The Effect of the Concentration of Sulphuric Acid on the Reaction Rate with Magnesium
The Effect of the Concentration of Sulphuric Acid on the Reaction Rate with Magnesium
Sarah Cain
SCH 4UB
Mr. Lankin
April 1, 2009
Introduction
The nature of the problem is to design an investigation that examines a variable affecting the reaction rate. In this experiment, magnesium will be reacted with different concentrations of sulphuric acid. The reaction is shown by the following chemical equation:
H2SO4 (l) + Mg (s) → MgSO4 (aq) + H2 (g)
This equation shows that when magnesium is combined with sulphuric acid, the magnesium dissolves in the acid to form an aqueous solution containing Mg (II) ion and hydrogen gas. Sulphuric acid (H2SO4) is a strong corrosive acid that is made from sulphur dioxide. It is commonly used in lab experiments and in the chemical industry (Faiers). Magnesium (Mg) is an alkaline earth metal which is solid at room temperature. When it reacts with an acid, it produces hydrogen gas and a salt. The hydrogen gas produced by this reaction is what will be measured in this investigation. The rate of reaction is defined as how fast a reaction takes place (Parry). There are certain factors which affect reaction rates, including the temperature of the reactants, the surface area of the reactants, the concentration of the reactants, and the presence of a catalyst. According to the collision theory, effective collisions between particles are needed in order for the reaction to take place (Neuss). By increasing the concentration of the solution, the number of effective collisions between the particles will also increase. This will produce more product (hydrogen gas). The concentration is the amount of substance contained within a given volume of a solution (Green & Damji 33). This is given as the number of moles of the substance in one cubic decimetre (equivalent to 1 litre). This can further be expressed in the following formula:
Concentration (mol· dm-3) = By increasing the
Sarah Cain
SCH 4UB
Mr. Lankin
April 1, 2009
Introduction
The nature of the problem is to design an investigation that examines a variable affecting the reaction rate. In this experiment, magnesium will be reacted with different concentrations of sulphuric acid. The reaction is shown by the following chemical equation:
H2SO4 (l) + Mg (s) → MgSO4 (aq) + H2 (g)
This equation shows that when magnesium is combined with sulphuric acid, the magnesium dissolves in the acid to form an aqueous solution containing Mg (II) ion and hydrogen gas. Sulphuric acid (H2SO4) is a strong corrosive acid that is made from sulphur dioxide. It is commonly used in lab experiments and in the chemical industry (Faiers). Magnesium (Mg) is an alkaline earth metal which is solid at room temperature. When it reacts with an acid, it produces hydrogen gas and a salt. The hydrogen gas produced by this reaction is what will be measured in this investigation. The rate of reaction is defined as how fast a reaction takes place (Parry). There are certain factors which affect reaction rates, including the temperature of the reactants, the surface area of the reactants, the concentration of the reactants, and the presence of a catalyst. According to the collision theory, effective collisions between particles are needed in order for the reaction to take place (Neuss). By increasing the concentration of the solution, the number of effective collisions between the particles will also increase. This will produce more product (hydrogen gas). The concentration is the amount of substance contained within a given volume of a solution (Green & Damji 33). This is given as the number of moles of the substance in one cubic decimetre (equivalent to 1 litre). This can further be expressed in the following formula:
Concentration (mol· dm-3) = By increasing the
Cited: Faiers, A. Kinetics. Mar. 2009. Chemistry in Perspective. Jan. 2008. . Green and Damji. Chemistry. Victoria: IBID Press, 2007. Neuss, Geoffrey. Chemistry for the IB Diploma: Study Guide. New York: Oxford University Press, 2007. Parry, R.. Chemistry Experimental Foundation. Boston: Prentice Hall College Div., 1982. ----------------------- Amount of solute (mol) Solution volume (dm3) Figure 1: Concentration of Solute