work differently from each other. This makes it an unfair test. The second problem with doing it on different days is the problem of room temperature which can have a big effect on the rate, because as I know from back ground knowledge, I know the warmer the acid is, the faster the reaction because particles have more energy so there are more successful collisions. I made the mistake of not recording which results are from which day, so I cannot tell if this had a major effect on the