VirtualLab_EsterEquilInvestigation

VirtualLab_EsterEquilInvestigation - Questions : 1. What...

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Investigating an Esterification Equilibrium Background Consider the following equilibrium: C 2 H 5 OH ( l ) + CH 3 COOH ( l ) CH 3 COOC 2 H 5( l ) + H 2 O ( l ) H = -3.5 kJ/mol K c = [ CH 3 COOC 2 H 5( l ) ][ H 2 O ( l ) ] [ C 2 H 5 OH ( l ) ][ CH 3 COOH ( l ) ] You can use the spreadsheet Ester_equ.xls to investigate: a. The change in amounts of reactants and products as the system comes to equilibrium. b. The effect on K c as the system comes to equilibrium. c. The rate at which equilibrium is reached. Variables include: a. The concentrations of reactants and products. b. The value of K c . c. A rate factor, which simulates the addition or removal of a catalyst. Set K c at 6, and the rate factor at 0.004 before you begin the activities. Activity 1 Set the Initial Concentrations of the reactants (ethanol and entanoic acid) at 1.75 and the products (ethyl ethanoate and water) at 0.25. Reverse these values for the Changed concentrations.
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Unformatted text preview: Questions : 1. What property of an equilibrium does this demonstrate? 2. Why are the equilibrium concentrations of the reactants, and the equilibrium concentrations of the products, the same? Activity 2 Reduce the initial concentration of the ethanoic acid. Question : 1. You will note that the difference in the initial and equilibrium concentrations of ethanoic acid and ethanol are the same. Why? Activity 3 Reduce the initial concentration of the ethanoic acid. Questions : 1. Which way does the position of the equilibrium move? 2. Is the reduction of the K c value equivalent to a reduction or an increase in temperature? Activity 4 Reduce the rate factor to its lowest value. This is equivalent of omitting the acid catalyst. Question : 1. What is the effect of this on the reaction?...
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