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This acid-base chemical reaction is given by the formula Ca CO3(s) 2HCl (aq) → Ca Cl2 (aq) CO2 (g) H2O (l).
The volume of carbon dioxide produced was measured using a measuring cylinder and a bee hive.
The acid-base reaction taking place in the conical flask produces carbon dioxide as a product which displaces the water in the measuring cylinder.
The controlled variables in this experiment include the volume of hydrochloric acid, the mass of the marble chips and environmental conditions.
30m L of hydrochloric acid was measured and reacted with the marble chips.
The volume of carbon dioxide produced is therefore measured by determining the volume of water displaced.
The concentration of the hydrochloric acid was varied throughout the experiment. In this experiment, 4g of marble chips reacted with 30m L of one molarity of hydrochloric acid to prove that concentration has strong correlation with reaction rate.
To prove this theory, this experiment was designed to demonstrate the influence of concentration over reaction rate by measuring the volume of carbon dioxide produced when five different molarities (0.5, 1.0, 1.5, 2.0 and 2.5) of hydrochloric acid measuring 30ml react with 4g of marble chips.
The reliability of the experiment was ensured by repeating the test six times with each molarity of hydrochloric acid.
The consistency of the volume of hydrochloric acid is therefore important to ensure the fairness of this test and so that the data generated at the conclusion of the experiment is accurate.
The equilibrium of the volume of hydrochloric acid was maintained by accurately measuring 30m L and by using a funnel to transfer the acid from a measuring cylinder to a conical flask.