Chemical Equilibrium
EXPERIMENT NO. 9 CHEMICAL EQUILIBRIUM
Audrey De Castro FCD3, Group 9, Ms. Sarah Sibug
Kristine Tavares March 27, 2014
I. ABSTRACT
Chemical equilibrium is mostly involved in industrial processes such as synthesis of ammonia gas, formation of sulfuric acid and methanol. It is also behind some of the natural phenomena like lime production from limestone. (Application of Chemical, n.d.)
In experiment 9, the response of a system in chemical equilibrium to disturbances or changes was observed. The objectives of the experiment was to evaluate how changes in concentration and temperature affect the equilibrium system, explain and interpret the results based on Le Chatelier’s principle.
The shifts in the position of the equilibrium were induced by the change in concentration and temperature. In changing the concentration, different reagents were added to a solution at equilibrium state. In changing the temperature, a solution inside a test tube was heated while another one was cooled. The changes in color of the solution indicated that a shift in the equilibrium occurred.
II. KEYWORDS: Chemical equilibrium, Le Chatelier’s Principle, dissociation, common ion effect, uncommon ion effect, shift
III. INTRODUCTION
Chemical equilibrium is reached when opposing reactions- forward and reverse reactions- occur at the same rate. This means that the rate at which the reaction forms the products is equal to the rate at which the reaction forms the reactants (Lemay et al, 2012). In this dynamic state, there is continuous formation of reactant and products (Committee on General Chemistry, 2012, p. 76). This principle is
Audrey De Castro FCD3, Group 9, Ms. Sarah Sibug
Kristine Tavares March 27, 2014
I. ABSTRACT
Chemical equilibrium is mostly involved in industrial processes such as synthesis of ammonia gas, formation of sulfuric acid and methanol. It is also behind some of the natural phenomena like lime production from limestone. (Application of Chemical, n.d.)
In experiment 9, the response of a system in chemical equilibrium to disturbances or changes was observed. The objectives of the experiment was to evaluate how changes in concentration and temperature affect the equilibrium system, explain and interpret the results based on Le Chatelier’s principle.
The shifts in the position of the equilibrium were induced by the change in concentration and temperature. In changing the concentration, different reagents were added to a solution at equilibrium state. In changing the temperature, a solution inside a test tube was heated while another one was cooled. The changes in color of the solution indicated that a shift in the equilibrium occurred.
II. KEYWORDS: Chemical equilibrium, Le Chatelier’s Principle, dissociation, common ion effect, uncommon ion effect, shift
III. INTRODUCTION
Chemical equilibrium is reached when opposing reactions- forward and reverse reactions- occur at the same rate. This means that the rate at which the reaction forms the products is equal to the rate at which the reaction forms the reactants (Lemay et al, 2012). In this dynamic state, there is continuous formation of reactant and products (Committee on General Chemistry, 2012, p. 76). This principle is
References: Brown, P. (2013). Theoretical physical advanced level chemistry -equilibria - chemical equilibrium Retrieved March 25, 2014, from http://www.docbrown.info/page07/equilibria3.htm Brown, T. L., Lemay, E. H. et al. (2012). Chemistry: The Central Science. USA: Pearson Education, Inc. Committee on General Chemistry. (2012).Laboratory manual in general chemistry 1.Philippines: University of the Philippines Manila.