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13 Dec 2019

Ethyl acetate, a solvent used in many fingernail-polish removers, is made by the reaction of acetic acid with ethanol: CH3CO2H(soln)Aceticacid +C2H5OH(soln)Ethanol⇌CH3CO2H(soln)Ethylacetate+H2O(soln)ΔH∘=−2.9kJ

Part A

Does the amount of ethyl acetate in an equilibrium mixture increase or decrease when the temperature is increased? Does the amount of ethyl acetate in an equilibrium mixture increase or decrease when the temperature is increased?

increase

decrease

Part B

How does Kc change when the temperature is decreased? Justify your answers using Le Chatelier's principle.

1- As the temperature is decreased, the reaction shifts from left to right. The product concentrations increase, and the reactant concentrations decrease. This corresponds to an increase in Kc.

2- As the temperature is decreased, the reaction shifts from right to left. The product concentrations decrease, and the reactant concentrations increase. This corresponds to an decrease in Kc.

3-As there is neither products no reactants in gas state the temperature does not shift the reaction. So decrease in temperature does not change Kc. SubmitMy AnswersGive Up

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Patrina Schowalter
Patrina SchowalterLv2
16 Dec 2019

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Related questions

The value of Kc for the reaction of acetic acid with ethanol is 3.4 at 25∘C:

CH3CO2H(soln)+ C2H5OH(soln)⇌ CH3CO2C2H5(soln)+H2O(soln)Kc=3.4
Acetic acid Ethanol Ethyl acetate

Part A

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 ∘C?

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.

Ok this is a three part questions but I think i correctly answered#1 but i get lost after that..

1. An aqueous solution of ethyl acetate at room temperature has aninitial concentration of 0.15 M. Calculate the equilibriumconcentrations of ethyl acetate (CH3COOC2H5), ethanol (C2H5OH) andacetic acid if the equilibrium constant at this temperature is Kc =3.00.
CH3COOC2H5(aq) + H2O ? CH3COOH(aq) + C2H5OH(aq)

Here I set up an ice table an ice table and got a quadratic ofx^2+3.00x-.45=0
and i got x=.143.

Now here is what I get confused..

2) 2. A solution contains 0.15 M acetic acid and 0.15 ethanol. Ifthe equilibrium constant defined by the reaction in Problem 1 is Kc= 3.00, calculate the equilibrium concentrations of ethyl acetate,acetic acid and ethanol.

Im guessing you just do products/reactants?
so
[0.15 M] x [0.15 M] / [CH3COOC2H5] = 3.00
and CH3COO2H5 = .0075 M.

I think im right up to this point then im not sure what to donext?

then there's

3. A solution contains 0.01 M ethyl acetate, 0.10 M acetic acid and0.10 M ethanol. For the same equilibrium constant of 3.00,calculate the equilibrium concentrations of ethyl acetate, ethanol,and acetic acid in the solution.

1) Consider the following equation: Rate = k [CH3I]2 [C15H11N]

i) If the concentration of C15H11N is doubled, does the rate constant:

A) Increase

B) Decrease

C) Remain unchanged

ii) If the concentration of of CH3I is decreased by a factor of 3, the time it takes for the reaction to finish will:

A) Increase by a factor of 3

B) Increase by a factor of 9

C) Decrease by a factor of 9

D) Remain Unchanged

iii) If the temperature increases how will the activation energy change:

A) It will increase

B) It will decrease

C) It will remain unchanged

2) During a titration of a weak acid with a strong base you add an additional small amount of base after reaching the equivalence point.

i) How does the pH of the solution change?

A) Increase

B) Decrease

C) Remain unchanged

ii) How does the Ka of the acid change?

A) Increase

B) Decrease

C) Remain unchanged

3) You combine a solution of silver nitrate (AgNO3) and a solution of sodium carbonate (Na2CO3) to form solid silver carbonate (Ag2CO3) and aqueous sodium nitrate (NaNO3), the net ionic equation is listed below. You observe the white solid, Ag2CO3 in the test tube. You add a strong acid (HNO3) to the mixture and it reacts with the carbonate ions as listed in the equations below. What would you expect to observe when adding the strong acid to the test tube?

2 Ag+(aq) + CO32-(aq) <--> Ag2CO3(s)

2 H+(aq) + CO32-(aq) <--> H2CO3

H2CO3 -> H2O(l) + CO2(g)

A) An increase in the amount of white solid

B) A color change of the solid

C) A decrease in the amount of white solid

D) No change in the amount of white solid

4) Ksp of BaF2 at room temperature is 1.84 x 10-7. It is also known that the reaction of dissolution of BaF2 is endothermic. Imagine that you have a saturated solution of BaF2 at equilibrium, that has some undissolved BaF2 precipitated on the bottom of the test tube.

4.1) If the temperature is increased how would that affect:

i) The solubility of BaF2

A) Increase

B) Decrease

C) Remain Unchanged

ii) The solubility constant of BaF2

A) Increase

B) Decrease

C) Remain unchanged

4.2 An additional amount of BaF2 was added to the solution how would that affect:

i) The solubility of BaF2

A) Increase

B) Decrease

C) Remain unchanged

ii) The solubility constant of BaF2

A) Increase

B) Decrease

C) Remain unchanged

4.3 If NaF is added to the solution how will it affect:

i) The solubility of BaF2

A) Increase

B) Decrease

C) Remain Unchanged

ii) The solubility constant of BaF2

A) Increase

B) Decrease

C) Remain unchanged

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