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Byju's Answer

Standard XII

Chemistry

Characteristics of Equilibrium Constant

If different ...

Question

If different quantities of ethanol and acetic acid are used in the following reversible reaction,
${C H}_{3} C O O H (l) + C_{2} H_{5} O H (l) ⇌ {C H}_{3} C O O C_{2} H_{5} (l) + H_{2} O (l)$ , the equilibrium constant will have values which will be:

different in all cases

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same in all cases

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higher in cases where higher concentration of ethanol is used

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higher in cases where higher concentration of acetic acid is used

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Solution

The correct option is B same in all cases
The value of equilibrium constant does not depend on the initial concentration of reactants. It depends only on the nature of reactants and the temperature of the reaction. So the value of it is the same in all cases.

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Similar questions

Q. The equilibrium constant for the reaction,

{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)

4

. What will be the composition of the equilibrium mixture when

1

mole of acetic acid is taken along with

4

moles of ethyl alcohol?

Q. When

3 m o l e s

of ethyl alcohol are mixed with

3 m o l e s

of acetic acid,

2 m o l e s

of ester are formed at equilibrium according to the equation:

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)

The value of the equilibrium constant for the reaction is:

Q. When alcohol

(C_{2} H_{5} O H (l))

and acetic acid

(C H_{3} C O O H (l))

are mixed together in equimolar ratio at

27^{o}

C. 33% of each is converted into ester. Then the

K_{c}

for the equilibrium

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

is:

Q. If different quantities of ethyl alcohol and acetic acid are used in the reversible reaction

C H_{3} C O O H + C_{2} H_{5} O H \Leftrightarrow C H_{3} C O O C_{2} H_{5} + H_{2} O

then the equilibrium constant will have the values:

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?

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If different quantities of ethanol and acetic acid are used in the following reversible reaction,CH3COOH(l)+C2H5OH(l)⇌CH3COOC2H5(l)+H2O(l), the equilibrium constant will have values which will be:

The correct option is B same in all casesThe value of equilibrium constant does not depend on the initial concentration of reactants. It depends only on the nature of reactants and the temperature of the reaction. So the value of it is the same in all cases.

If different quantities of ethanol and acetic acid are used in the following reversible reaction,
${C H}_{3} C O O H (l) + C_{2} H_{5} O H (l) ⇌ {C H}_{3} C O O C_{2} H_{5} (l) + H_{2} O (l)$ , the equilibrium constant will have values which will be:

The correct option is B same in all cases
The value of equilibrium constant does not depend on the initial concentration of reactants. It depends only on the nature of reactants and the temperature of the reaction. So the value of it is the same in all cases.