Question

One litre of 2M acetic acid and one litre of
3M ethyl alcohol were mixed. The
esterification takes place according to the
reaction:
CH,COOH + C,H,OH - CH,COOCH
+ H₂O
If each solution is diluted by one litre water
the rate would become -
(A) 4 times
(B) 2 times
(C) 0.5 times
(D) 0.25 times​

Answer 1

Answer:

option D is correct

mole of $CH_{3} COOH$=Molarity*volume

                                                    =2M*1L

                                                    =2mole

final molarity after dilution=$\frac{mole}{Total volume}$

Molarity of acetic acid after dilution=$\frac{2mole}{2L}=1M$

molarity of ethyl alcohol=3M*1L=3mole

final molarity of ethyl alcohol=1.5M

on solving the equations we get

$\frac{r_{1} }{r_{2} } =2*2$

$r_{1} =4r_{2}$

$r_{2} =\frac{r_{1} }{4} =0.25r_{1}$

so it is 0.25 times high

Answer 2

Explanation:

*Hope its clear to all*