# Chemistry

posted by .

Find the equilibrium moles for the following reaction with initially 0.051 mol for Ethyl acetate, 0.260 mol for water and 0.03045 mol of acetic acid at equilibrium.

I'm not sure how to get the ones at equilibrium for the left side or even how much you have to take away for the reaction.

CH3CH2COOCH3 + H2O ---> CH3CH2OH + CH3COOH

initial:
EthylAc: 0.051 mol
Water: 0.260 mol
EthylOH: --------
Acetic: --------

rxn:
EthylAc:
Water:
EthylOH:
Acetic:

eq:
EthylAc: ?
Water: ?
EthylOH: ?
Acetic: 0.03045 mol

Thank you

• Chemistry -

does it mean that because acetic acid has 0.03045 mol at equilibrium that x = 0.03045 mol? So then Ethanol would also have 0.03045 mol at eq and EtAc and H20 would both be their initial [conc] - x?

• Chemistry -

because it's a 1:1 ratio for all, then at rxn, we would have -x for both EtAc and H2O and + x on the right, so x = 0.03045.
Is this correct?

• Chemistry -

You have run your sentence together and I can't be sure about the concentrations. From the table, however, it appears initially you have EtOAc of 0.051 and H2O of 0.260 (so initially EtOH = 0 and acetic acid = 0).
Yes, if you have 0.03045 mols acetic acid at equilibrium you will have 0.03045 mols EtOH at equilibrium.
.......EtOAc + H2O ==> EtOH + HAc
I......0.051..0.260.....0......0
C.......-x.....-x.......x.......x
E.....0.051-x.0.260-x...x......x
So = 0.03045 which allows you to place numbers for all and calculate Keq.(at least I suppose that is what you are to do).

• Chemistry -

okay thanks Dr.Bob, that's exactly what I did too.

## Respond to this Question

 First Name School Subject Your Answer

## Similar Questions

1. ### chem

The equilibrium constant Kc equals 5.90 for the reaction CH3COOH + C2H5OH <==> CH3COOC2H5 + H2O Find the molar concentrations of acetic acid, ethanol, ethyl acetate, and water at equilibrium when .10 M acetic acid and .20 M ethanol …
2. ### chemistry

In an esterification experiment, 2.0 mol of ethanol were mixed with 1.0 mol of ethanoic acid in a container of volume 30cm3 and the chemicals were allowed to come to equilibrium at 25°, CH3CO2H + C2HOH <-> CH3COOC2H5 + H20 If …
3. ### chemistry

A classic experiment in equilibrium studies dating from 1862 involved the reaction in solution of ethanol and acetic acid to produce ethyl acetate and water. The reaction can be followed by analyzing the equilibrium mixture for its …
4. ### chemistry

n one experiment, a mixture of 1.000 mol acetic acid and 0.5000 mol ethanol is brought to equilibrium. A sample containing exactly one-hundredth of the equilibrium mixture requires 28.80mL 0.1040M Ba(OH)2 for its titration. Calculate …
5. ### AP Chemistry

The equilibrium constant for thermal dissociation of F2 F2(g)<->2F(g) is 0.300. If initially 1.00 mol F2 is placed in a 1.00 L container, which of the following is the correct number of moles of F2 that have dissociated at equilibrium?
6. ### Chemistry

An equilibrium mixture in a 10.0 L flask contains 7.0 mol HI(g) and 1.0 mol each of I2(g) and H2(g). If 2.5 mol H2, 5.0 mol I2 and 2.0 mol HI are added to that equilibrium mixture how many moles of each gas will be present when equilibrium …
7. ### Chemistry

Consider the reaction HCHO(g) *) H2(g) + CO(g). 1.0 mol of HCHO, 1.0 mol of H2 and 1.0 mol of CO exist in equilibrium in a 2.0 L reaction vessel at 600C. a) Determine the value of the equilibrium constant Kc for this system. 2.0 moles …
8. ### Chemistry

At a certain temperature, 0.885 mol of N2, and 2.654 mol of H2 are placed in a container. N2+3H2=2NH3 At equilibrium, there is 0.823 mol of NH3 present. Determine the number of mol of N2 and H2 that are present when the reaction is …
9. ### Chem

At a certain temperature, 0.885 mol of N2, and 2.654 mol of H2 are placed in a container. N2+3H2=2NH3 At equilibrium, there is 0.823 mol of NH3 present. Determine the number of mol of N2 and H2 that are present when the reaction is …
10. ### Chemistry

When 0.20 mol of hydrogen gas and 0.15 mol of iodine gas are heated at 723 K until equilibrium is established, the equilibrium mixture is found to contain 0.26 mol of hydrogen iodide. The equation for the reaction is as follows. H2(g) …

More Similar Questions