The ester, ethyl acetate is formed by the reaction between ethanol and acetic acid and their equilibrium is represented as:

$C H_{3} COO H_{(l)} + C_{2} H_{5} O H_{(l)} ⇌ C H_{3} COO C_{2} H_{5 (a q)} + H_{2} O_{(l)}$

(a) Write the concentration ratio (reaction quotient), $Q_{e}$ , for this reaction. Note that water is not in excess and is not a solvent in this reaction.

(b) At $293 K$ , if one starts with $1.00$ mole of acetic acid and $0.180$ mole of ethanol, there is $0.171$ mole of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant.

(c) Starting with $0.500$ mole of ethanol and $1.000$ mole of acetic acid and maintaining it at $293 K$ , $0.214$ mole of ethyl acetate is found after some time. Has equilibrium been reached?

Question

The ester, ethyl acetate is formed by the reaction between ethanol and acetic acid and their equilibrium is represented as:

C H_{3} COO H_{(l)} + C_{2} H_{5} O H_{(l)} ⇌ C H_{3} COO C_{2} H_{5 (a q)} + H_{2} O_{(l)}

(a) Write the concentration ratio (reaction quotient),

Q_{e}

, for this reaction. Note that water is not in excess and is not a solvent in this reaction.

(b) At

293 K

, if one starts with

1.00

mole of acetic acid and

0.180

mole of ethanol, there is

0.171

mole of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant.

(c) Starting with

0.500

mole of ethanol and

1.000

mole of acetic acid and maintaining it at

293 K

,

0.214

mole of ethyl acetate is found after some time. Has equilibrium been reached?

Filo · Accepted Answer

(i) The concentration ratio is Qc​=[CH3​COOH][C2​H5​OH][CH3​COOC2​H5​][H2​O]​(ii) The initial concentrations are[CH3​COOH]=1.00[C2​H5​OH]=0.18[CH3​COC2​H4​]=0[H2​O]=0The equilibrium concentrations are:[CH3​COOH]=V1−0.171​=V0.829​[C2​H5​OH]=V0.18−0.171​=V0.009​[CH3​COC2​H4​]= V0.171​[H2​O]= V0.171​The equilibrium constant expression is Kc​=[CH3​COOH][C2​H5​OH][CH3​COOC2​H5​][H2​O]​=V0.829​ ×V0.009​V0.171​×V0.171​​=3.92(iii) The initial concentrations are:[CH3​COOH]=1.00[C2​H5​OH]=0.500[CH3​COC2​H4​]=0[H2​O]=0The equilibrium concentrations are:[CH3​COOH]=V1−0.214​=V0.786​[C2​H5​OH]=V0.500−0.214​=V0.286​[CH3​COC2​H4​]= V0.214​[H2​O]= V0.214​The expression for the reaction quotient is: Qc​=[CH3​COOH][C2​H5​OH][CH3​COOC2​H5​][H2​O]​=V0.786​ ×V0.286​V0.214​×V0.214​​=0.204As the value of the reaction quotient is not equal to the value of the equilibrium constant, the equilibrium is not yet achieved.

Question Text	The ester, ethyl acetate is formed by the reaction between ethanol and acetic acid and their equilibrium is represented as: $C H_{3} COO H_{(l)} + C_{2} H_{5} O H_{(l)} ⇌ C H_{3} COO C_{2} H_{5 (a q)} + H_{2} O_{(l)}$ (a) Write the concentration ratio (reaction quotient), $Q_{e}$ , for this reaction. Note that water is not in excess and is not a solvent in this reaction. (b) At $293 K$ , if one starts with $1.00$ mole of acetic acid and $0.180$ mole of ethanol, there is $0.171$ mole of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant. (c) Starting with $0.500$ mole of ethanol and $1.000$ mole of acetic acid and maintaining it at $293 K$ , $0.214$ mole of ethyl acetate is found after some time. Has equilibrium been reached?
Answer Type	Text solution:1
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Text solutionVerified

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