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Standard XII

Chemistry

CH_3COOH(l) ...

Question

$C H_{3} C O O H (l) + C_{2} H_{5} O H (l) ⇌ C H_{3} C O O C_{2} H_{5} (l) + H_{2} O (l)$

In the above reaction, one mole of each of acetic acid and alcohol are heated in the presence of

little conc. $H_{2} S O_{4}$ . On equilibrium being attained

1 mole of ethyl acetate is formed

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2 mole of ethyl acetate are formed

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1/2 moles of ethyl acetate is formed

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2/3 moles of ethyl acetate is formed

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Solution

The correct option is D
2/3 moles of ethyl acetate is formed

In presence of little $H_{2} S O_{4}$ (as catalyst) about $\frac{2}{3} m o l e$ of each of

$C H_{3} C O O H$ and $C_{2} H_{5} O H$ react to form $\frac{2}{3} m o l e$ of the product at

equilibrium.

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Similar questions

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

C H_{3} C O O H_{(l)} + C_{2} H_{5} O H_{(l)} ⇌ C H_{3} C O O 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.

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?

$C H_{3} C O O H (l) + C_{2} H_{5} O H (l) ⇌ C H_{3} C O O C_{2} H_{5} (l) + H_{2} O (l); K_{c} = 4$

In the above reaction, one mole of each of acetic acid and alcohol are heated in the presence of little conc. $H_{2} S O_{4}$ . On equilibrium being attained

$C H_{3} C O O H (l) + C_{2} H_{5} O H (l) ⇌ C H_{3} C O O C_{2} H_{5} (l) + H_{2} O (l)$

In the above reaction, one mole of each of acetic acid and alcohol are heated in the presence of

little conc. $H_{2} S O_{4}$ . On equilibrium being attained

1.0

mole of ethyl alcohol and

1.0

mole of acetic acid are mixed. At equilibrium,

0.666

mole of ester is formed. The value of equilibrium constant is:

1.0 m o l e

of ethyl alcohol and

1.0 m o l e

of acetic acid are mixed. At equilibrium,

0.666 m o l e

of ester is formed. The value of equilibrium constant is:

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Standard XII Chemistry

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CH3COOH(l) + C2H5OH(l) ⇌ CH3COOC2H5(l) + H2O(l) In the above reaction, one mole of each of acetic acid and alcohol are heated in the presence of little conc. H2SO4. On equilibrium being attained

The correct option is D 2/3 moles of ethyl acetate is formed In presence of little H2SO4 (as catalyst) about 23 mole of each of CH3COOH and C2H5OH react to form 23 mole of the product at equilibrium.

$C H_{3} C O O H (l) + C_{2} H_{5} O H (l) ⇌ C H_{3} C O O C_{2} H_{5} (l) + H_{2} O (l)$

In the above reaction, one mole of each of acetic acid and alcohol are heated in the presence of

little conc. $H_{2} S O_{4}$ . On equilibrium being attained

The correct option is D
2/3 moles of ethyl acetate is formed

In presence of little $H_{2} S O_{4}$ (as catalyst) about $\frac{2}{3} m o l e$ of each of

$C H_{3} C O O H$ and $C_{2} H_{5} O H$ react to form $\frac{2}{3} m o l e$ of the product at

equilibrium.