The Equilibrium Constant Of An Ester Hydrolysis Reaction
The Equilibrium Constant of an Ester Hydrolysis Reaction
Julia Stanley
CHM 152 LL
Dr. Asmita Kane Budruk
Goal of the lab:
The purpose of this laboratory is to determine the equilibrium constant, Kc, for the acid-catalyzed reaction between an unknown ester and water to produce an unknown alcohol and an unknown carboxylic acid. I was using Unknown Ester #3 with a density of 0.9342 and Molar Mass of 74.08 g/mol; alcohol with density 0.7914 and Molar Mass 32.04 g/mol.
Chemical principle or theory involved:
I used chapter 14, part 14.1 The Concept of Equilibrium and the Equilibrium Constant. Equilibrium is a state of balance in a chemical reaction in which the forward and backward rates are equal.
For the reaction below, when A and B were mixed, the reaction proceeds in the forward direction to produce C and D. However, as time progresses, the concentration of C and D increases causing an increase in the rate of the reverse reaction. Concurrent with this increased rate of the reverse reaction is a reduction of the forward rate due to the decrease in the concentration of A and B. At some point, the rate of the forward and reverse reactions will become the same and we will reach a state of dynamic equilibrium: aA + bB cC + dD (1)
For a general equilibrium equation we can specify an equilibrium constant, Kc, that relates the concentrations of all product and reactant species, (2) where [A], [B], [C], and [D] are the molar concentration of all species present at equilibrium. The exponents, a, b, c, and d represent the stoichiometry coefficients from the balance chemical reaction. Kc is really the ratio of the rate of the reverse reaction divided by the rate of the forward reaction and so is a dimensionless constant at a given temperature. Additionally, functional groups are important for this experiment. Functional group: A group of atoms whose bonding is the same from molecule to molecule. A functional group has
Julia Stanley
CHM 152 LL
Dr. Asmita Kane Budruk
Goal of the lab:
The purpose of this laboratory is to determine the equilibrium constant, Kc, for the acid-catalyzed reaction between an unknown ester and water to produce an unknown alcohol and an unknown carboxylic acid. I was using Unknown Ester #3 with a density of 0.9342 and Molar Mass of 74.08 g/mol; alcohol with density 0.7914 and Molar Mass 32.04 g/mol.
Chemical principle or theory involved:
I used chapter 14, part 14.1 The Concept of Equilibrium and the Equilibrium Constant. Equilibrium is a state of balance in a chemical reaction in which the forward and backward rates are equal.
For the reaction below, when A and B were mixed, the reaction proceeds in the forward direction to produce C and D. However, as time progresses, the concentration of C and D increases causing an increase in the rate of the reverse reaction. Concurrent with this increased rate of the reverse reaction is a reduction of the forward rate due to the decrease in the concentration of A and B. At some point, the rate of the forward and reverse reactions will become the same and we will reach a state of dynamic equilibrium: aA + bB cC + dD (1)
For a general equilibrium equation we can specify an equilibrium constant, Kc, that relates the concentrations of all product and reactant species, (2) where [A], [B], [C], and [D] are the molar concentration of all species present at equilibrium. The exponents, a, b, c, and d represent the stoichiometry coefficients from the balance chemical reaction. Kc is really the ratio of the rate of the reverse reaction divided by the rate of the forward reaction and so is a dimensionless constant at a given temperature. Additionally, functional groups are important for this experiment. Functional group: A group of atoms whose bonding is the same from molecule to molecule. A functional group has