1.25 mole of ethanol and 1.85 mole of acetic acid are dissolved in water and kept at 100 degree C. The volume of the solution is 250.0 ml. At equilibrium, 0.25 mole of acetic acid has been consumed in producing ethyl acetate. Calculate Kc at 100 degree C for the reaction.
2. 1.25 mole of ethanol and 1.85 mole of acetic acid are dissolved in water and kept at 100°C. The volume of the solution is 250.0 mL. At equilibrium, 0.25 mole of acetic acid has been consumed in producing ethyl acetate. Calculate Ke at 100°C for the reaction ethanol acetic acid ethyl acetate
How many moles of ethyl acetate are present in an equilibrium mixture that contains 3.7 mol of acetic acid, 6.4 mol of ethanol, and 12.5 mol of water at 25 âC?
Part B
Calculate the number of moles of all reactants and products in an equilibrium mixture prepared by mixing 1.00 mol of acetic acid and 10.00 mol of ethanol.
Calculate the number of moles of all reactants and products in an equilibrium mixture prepared by mixing 1.00 mol of acetic acid and 10.00 mol of ethanol.
