4. In the production of an ester the following equilibrium is established at 304 K: CH3CH2OH) + CH3CO2H = CH3CO2CH2CH3 + H2O 1.2 moles of ethanol is added 1.4 moles of ethanoic acid at 294 K in the presence of sulphuric acid and allowed to reach equilibrium. At equilibrium there was found to be 0.7 moles of ethylethanoate. a. Write an expression for Ke for this reaction. b. Use this information above to determine the value of Ke at this temperature. What does this tell you about the position of equilibrium? c. The experiment is the repeated at a different temperature and the following equilibrium concentrations were recorded: CH3CO2CH2CH311) H2O) Moles at equilibrium CH3CH2OH() 0.025 CH3CO2HD 0.025 0.015 0.015 Determine Ke of the reaction at this new temperature. d. Given that the equilibrium described above is exothermic: i. Identify and explain how you would expect K to change if an additional 0.002 moles of CH-CH2OH were added to the reaction mixture ii. Identify and explain how you would expect K to change if temperature of the system was changed to 334 K 4.1