The equation is given for both questions :
CH3COOH + C2H5OH <--> CH3CO2C2H5 + H2O
Question 1:
In an experiment to determine Kc, 1.00 mol of ethanoic acid was allowed to reach equilibrium with 1.00 mol of ethanol in the presence of 0.100mol of H+ dissolved in 1.00mol of water. It forms an homogeneous mixture. At equilibrium, it was found that 0.43 mol of ethanoic acid was present. How many moles of water are present at equilibruim ?
In this case, does it mean that the initial number of mole of water is 1.0 mol ?
Why the question gives me the number of mole of hydrogen ion ?
I'm not sure with that, can anyone tell me that ?
Question 2:
A mixture of 6.0g of ethanoic acid and 6.0g of ethanol was added to 4.4g of ethyl ethanoate and the overall mixture allowed to reach equilibrium. It was found that 0.040mol of ethanoic acid was present in the equilibrium mixture.
This is my analysis for the number of moles of the chemicals
CH3COOH
Initial number of mole (n) : 0.1
At equilibrium (eq) : 0.04
C2H5OH
n : 0.13
eq : 0.07
CH3COOC2H5
n : 0.05
eq : 0.11
H2O
n : 0
eq : 0.06
Correct me please if I'm wrong .
I want to know whether my analysis is wrong or not. Thanks