The alkaline hydrolysis of ethyl acetate is represented by the equation- CH3 COOC2H5 - NaOH - CH3COONa - C2H5OH Experimentally it is found that for this reaction- dxdt - k-CH3COOC2H5-NaOH- Then the reaction is

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

State (Phase) of Alkanes

The alkaline ...

Question

The alkaline hydrolysis of ethyl acetate is represented by the equation:

$C H_{3} C O O C_{2} H_{5} + N a O H \to C H_{3} C O O N a + C_{2} H_{5} O H$

Experimentally it is found that for this reaction:

$\frac{d x}{d t} = k [C H_{3} C O O C_{2} H_{5}] [N a O H]$

Then the reaction is

Bimolecular and of first order

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Bimolecular and of second order

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Pseudo-bimolecular

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Pseudo—unimolecular

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is D Bimolecular and of second order
Since 2 reactants are involved, the reaction is $b i m o l e c u l a r .$
Also, as can be seen from the experimental analysis, the order of the reaction is $t w o$ .
hence option (B) is correct.

Suggest Corrections

Similar questions

Q. The reaction,

C H_{3} C O O C_{2} H_{5} + N a O H \to C H_{3} C O O N a + C_{2} H_{5} O H

is:

C H_{3} C O O C_{2} H_{5} + N a O H \to C H_{3} C O O N a + C_{2} H_{5} O H

Rate

= K [C H_{3} C O O C_{2} H_{5}] [N a O H]

If three times water is added to the reaction mixture, the rate of the reaction compared to the original rate will be:

Ethyl acetate is formed by the reaction between ethanol and acetic acid and the

equilibrium is represented as:

(i) Write the concentration ratio (reaction quotient), Qc, for this reaction (note: water is not in excess and is not a solvent in this reaction)

(ii) At 293 K, if one starts with 1.00 mol of acetic acid and 0.18 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant.

(iii) Starting with 0.5 mol of ethanol and 1.0 mol of acetic acid and maintaining it at 293 K, 0.214 mol of ethyl acetate is found after sometime. Has equilibrium been reached?

Q. The rate of the reaction:

C H_{3} C O O C_{2} H_{5} + N a O H \to C H_{3} C O O N a + C_{2} H_{5} O H

is given by the equation,

r a t e = k [C H_{3} C O O C_{2} H_{5}] [N a O H]

If concentration is expressed in

m o l / L

, the units of

k

are:

Q. The hydrolysis of ethyl acetate,

C H_{3} C O O C_{2} H_{5} + H_{2} O H^{+} - - \to C H_{3} C O O H + C_{2} H_{5} O H

is a reaction of:

Join BYJU'S Learning Program

The alkaline hydrolysis of ethyl acetate is represented by the equation: CH3COOC2H5+NaOH→CH3COONa+C2H5OH Experimentally it is found that for this reaction: dxdt=k[CH3COOC2H5][NaOH] Then the reaction is

The correct option is D Bimolecular and of second orderSince 2 reactants are involved, the reaction is bimolecular.Also, as can be seen from the experimental analysis, the order of the reaction is two.hence option (B) is correct.

The alkaline hydrolysis of ethyl acetate is represented by the equation:

$C H_{3} C O O C_{2} H_{5} + N a O H \to C H_{3} C O O N a + C_{2} H_{5} O H$

Experimentally it is found that for this reaction:

$\frac{d x}{d t} = k [C H_{3} C O O C_{2} H_{5}] [N a O H]$

Then the reaction is

The correct option is D Bimolecular and of second order
Since 2 reactants are involved, the reaction is $b i m o l e c u l a r .$
Also, as can be seen from the experimental analysis, the order of the reaction is $t w o$ .
hence option (B) is correct.